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Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 2 Behaviour of Gases offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 2 Question Answer – Behaviour of Gases

Very Short Answer Type Questions :

Question 1.
Why are gaseous molecules always in incessant motion?
Answer:
Because gaseous molecules have no mutual force of attraction.

Question 2.
What is the cause of pressure of a gas taken in a vessel?
Answer:
Gaseous molecules continuously strike against the walls of the container.

Question 3.
In which direction pressure exerted by a gas in vessel does vary, if at all?
Answer:
Equal in all direction.

Question 4.
What is the effect of supplying heat to a gas at constant volume ?
Answer:
Pressure of the gas increases.

Question 5.
What is the cause of temperature of gas ?
Answer:
Kinetic energy possessed by gaseous molecules.

Question 6.
What is the effect of withdrawal of heat from a gas at constant volume ?
Answer:
Temperature of the gas falls.

Question 7.
What are the two constant quantities in Boyle’s law ?
Answer:
Mass of the gas and temperature.

Question 8.
What is the temperature inCelsius scale corresponding to absolute zero?
Answer:
-273°C

Question 9.
What Is meant by ideal gases?
Answer:
Gases which obey Boyle’s law and Charle’s law at all pressure and temperature.

Question 10.
How does the volume of a gas change for each degree celsius rise of temperature at constant pressure?
Answer:
\(\frac{1}{273}\) of volume of the gas at 0°C increases.

Question 11.
What will happen when a gas-filled balloon heated?
Answer:
The balloon will burst as the supplied heat increases the volume of the gas inside the balloon.

Question 12.
What will be the volume of an ideal gas at absolute zero?
Answer:
The volume will be zero.

Question 13.
At what temperature speed of gas molecules becomes zero?
Answer:
At -273°C or 0 K speed of gas molecule becomes zero.

Question 14.
What are the constant quantities inCharle’s law?
Answer:
In Charle’s law, the constant quantities are mass of the gas and pressure.

Question 15.
What are the variable quantities inCharle’s law?
Answer:
In Charle’s law, the variable quantities are temperature and volume.

Question 16.
What are the variable quantities in Boyle’s law?
Answer:
In Boyle’s law the variable quantities are pressure and volume.

Question 17.
What is the freezing temperature of water in absolute scale?
Answer:
273 K

Question 18.
Give a mathematical expression of Boyle’s law.
Answer:
V × P= constant

Question 19.
Give a mathematical expression ofCharle’s law.
Answer:
[\(\frac{V}{T}\) = constant]

Question 20.
What is the SI unit of pressure?
Answer:
SI unit of pressure is Pascal.

Question 21.
How is atmospheric pressure determined ?
Answer:
Atmospheric pressure is determined by Barometer invented by Torricelli.

Question 22.
How is pressure of a gas determined ?
Answer:
The pressure of a gas is determined by Manometer.

Question 23.
What is absolute zero?
Answer:
The temperature at which the volume of a gas reduces to zero is called absolute zero.

Question 24.
IsCharle’s law applicable for liquids ?
Answer:
Charle’s law is not applicable for liquids.

Question 25.
Write the ideal gas equation for one gram-mole gas.
Answer:
PV = RT

Question 26.
What is the value of absolute temperature in Fahrenheit scale ?
Answer:
(-) 4594° F

Question 27.
What is the relation between absolute scale and celsius scale of temperature?
Answer:
If any temperature is t°C in celsius scale and if is TK in Kelvin scale then
T = t + 273

Question 28.
What is Torr?
Answer:
Torr is the unit of pressure used at high vacuum. 1 Torr = 1 mm of Hg

Question 29.
What is Loschmidt number?
Answer:
The numher of molecules present in 1 ml of gas or vapour at STP is known as Loschmidt number.

Question 30.
What is Boyle’s temperature?
Answer:
The temperature above which a real gas behaves like an ideal gas is called Boyle’s temperature.

Question 31.
Give a main property of a gas.
Answer:
Diffusion is a main property of a gas.

Question 32.
How does rate of diffusion of a gas vary with temperature ?
Answer:
Rate of diffusion of a gas increases with increase in temperature.

Question 33.
State the names of the scientists related to kinetic theory of gases.
Answer:
Kinetic theory of gases was proposed by Bernouli and extended by Clausius, Maxwell, Kronig, Boltzmann etc.

Question 34.
What is collision frequency?
Answer:
The number of collisions made by all gas molecules in a unit volume per second is known as collision frequency.

Question 35.
Define torr ?
Answer:
Pressure exerted by exactly 1 mm of mercury column at 0°C and at standard gravity is termed as 1 torr.

Question 36.
Which state of matter has no definite volume and no definite shape?
Answer:
gaseous state.

Question 37.
What is the value of gas constant in SI unit ?
Answer:
8.314 JK^-1 mol^-1

Question 38. How is the unit ‘L’ related to dm³ ?
Answer:
IL=1 dm³

Question 39.
Name the SI unit of pressure ?
Answer:
Pascal

Question 40.
Under what conditions is Boyle’s law is applicable?
Answer:
At constant mass and at constant temperature.

Question 41.
What is the effect of increase of temperature on vapour of a liquid at constant pressure?
Answer:
With rise of temperature vapour of a liquid increases at constant pressure.

Question 42.
Write down the value of R in L atm mol ^-1 k^-1.
Answer:
0.0821 L atm mol^-1 k^-1

Short Answer Type Questions :

Question 1.
State one point of difference between expansion of gas and expansion of solid.
Answer:
For any range of temperature rise all gases expand equally, but different solids expand by different amount for same range of temperature rise.

Question 2.
Why does not the volume of a real gas become zero at absolute zero?
Answer:
Explanation : Any gas or vapour liquefies much before reaching this low temperature -273°C. Again,Charle’s law is valid for gases, not for liquids. Hence, this situation of zero volume of gas is never attained practically.

Question 3.
Why tyre of an automobile is inflated to a lesser pressure in summer than in winter?
Answer:
Explanation : In summer, the room temperature is much higher as compared to winter.Consequently, the same volume of air will exert greater pressure in summer. Therefore, it is always advisable to inflate the tyre to lesser extent in summer as compared to winter to avoid the bursting of tyres.

Question 4.
Is it possible to cool a gas below absolute zero ?
Answer:
Explanation : No, it is not possible to cool a gas below absolute zero. At absolute zero, the kinetic energy of the gas molecules becomes zero. The molecules come to rest at the bottom of the container.
Therefore, pressure of the gas is also zero. It is therefore, impossible to cool a gas below absolute zero, since there is no heat left to be removed from the gas.

Question 5.
What is effusion of a gas?
Answer:
Effusion: It is the passage of a gas under pressure through a tiny hole in a container. Process of effusion is used to separate the isotopes of an element. During effusion, the lighter isotopes escape first from the pores of the container leaving behind the heavier isotopes.

Question 6.
How does an ideal gas differ from a real gas?
Answer:
Explanation : As ideal gas obeys gas laws or the gas equation P V=n R T all temperatures and pressures whereas a real gas obeys the gas laws or the gas equation only at high temperatures and low pressures. There is no cooling or heating effect observed when an ideal gas expands in vacuum whereas a real gas shows either cooling or heating effect.

Question 7.
Is it possible to keep liquid nitrogen in a sealed cylinder at ordinary temperature like ammonia?
Answer:
Reason : No, it is not possible to keep the liquid nitrogen in a sealed container at ordinary temperature like ammonia because critical temperature of nitrogen is very low whereas the critical temperature of ammonia is lighter than that of ordinary temperature.

Question 8.
Why aerated bottles are kept under water during summer ?
Answer:
Explanation : Areated water bottles contain carbon dioxide gas dissolved in aqueous solution under pressure. In summer, the solubility of the gas in solution decreases with rise in temperature.Consequently, the amount of free gas in bottle increases. This leads to increase in pressure. Thus, the bottle may explode. To avoid explosion, bottles are kept under cold water in summer.

Question 9.
State two characteristics of gases.
Answer:
Characteristics of gases :
(i) A gas has no definite shape or volume. It takes the shape and attains the volume in which it is kept. This tendency of scattering of the gas molecules is called expansion of gas.
(ii) If a few gases which do not react with each other, are kept in a container, these gases mix with each other and a homogeneous mixture is prepared. This property is known as diffusion.

Question 10.
What is normal temperature and pressure (NTP) ?
Answer:
NTP or STP (Standard Temperature and Pressure): It is defined as the pressure exerted by a column of mercury 76 cm in height at 0°C, at 45° latitude and at mean sea-level.

Question 11.
Calculate the value of normal preseure inCGS and SI system.
Answer:
Normal pressure inCGS system : 76 × 13.6 × 980 = 1.013 × 10⁶ dyne / cm² Normal pressure in SI system : 1.013 × 10⁵ N / m²=1.013 × 10⁵ pascal

Question 12.
State Boyle’s law.
Answer:
Boyle’s law (1662) : At constant temperature, the volume of a definite mass of any gas’varies inversely as the pressure of the gas.

Question 13.
Deduce the mathematical expression of Boyle’s law.
Answer:
Mathematical expression of Boyle’s law : If P be the pressure and V the volume of a given mass of a gas, then according to Boyle’s law,
V ∝ \(\frac{1}{P}\) (the mass and the temperature remaining constant)
or, V = \(\frac{K}{P}\) ( K is a proportionality constant)
or, PV = K (constant)
This is the mathematical experession of Boyle’s law.

Question 14.
What will be the nature of graph if P is plotted against V for a given mass of gas at constant temperature?
Answer:
Explanation of graph : On plotting P against volume V fat a given temperature, the graph will be a rectangular hyperbola as shown below.

Question 15.
When a balloon infiates, It seems to violate Boyle’s law. Explain.
Answer:
Explanation : When a rubber balloon inflated with the end of a pump, the pressure inside increases but the volume instead of suffering a decrease in accordance with Boyle’s law increases. This happens because with the introduction of air, the mass of the gas increases resulting an increase in volume. Thus, inflation of a balloon by mouth or pump appears to violate Boyle’s law but it is not so in the true sense.

Question 16.
StateCharle’s law.
Answer:
Charle’s law (1787): At constant pressure, the volume of a given mass of a gas increases or decreases by \(\frac{1}{273}\) of its volume at 0°C for each one degree rise or fall in temperature.

Question 17.
Deduce the mathematical expression ofCharle’s law.
Answer:
Mathematical expression of Charle’s law :
Let V₀ be the volume of adiefnite mass of a gas at 0°C, then the volume of 1°C rise in temperature will be =(V₀+V₀ × \(\frac{1}{273}\))
∴ The volume of t°C rise in temperature will be =V₀ + V₀ × \(\frac{1}{273}\) If V_t represents this volume at t°C then
V_t + V₀+V₀ × \(\frac{t}{273}\) = V₀(1 + \(\frac{t}{273}\))
Similarly, when temperature at the same mass of gas be gradually made to decrease, its volume at -t°C is given by
V_t + V₀ + V₀ × \(\frac{t}{273}\) = V₀(1-\(\frac{t}{273}\))

Question 18.
What will be the nature of graph if V_t is plotted against t for a given mass of gas at constant pressure?
Answer:
Explanation of graph : On plotting V_t against t, at a given pressure the graph will be a straight line. If this straight line is extraploted then the straight line meets at ‘ X ‘-axis which represents the absolute temperature (-273°C).

Question 19.
What is absolute zero? Define absolute scale of temperature.
Answer:
Absolute zero: The lowest possible temperature at which a given mass of gas does not occupy any volume or does not exert any pressure is known as absolute zero.
Absolute scale of temperature : The temperature scale which has been devised by taking -273°C as zero and using the magnitude of each degree as the celsius degree is known as absolute or Kelvin scale of temperature.

Question 20.
What is the alternative form ofCharle’s law?
Answer:
Alternative form ofCharle’s law : Suppose at constant pressure, the volume of a certain mass of gas at 0°C = V₀ and at t₁°C and t₂°C temperatures, the volumes are V₁ and V₂ respectively.

According toCharle’s law,

Alternative statement ofCharle’s law : The volume of a given mass of a gas kept at constant pressure is directly proportional to its absolute (Kelvin) temperature.

Question 21.
State Pressure-Temperature relationship or Gay-Lussac’s law.
Answer:
Pressure-Temperature relationship or Gay-Lussac’s law : At constant volume, the pressure of a given mass of a gas increases by \(\frac{1}{273}\) of its original value at 0°C for every 1°C rise in temperature.

Question 22.
State the mathematical expression of Gay-Lussac’s law.
Answer:
Mathematical expression of Gay-Lussac’s law :

Therefore, Gay. Lussac’s law can also be stated. At constant volume, the pressure of a given mass of a gas is directly proportional to its absolute temperature.

Question 23.
Establish the combined law of Boyle’s andCharle’s laws.
Answer:
Combination of Boyle’s law andCharle’s law :
Let V be the volume of a given mass of gas at pressure P and temperature T (absolute).
From Boyle’s law, V ∝ \(\frac{I}{P}\)
[When temperature and mass of the gas are constant]
FromCharle’s law, V ∝ T
[ When pressure and mass of the gas are constant]
∴ V∝ \(\frac{T}{P}\) when both T and P vary.
or, V = \(\frac{KT}{P}\) or, \(\frac{PV}{T}\) = K [K= constant]
Now, if V₁ is the volume of a gas at pressure P₁ and temperature T₁ and V₂ is the volume of the same amount of gas at pressure P₂ and temperature T₂ then,
\(\frac{P_1 V_1}{T_1}=\frac{P_2 V_2}{T_2}\)

Question 24.
What Is equation of state? What is universal gas constant ?
Answer:
Equation of state: From the combination of Boyle’s andCharle’s laws we get, \(\frac{PV}{T}\) = K
The numerical value of the constant of proportionality (K) depends upon quantity of gas and the units in which volume and pressure are expressed but is totally independent of the nature of the gas.
For 1 mole of gas, the constant is termed as universal gas constant.
∴ \(\frac{PV}{T}\) = R
or, PV = RT
This is known as general gas equation.
For ‘ n ‘ moles of the gas therefore, the gas equation may be written as:
PV = nRT

Question 25.
What is the relation between density and pressure of an ideal gas.
Answer:
According to ideal gas equation PV = nRT = \(\frac{m}{MRT}\) where ‘m’ is the mass of gas and ‘m’ its molecular mass,
P = \(\frac{m}{V}\) \(\frac{RT}{M}\)
or, P = d \(\frac{RT}{M}\) where d = \(\frac{m}{V}\) = density of the gas.
∴ d α P constant temperature.

Question 26.
What is real gas? What is ideal gas ?
Answer:
Real gas : It is a gas which does not obey general gas equation and all other gas laws strictly but tends towards ideality at low pressure and high temperature.
Ideal gas : It is a gas obeys the general gas equation and other gas laws under all conditions of temperature and pressure.

Question 27.
State the values of universal gas constant R in different units.
Answer:
Values of universal gas constant R in different units ;

1. 0.0821 lit atm mol^-1 K^-1
2. 8.314 × 10⁷ erg mol^-1 K^-1
3. 8.314 J mol^– K^-1
4. 1.987 cal mol^-1 K^-1

Broad Answer Type Questions :

Question 1.
What are the characteristic properties of gases ?
Answer:
Characteristic properties of gases :

1. Shape and Volume: Since particles of gases are not held in fixed positions and move freely, gases neither have definite shapes nor definite volumes.
2. Homogeneous nature : All the parts of a gas or a gaseous mixture have similar composition throughout.
3. Density : Due to large separation of molecules, gases have large volume and thus low density.
4. Compressibility : On increasing pressure gases can be readily compressed due to the presence of large empty spaces.
5. Random motion : The molecules or atoms of a gas are in a state constinuous zig-zag motion in all directions.
6. Pressure : Due to their random motion, the molecules of the gas collide on the walls of the container and thus exert certain force on walls of the container. The force per unit area is called the gas pressure.
7. Diffusion : Gases mix (diffuse) with each other freely due to the free movement of their molecules.
8. Liquefaction : On cooling and applying pressure, gases can be liquefied. However, a gas has to be cooled below a certain characteristic temperature called critical temperature before it can be liquefied by the application of pressure alone.

Question 2.
What are the postulates of Kinetic theory of gases?
Answer:
Postulates of Kinetic theory of gases :

1. All gases consist of very large number of tiny particles called molecules that are in constant rapid motion.
2. The gas molecules are perfectly round, very hard and separated by large distances. Their actual volume is thus, negligible as compared to the total volume of the gas.
3. The collisions between the gas molecules are perfectly elastic, i.e. there is no loss of energy during these collisions.
4. The distance between gas molecules being very large, there is no effective force of attraction or repulsion between them.
5. The average kinetic energy of the gas molecules is directly proportional to the absolute temperature of the gas.
6. The gas molecules collide with one another and with the walls of the container. The pressure exerted by a gas is due to the bombardment of its molecules on the walls of the vessel.
7. The gas molecules move freely in all directions. Their speed and direction change continously due to collisions among them. As a result, their motion becomes zig-zag or random.

Brain Storming Questions :
Very Short Answer Type Questions :

Question 1.
What is the significance of S.T.P. or N.T.P?
Answer:
Temperature and pressure affects the volume of gas. In order to compare the volumes of any two gases, they are to be brought under some standard condition of temperature and pressure. For this reason, S.T.P. or N.T.P. are introduced during study of gas.

Question 2.
Why do hot air balloons rise higher than cold air balloons?
Answer:
At higher temperature, a given mass of gas occupies more volume as per charles’ law and is thus dense.Cold air being denser than hot air, raises the balloon to a lesser height.

Question 3.
Why do gas balloons brust at high altitudes?
Answer:
We know that, at high altitudes, the atmospheric pressure on the balloon decreases, resulting in increase in volume as per Boyles’law. So the balloon brusts at high altitudes.

Question 4.
Under what conditions the value of \(\frac{P}{T}\) will be constant irrespective of the value of T ?
Answer:
We know that, for a certain mass of gas at constant volume, \(\frac{P}{T}\) = K (constant). So, the value of \(\frac{P}{T}\) is constant for a fixed mass of gas at constant volume no matter what the value of T is. This is obtained from Gay Lussac’s law.

Question 5.
Carbondioxide is heavler than air, yet it does not form the lower layer of air-why?
Answer:
From the definition of diffusion we know that gases in the air get intermixed. Although CO₂ is heavier than air yet it does not form the lower layer.

Question 6.
Wet air is more penetrating than dry air-why?
Answer:
As wet air being lighter than dry air, so wet air diffuses more readily than dry air.

Question 7.
Name an instrument to measure the pressure of a gas.
Answer:
Manometer is used to measure the pressure of a gas.

Question 8.
What do you mean by STP?
Answer:
STP means standard temperature and pressure. Standard temperature is 0°C. 76 cm mercury pressure or 1 atm. pressure is taken as standard.

Question 9.
Can temperature in Keloin scale be negative?
Answer:
No. starting with the zero reading at absolute zero temperature, temperature in kelvin scale is always positive.

Question 10.
What is the dimension of R ?
Answer:
We know that, universal gas constant, R

Question 11.
On which two factors does the molar volume of a gas depend?
Answer:
Molar volume of a gas depends on pressure and temperature.

Question 12.
What is the Boyle temperature of hydrogen gas?
Answer:
Boyle temperature of hydrogen is -156°C.

Question 13.
Mention an example of diffusion applicable to daily life.
Answer:
Detection of fragrance of perfumes occurs due to gaseous diffusion.

Question 14.
What is the nature of collisions between the molecules of a gas?
Answer:
The collisions between the molecules are perfectly elastic i.e.there is no loss of energy during these collisions.

Question 15.
What is the value of kinetic energy of an Ideal gas at absolute zero temperature ?
Answer:
At absolute zero temperature all the molecular motions cease and hence the kinetic energy of an ideal gas becomes zero.

Question 16.
What is molar volume?
Answer:
The volume occupied by one mole of substance at a given temperature and pressure is called the molar volume of the substance.

Numerical Problems :

(i) T_t=t_c+273
(ii) P₁ V₁=P₂ V₂ (at constant temperature and constant mass of gas)
(iii) V₁=V_{\circ(1+\frac{t{273)
(iv) \(\frac{V_1}{T_1}=\frac{V_2}{T_2}\) (at constant pressure and constant mass of gas)
(v) \(\frac{P_1}{T_1}=\frac{P_2}{T_2}\) (at constant volume and constant mass of gas)
(vi) PV = nRT = \(\frac{m}{MRT}\)

Erample 1:
What will be the reading of 30°C in absolute scale of temperature?
Answer:
The reading of 30°C in absolute scale of temperature
= (273 + 30) K = 303K

Example 2:
What is the value of absolute zero in the celsius scale?Calculate its value in Farhenheit scale.
Answer:
The value of absolute zero in celsius scale = -273°C.
Let the value of the above temperature in Farhenheit scale = X° F.
We know, \(\frac{C}{5}\) = \(\frac{F-32}{9}\)
or, \(\frac{-273}{5}\) = \(\frac{X-32}{9}\)
or, 5 x-160 = -2457 or, 5 x = -2297
or, x = -459.4° F
∴ The temperature in Farhenheit scale = -459.4° F

Example 3 :
27°C or 300 K, which temperautre is higher?
Answer:
27°C = (27 + 273)K = 300 K
So, the two temperatures are equal.

Example 4 :
30°C or 300 K, which temperature is higher ?
Answer:
30°C=(30+273) K=303 K
So, 30°C is higher than 300 K

Example 5:
A weather balloon has a volume of 175 L when filled with hydrogen at a pressure of 1.00 atm.Calculate the volume of the balloon when it rises to a height of 2000 m, where the atmospheric pressure is 0.80 atm. Assume that the temperature is constant.
Answer:
P₁ = 1.00 atm
V₁ = 175 L
P₂ = 0.80 atm
V₂ = ?

According to Boyle’s law
P₁ V₁=P₂ V₂
or, V₂=\(\frac{P_1 V_1}{P_2}\) = \(\frac{1 \times 175}{0.80}\)

Example 6:
A sample of oxygen has a volume of 880 mL and a pressure of 740 torr. What additional pressure is required to reduce the volume to 440 mL.
Answer:
P₁ = 740 torr
V₁ = 880 mL
P₂ = ?
V₂ = 440 mL

According to Boyle’s law
P₁V₁ = P₂ V₂
or, P₂ = \(\frac{P_1 V_1}{V_2}=\frac{740 \times 880}{440}\)
= 218.75 L
∴ Additional pressure required
= (1480-740) torr
= 740 torr

Example 7:
A bottle of volume 9 litres contains a gas at 10 atmospheric pressure. How many bottles each of 1 litre capacity can be filled with the gas at 2 atmospheric pressure, at constant ternerature.
Answer:
P₁ = 10 atm
V₁ = 9 lit
P₂ = 2 atm
V₂ = ?

According to Boyle’s law
P₁ V₁=P₂ V₂
or, V₂=\frac{P₁ V₁{P₂=\frac{10 × 9{2=45 lit
∴ 45 bottles, each of 1 litre volume can be filled.

Example 8 :
A sample of helium has a volume of 520 cm³ at 373 K.Calculate the temperature at which the volume will become 260 cm³. Assume that the pressure is constant.
Answer:
According toCharle’s law
V₁ = 520 cm³
T₁ = 373 K
V₂ = 260 cm³
T₂ = ?
or, = 186.5 K

Example 9:
Find the volume of N₂ at 27°C at a pressure of 760 torr, if it occupies 40 mL at STP.
Answer:
V₁ = 40 mL
T₁ = 373 K
T₂ = (27+373) K=300 K
V₂ = ?

According toCharle’s law

\(\frac{V_1}{T_1}=\frac{V_2}{T_2}\)
or, V₂= \(\frac{V_1 \times T_2}{T_1}\) = \( \frac{40 \times 300}{273}\) = 44 mL

Example 10:
The volume of a certain mass of gas at of 400 K and pressure 202600 Pascal is 2 cubic metres. What would be the volume of the gas at 327°C and 152 cm of mercury pressure?
[given 1.013 × 10⁵ pascal =1 atmospheric pressure]
Answer:
1.013 × 10⁵ Pascal = 76 cm of Hg
202600 Pascal = \(\frac{76 \times 202600}{1.013 \times 10^5}\)
= 125 cm of Hg
T₁ = 327°C = (327 + 273) K = 600K
V₁ = 2 m³
V₂ = ?
T₁ = 400 K

According toCharle’s law

\(\frac{V_1}{T_1}=\frac{V_2}{T_2}\)
or, V₂ = \(\frac{V_1 \times T_2}{T_2}\)
or, V₂ = \(\frac{2 \times 600}{400}\)
∴ V₂ = 3 m³

Example 11:
A steel tank contains carbon dioxide at 27°C and a pressure of 10.0 atm.Calculate the internal gas pressure when the tank and the gas are heated to 100°C.
Answer:
P₁ = 10.0 atm
T₁ = (27 + 273) K = 300 K
P₂ = ?
T₂ = (100 + 273) K = 373 K

According to Gay-Lussac’s law.

\(\frac{P_1}{T_1}=\frac{P_2}{T_2}\)
or, P₂ = \(\frac{P_1 \times T_2}{T_1}\)
or, P₂ = \(\frac{10 \times 373}{300}\) = 12.43 atm.

Example 12 :
An iron cylinder contains helium at a pressure at 250 K Pa at 300 K. The cylinder can withstand a pressure of 1 × 10⁶ Pa. The room in which cylinder is placed catches fire. Predict whether the cylinder will blow up before it melts or not.
(M.P. of the cylinder =1800 K )
Answer:
P₁ = 250 KPa = 250 × 10³ Pa
V₁ = 300 K
P₂ = ?
T₂ = 1800 K

According to Gay-Lussac’s law

\(\frac{P_1}{T_1}=\frac{P_2}{T_2}\)
or, P₂ = \(\frac{P_1 \times T_2}{T_{21}}\)
or, P₂ = \(\frac{250 \times 10^3 \times 1800}{300}\) = 1.5 × 10⁶ Pa

Example 13:
A gas having temperature 0°C is heated so that its pressure and volume are doubled. What will be the final temperature of the gas?
Answer:
Let, P₁ = P (say)
by condition, P₂ = 2 P
again V₁ = V (say)
So, V₁ = 2 V
T₁ = (0 + 273) K = 273 K
T₂ = ?

By combining Boyle’s law andCharle’s law we get

Example 14:
A certain quantity of a gas occupies a volume of 1000 cm³ at 760 mm and 27°C. Find the volume of the gas if the pressure and temperature are 1520 mm and 327°C.
Answer:
P₁ = 760 mm
V₁ = 1000 cm³
T₂ = (273 + 27) K = 300 K
P₂ = 1520 mm
T₂ = (273 + 327) K = 600 K
V₂ = ?

By combining Boyle’s law andCharle’s law we get,

Example 15:
7.0 g of a gas at 300 K and 1 atmospheric pressure occupies a volume of 4.1 littres. What is the molecular mass of gas?
Answer:
w = 7.0 g
R = 0.0821 lit atm mol^-1 K^-1
T = 300 K
M = ?
P = 1 atm
V = 4.1 lit

Applying ideal gas equation,

PV = nRT
PV = \(\frac{w}{M}\)
or, M = \(\frac{wRT}{PV}\)
or, M = \(\frac{7 \times 0.0821 \times 300}{1 \times 4.1}\)
∴ M = 42 g-mol^-1

Example 16:
10 g of oxygen are introduced in a vessel of 5 lit capacity at 27°C.Calculate the pressure of the gas in atmospheres in the container.
Answer:
w = 10 g
M = 32
R = (27+273) K=3000 K
V = 5 lit
R = 0.0821 lit atm mol^-1 K^-1
P = ?

Applying ideal gas equation,

P V =n R T
∴ P V = \(\frac{w}{M}\)
or, P = \(\frac{w R T}{V \times M}\)
∴ P = 1.539 atm

Example 17:
The volume of 1 gram mole of oxygen gas is 22400 mL at 760 mm.Calculate the temperature of the gas (Given R=0.082 L-atm mol{ ^-1 K^-1 )
Answer:
P = 670 mm = 1 atm
V = 22400 mL = 22.4 L
R = 0.082 L – atm mol^-1 K^-1

We know from ideal gas equation for 1 mole of an ideal gas

PV = RT
or, T = \(\frac{P V}{R}\) or, T = \(\frac{1 \times 22.4}{0.082}\)
or, T = 273.17 K
Temperature in celsius scale = 273.17 – 273 = 0.17°C

Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 4 Thermal Phenomena offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 4 Question Answer – Thermal Phenomena

Very Short Answer Type Questions :

Question 1.
Is it possible for a body to have negative temperature in kelvin scale?
Answer:
No, because below 0K temperature, volume of a gas would be negative which is impossible.

Question 2.
What is the SI unit of heat ?
Answer:
SI unit of heat is Joule.

Question 3.
Mention the CGS unit of heat?
Answer:
CGS unit of heat is calorie.

Question 4.
Is volume coefficient of a gas different from its pressure coefficient?
Answer:
No, they are equal.

Question 5.
What is the value of specific heat of water in SI unit?
Answer:
4200 J kg^-1 K^-1.

Question 6.
Is it possible that heat is supplied to a body without changing the temperature?
Answer:
Yes, during change of state there is no change in temperature although heat is supplied.

Question 7.
What is the value of latent heat of fusion of ice in CGS system?
Answer:
80 cal g^-1.

Question 8.
Do water and ice have the same specific heat?
Answer:
No, specific heat of water is 1 cal g^-1 °C^-1 and that of ice is 0.5 cal g^-10 C^-1.

Question 9.
What is difference between 1° C and 1 C° ?
Answer:
1° C is a particular temperature, while 1 C° is the interval of one degree Celsius of temperature.

Question 10.
What is the lower fixed point of a celsius scale?
Answer:
0° C

Question 11.
What is the upper fixed point of a Fahrenheit Scale?
Answer:
212° F

Question 12.
Is there any upper fixed point in Kelvin Scale?
Answer:
273.13 K, which is the triple point of water.

Question 13.
Which is more expansible-solid, liquid or gas ?
Answer:
Gas.

Question 14.
A metal scale does not give correct value at all temperature-explain.
Answer:
At different temperature distance between different marks of the metal scale is different due to thermal expansion of the metal.

Question 15.
The Coefficient of linear expansion of a metal is 19 × 10^-6° C^-1. What is its value per degree Fahrenheit ?
Answer:
∝ = \(\frac{5}{9}\) × 19 ×10^-6 = 10.6 × 10^-6 °F.

Question 16.
Is coefficient of linear expansion possible in the case of a liquid?
Answer:
No, liquid has no definite length.

Question 17.
There is co-efficient of apparent expansion in a liquid but not in a gas-why ?
Answer:
For same rise of temperature, liquid expands only about 10 times than solid, while gas expands about 100 times than solid. So expansion of vessel can be neglected in case of gases.

Question 18.
What is anomalous expansion of water?
Answer:
In the range 0°C to 4°C, volume of water decrease instead of increasing, like other liquids. This is known as anomalous expansion of water.

Question 19.
Why are there two types of coefficient of expansion of a gas?
Answer:
The change of temperature is very much affected by both its pressure and volume, so gas has two types of coefficient of expansion.

Question 20.
Is a temperature lower than absolute zero of temperature possible?
Answer:
No.

Question 21.
What is thermal conductivity of a perfect heat conductor?
Answer:
Infinite.

Question 22.
What is thermal conductivity of a perfect heat insulator?
Answer:
Zero.

Question 23.
Can heat flow by canvection take place in a straight line?
Answer:
In convection heat travels in straight or curved path in upward direction only.

Question 24.
Can convection take place in solid ?
Answer:
No, for convection a fluid medium is required.

Question 25.
What is the absorbing power of a perfectly black body ?
Answer:
One

Question 26.
What is the reflecting power of a perfectly black body ?
Answer:
Zero.

Question 27.
What is a perfectly black body ?
Answer:
A body which absorbs all radiations incident it.

Question 28.
By which mode the heat reaches to the earth from the Sun?
Answer:
Radiation.

Question 29.
Explain for cooking, a black vessel is more convenient than a polished one.
Answer:
Black surface is better absorber of heat.

Question 30.
Heat is generated continuously in an electric heater but its temperature becomes constant offers some time. Why?
Answer:
When rate at which heat is generated by electric current becomes equal to the rate at which heat is lost by radiation, thermal equilibrium is reached and hence temperature becomes constant.

Question 31.
Why ventilator are placed near the roof at a room?
Answer:
Warm air of the room becomes lighter and moves upward. So for better convection current ventilators are placed near the roof of the room.

Question 32.
Name three modes of transfer of heat.
Answer:
Conduction, convection and radiation.

Question 33.
Name the element which is the best conductor of heat ?
Answer:
Silver.

Question 34.
What is the unit of coefficient of thermal conductivity in SI ?
Answer:
Wm^-1 K^-1.

Question 35.
What is thermal expansion?
Answer:
Dimensions of all substances generally increases with increase in temperature. This phenomenon is known as thermal expansion.

Question 36.
Name the three types of expansion in solid?
Answer:
The types of expansion in solid –

1. Linear expansions
2. Superficial expansions
3. Volume expansions.

Question 37.
Define the term ‘coefficient’ of linear expansion of solld.
Answer:
Coefficient of linear expansion of solids : The coefficient of linear expansion of a solid is the increase in its length per unit length per degree rise of temperature.

Question 38.
Give the SI unit of coefficlent of linear expansion.
Answer:
K^-1.

Question 39.
Write the relationship among α, β and γ.
Answer:
α = \(\frac{β}{2}\) = \(\frac{γ}{3}\)

Question 40.
Does unit of coefficient of linear expansion depend on unit of length?
Answer:
No.

Question 41.
What is thermal conduction ?
Answer:
Conduction is the process of transfer of heat through a substance without any motion of the particles of the substance.

Question 42.
Name two substances which are good conductors of heat.
Answer:
Silver, Copper.

Question 43.
Name two bad conductors of heat.
Answer:
Glass and wooden rod.

Short answer type questions :

Question 1.
What do you mean by heat ?
Answer:
Heat : It is a form of energy which produces sensation of warmth.

Question 2.
What are the different types of motion?
Answer:
Different types of motions are

1. Translational motion
2. Vibrational motion
3. Rotational motion

Question 3.
What is definition of heat with respect to motion?
Answer:
Definition of heat with respect to motion: Heat possessed by a body is the total thermal energy of the body and is the sum of kinetic energies of all the individual molecules forming the body due to translational, vibrational and rotational motions of the molecules.

Question 4.
What do you mean by calorie?
Answer:
Calorie: It is the quantity of heat required to raise the temperature of 1 g} water through 1° \mathrm{C}.

Question 5.
What is temperature?
Answer:
Temperature : It is the thermal condition of a body which would determine the direction of flow of heat, when the body is placed in thermal contact with another body.

Question 6.
What is upper fixed point of a thermometer ?
Answer:
Upper fixed point : It is the temperature of steam from water boiling under a pressure of 76 cm} of mercury at sea level and 45° latitude.

Question 7.
What is lower fixed point of a thermometer ?
Answer:
Lower fixed point: It is the temperature of melting ice under a pressure of 76 cm} of mercury at sea level and 45° latitude.

Question 8.
What is fundamental interval ?
Answer:
Fundamental interval. The difference between the fixed points of a scale is called fundamental interval.

Question 9.
What do you mean by thermal expansion ?
Answer:
Thermal Expansion: Dimension of all substances generally increases with increase in temperature. This phenomenon is known as thermal expansion.

Question 10.
What are the types of expansions in solids ?
Answer:
Types of expansions in solids:

1. Linear expansions
2. Superficial expansions
3. Volume expansions

Question 11.
What is apparent expansion of the liquid ?
Answer:
Apparent expansion of the liquid: If the expansion of the liquid is measured ignoring the expansion is called the apparent expansion of the liquid.

Question 12.
What is real expansion of the liquid ?
Answer:
Real expansion of the liquid: When the actual expansion of the liquid is measured by considering the expansion of the containing vessel, it is called real expansion of the liquid.

Question 13.
What is the conclusion of Hope’s experiment ?
Answer:
Conclusion of Hope’s experiment: From Hope’s experiment it is proved that water at bottom which is densest at 4°C. After sufficiently long time the temperature of the lower thermometer falls slightly due to loss of heat by conduction to the upper regions.

Question 14.
What is molar specific heat at constant volume (C_v) ?
Answer:
Molar specific heat at constant volume (C_v) : The molar specific heat of a gas at constant volume (C_v) is the amount of heat required to raise the temperature of one mole of the gas through one degree keeping the volume constant throughout.

Question 15.
What is molar specific heat at constant pressure (C_p) ?
Answer:
Molar specific heat at constant pressure (C_p) : The molar specefic heat of a gas at constant pressure (C_p) is the amount of heat required to raise the temperature of one mole of the gas through one degree keeping the pressure constant throughout.

Question 16.
What is water equivalent of a body ?
Answer:
Water equivalent: Water equivalent of a body is the mass of water which will be heated through one degree by the amount of heat that raises the temperature of the body through one degree.

Question 17.
What is Regelation ?
Answer:
Regelation: The phenomenon of melting of ice under pressure and freezing again on releasing the pressure is called regelation.

Question 18.
What do you mean by vapour pressure of a liquid ?
Answer:
Vapour pressure: Whenever a liquid evaporates at any temperature, the vapour exerts a definite pressure on everything in contact. This pressure is called vapour pressure of the liquid at that temperature.

Question 19.
What is conduction of heat ?
Answer:
Conduction: It is the process of the transfer of heat through a substance without any detectable motion of the particles of the substance.

Question 20.
What is convection of heat ?
Answer:
Convection of heat: It is the process by which heat is transmitted through a liquid or gas from a hotter point to a colder point due to the bodily motion of the heated particles of the substances.

Question 21.
What is Radiation of heat ?
Answer:
Radiation: It is the transmission of heat from a hot body to a cold body without the help of any medium and without appreciable heating at the intervening medium if any.

Question 22.
What is perfectly black body ?
Answer:
Perfectly black body: A perfectly black body is that which absorbs completely the radiations of all the wavelengths on it.

Question 23.
What is green house effect ?
Answer:
Green house effect: Green house effect is an example of selective absorption of heat by glass. The amount of heat transmitted through a substance depends on temperature of the source of heat.

Question 24.
What do you mean by global warming ?
Answer:
Global warming: Carbon dioxide, water vapour, methane, nitrus oxide, tropospheric ozone, chlorofluoro carbon compounds, halogens campounds etc. on increasing the amount of greenhouse gases in the atmosphere, the temperature of earth increases. It is known as global warming.

Broad answer type questipns :

Question 1.
State the units and dimensions of different coefficient.
Answer:
The unirs and dimensions of different coefficient.

Question 2.
What is anomalous expansion of water ?
Answer:
Aromalous expancion of water: Usually liquids expand on heating. But in the case of water we find deviation from this general behaviour of the liquids within a certain range of temperature. The volume of water is minimum at 4°C and hence its density is maximum at 4°C. This phenomenon is called the anomalous expansion of water.

Question 3.
What is the fundamental principle of calorimetry ? What are the conditions ?
Answer:
Fundamental principle of calorimetry:
Heat lost by hot body = Heat gained by cold body.
Cotditicns: (i) during the process of heat transfer, there is no heat exchange with the surrounding.
(ii) no chemical reaction takes place between the bodies.

Question 4.
What is thermometric conductivity ?
Answer:
Thermometric conductivity: The rate of rise of temperature during the variable state is proportional to K/p_s (where K = thermal conductivity of the material, P_s = specific heat). This ratio is known as thermometric conductivity or the thermal conductivity per thermal capacity per unit volume.

Question 5.
Give few applications of conductivity ?
Answer:
Applications of conductivity:
(i) Ice is packed in saw dust, because air which is bad conductors of heat being trapped in the saw dust prevents transfer of heat from the surrounding to the ice. So ice does not melt.
(ii) Cooking utensils are provided with wooden or plastic handles, as wood or plastic are bad conductors of heat, so we can hold the hot utensiles with the help of these handles.
(iii) In winter, birds often swell their feathers, ther by enclosing air between their bodies and feathers and thus does not allow flow of heat from the bodies of the birds and keeps them warm.

Frain Storing Questions :
Very Short Answer Type Questions :

Question 1.
The value of α for iron is 1.2 × 10^-5. What do you mean by that?
Answer:
This means 1 cm of an iron rod (at 0°c) expands linearly by 1.2 × 10^-5 cm for 1°C rise in temperature.

Question 2.
Name two devices which use bimetallic strip.
Answer:
Automatic fire alarm and thermostat.

Question 3.
The diameter of an iron tyre is kept slightly smaller than the wooden wheel on which this tyre is to be mounted. why?
Answer:
The diameter of an iron tyre is kept slightly smaller than the wooden wheels because of heating, the iron tyre expands and perfectly fits over the wooden wheels.

Question 4.
Between apparent and real expansion coefficients of a liquid which one is its own characteristic?
Answer:
Apparent expansion of liquid happens simply because the container expands. Therefore, real expansion coefficient of a liquid is its own characteristic.

Question 5.
How δ_r is related to δ_a & δ_g ?
Answer:
The relation is :
δ_r = δ_a + δ_g (δ_r = Real expansion of liquid
δ_a = Apparent expansion of the liquid
δ_g = Volume expansion of the container)

Question 6.
What is the conductivity for vacuum ?
Answer:
Conduction does not take place through vacuum. So, pure vacuum has zero conductivity.

Question 7.
What is thermal resistivity?
Answer:
Reciprocal of coefficient of thermal conduction is called thermal resistivity (\(\frac{1}{K}\)).

Question 8.
What is the unit of thermal resistivity?
Answer:
The unit of thermal resistivity is j^-1 m.k.s

Question 9.
What should be the value of thermal conductivity for an ideal conductor ?
Answer:
The value of thermal conductivity for an ideal conductor is infinite.

Question 10.
Write the dimension of thermal conductivity (K)
Answer:

Numerical Problems

Example 1:
On a certain day the maximum temperature was found to be 120°F. What is it in celsius scale?
Answer:
We know that
\(\frac{C}{5}\) = \(\frac{F-32}{9}\)
Let 120°F = x°C
or, \(\frac{x}{5}\) = \(\frac{120-32}{9}\)
or, x = 48.9°C

Example 2:
A thermometer reads 5° in melting ice and 99° in dry steam at normal pressure. Find the temperature on the Fahrenheit scale when the thermometer reads 52°.
Answer:
Let the temperature in the Fahrenheit scale be x°F corresponding to 52° in the faulty thermometer whose fundamental interval in 99° – 5° = 94°. Thus,

or,
x = 90 + 32 = 122°F

Example 3:
Find the temperature at which the reading in Fahrenheit scale is double of the reading in the celsius scale.
Answer:
Let x°C = 2 x°F
We know \(\frac{C}{5}\) = \(\frac{F-32}{9}\)
or, \(\frac{x}{5}\) = \(\frac{2 x-32}{9}\)
or, x = 160°C and 2 x = 320°F

Example 4:
What is the reading of a Fahrenheit thermometer when a centigrade thermometer reads 25°C ? The temperature of a body is raised by 25°C. What is the value of this rise of temperature in Fahrenheit scale?
Answer:
We know, \(\frac{C}{5}\) = \(\frac{F-32}{9}\)
We have, \(\frac{25}{5}\) = \(\frac{F-32}{9}\)
∴ F = 45 + 32 = 77°F
We know, 1 division on centigrade scale = \(\frac{9}{5}\) division on the Fahrenheit scale
∴ 25°C = \(\frac{9}{5}\) × 25 = 45°F

Example 5:
Find the increase in energy per atom of aluminium when temperature of a piece of aluminium increases by 1° C .27 g of aluminium contains 6 ×10²³ atoms and its specific heat is 0.2 .
Answer:
Let us take 27 g of aluminium heat absorbed by it in raising its temperature by 1°C = 27 × 1 × 0.2 = 5.4 cal
= 5.4 × 4.2 J
Now, 27 g of aluminium contains 6 ×10²³ atoms
Thus, energy per atom = \(\frac{5.4 ×4.2}{6 ×10²³}\) = 3.78 × 10^-23 J

Example 6:
Two rods, one of glass and the other of steel, are of equal length of 0°C. At 100°C they differ in length by 1 mm. Find their length at 0°C. Given α for glass = 8 × 10^-6 C and α for steel = 12 ×10^-6 C^-1.
Answer:
Let length of each rod l₀ m at 0° C and at 100° C. Let the lengths of glass and steel rod be l g and l s metres respectively.
This, l_s = l (1 + 8 × 10^-6: 100) and l_s = l₀(1 + 12 × 10^-6 × 100)
∴ l_s – l_g + l₀ × 1 v^-4(12-8) = 4 × 1 J^-4 l₀
Now, l_s – l_s = 1 mm = 10^-3 m
So, 10^-3 = 4 × 10^-4 l₀
∴ l₀ = 25 m

Example 7:
Two vessels connected by a thin pipe with a sliding plug contain a liquid at temperature 20° C and 80° C. What is the ratio of the heights of liquid columns in the vessel if the coefficient of volume expansion of the liquid be 10^-3 °C^-1 ?
Answer:
Let h₁ and h₂ be the heights of the liquid columns at 20°C and 80°C and corresponding densities be ρ₁ and ρ₂.
Now at equilibrium condition,

h₁ ρ₁ g=h₂ ρ₂ g
or,

Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 8.1 Periodic Table and Periodicity of the Properties of Elements offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 8.1 Question Answer – Periodic Table and Periodicity of the Properties of Elements

Very Short Answer Type Questions :

Question 1.
Periodic changes of what occur in a periodic table?
Answer:
Physical and chemical properties of sets of elements arranged in some manner change periodically.

Question 2.
How does atomic size of elements change in a group?
Answer:
Atomic size gradually increases downward in a yroup.

Question 3.
How does electronegativity of elements change along a period of periodic table?
Answer:
Electronegativity of elements gradually increases along a period from left to right of periodic table.

Question 4.
How many groups are there in the long form periodic table ?
Answer:
There are 18 groups in the long form periodic table.

Question 5.
How does metallic character of elements change in a group in periodic table?
Answer:
Metallic character of elements gradually increases downward in a group.

Question 6.
Which is more fundamental-atomic number or atomic weight of elements ?
Answer:
Atomic number is more fundamental than atomic weight of elements.

Question 7.
How are elements arranged in Mendeleev’s modern periodic table?
Answer:
Elements are urianged in Mendeleev’s modern periodic table in ascending order of their atomic number.

Question 8.
What is the position of chlorine in the Mendeleev’s periodic table?
Answer:
The position of chlorine in the Mendeleev’s periodic table:
Period : 3
Group : VIIB

Question 9.
In which group of Mendeleev’s periodic table are kept the alkali metals ?
Answer:
Alkali metals are kept in group IA in Mendeleev’s periodic table.

Question 10.
What is the name ‘Oxygen’ group ?
Answer:
Chalcogens, group.

Question 11.
What are ‘d’-block elements called?
Answer:
‘d’-block elements are called transition elements.

Question 12.
What are ‘f’-block elements called ?
Answer:
‘f’-block elements are called inner transition elements.

Question 13.
How many elements are there in first period of Mendeleev’s periodic table?
Answer:
The first period contains two elements. (Hydrogen and Helium)

Question 14.
What is the name of first group elements of periodic table ?
Answer:
The first group elements of periodic table are called alkali metals.

Question 15.
What is the decreasing order of electron affinity of F, Cl, Br ?
Answer:
The decreasing order of electron affinity of F, Cl, Br is Cl>Br>F.

Question 16.
Is Cobalt a transition element ?
Answer:
Yes, Cobalt is a transition element.

Question 17.
Is the second I.P. is always greater than the first I.P. of a given species?
Answer:
The second I.P. is always greater than the first I.P. of a given species.

Question 18.
Is radioactivity a periodic property ?
Answer:
Radioactivity is not a periodic property.

Question 19.
Between K and C a atom which one has larger in size ?
Answer:
K atom has larger in size than Ca atom.

Question 20.
What is the symbol of the element having atomic number 109 ?
Answer:
The symbol of the element having atomic number 109 is Mt.

Question 21.
Who proposed modern periodic law ?
Answer:
Modern periodic law was proposed by Mosely.

Question 22.
What are representative elements ?
Answer:
Elements of s-and p-blocks are collectively known as normal or representative elements.

Question 23.
What are the elements of second period called ?
Answer:
Elements of second period are called bridge elements.

Question 24.
What are the elements of third period called ?
Answer:
Elements of third period are called typical elements.

Question 25.
Between Na and \(\mathbf{N a} a^{\oplus}\) which one has greater is size ?
Answer:
Na has greater in size than \(\mathbf{N a} a^{\oplus}\).

Question 26.
Between Cl and \(\mathrm{Cl}^{\Theta}\) which one has smaller in size ?
Answer:
Cl has smaller in size than \(\mathrm{Cl}^{\Theta}\).

Question 27.
Between \(\mathbf{N a} a^{\oplus}\) and Mg²⁺ which one has smaller in size ?
Answer:
Mg²⁺ has smaller in size than \(\mathbf{N a} a^{\oplus}\).

Question 28.
Are Van der Waal’s radii larger than covalent radii ?
Answer:
Van der Waal’s radii are larger than covalent radii.

Question 29.
Atomic radii decrease across a period. However, at the end of each period there is increase in atomic radii. Why?
Answer:
Because atomic radii in case of noble gases are Van der Waal’s radii.

Question 30.
Have ionisation energies a positive value?
Answer:
lonisation energies have a positive value.

Question 31.
Why halogens have high values of electron affinity ?
Answer:
Halogens have high values of electron affinity due to their ns² np⁵ configuration.

Question 32.
What is the classification of elements ?
Answer:
The method of arranging similar elements together and separating them from dissimilar elements is called classification of elements.

Question 33.
What is the law of triads?
Answer:
According to law of triads, in a triad of elements, having similar properties, the atomic weight of the central atom was merely the arithmetic mean of the atomic weights of the other two elements.

Question 34.
Between Br and I which one has metallic character ?
Answer:
Between Br and I, iodine has metallic character.

Question 35.
What is the valency of an alkali metal ?
Answer:
The valency of an alkali metal is 1.

Question 36.
What is the relation between N^3- and O^2- ?
Answer:
N^3- and O^2- are iso-electronic ions.

Question 37.
Which halogen is radioactive element?
Answer:
Astatine (At) is the only radioactive halogen.

Question 38.
Which group of elements was missing from Mendeleev’s original periodic table?
Answer:
Mendeleev’s original periodic table did not contain noble or inert gases belonging to Group 18 of the modern periodic table.

Question 39.
In. which period of the periodic table are first transitonal elements found?
Answer:
The first series of transitional elements belong to the 4th period.

Question 40.
X, Y and Z are the elements of a Dobereiner’s triad. If the atomic mass of X be 20 and that of Z be 40, What should be the atomic mass of Y ?
Answer:
Atomic mass of Y = Arithmetic mean of atomic masses of X and Z = \(\frac{20+40}{2}\) = 30

Question 41.
Mention the position of the radioactive alkall metal.
Answer:
Francium (Fr), the radioactive alkali metal, has the position in 1st group of 7 th period.

Question 42.
Name the lanthanide having the lowest atomic number.
Answer:
Cerium \({ }_{58} \mathrm{Ce}\) is the lanthanide having lowest atomic number.

Question 43.
Which halogen has the lowest electronegativity?
Answer:
Electronegativity of an atom decreases from top to bottom in a group. There fore, Astatine (At) has the lowest electronegativity of 2.2 (Pauling scale).

Question 44.
The atomic number of an element is 9. In which group should tt be placed in the modern periodic table?
Answer:
The electronic configuration of the element is 2,7. Since it has 7 electrons in its outermost shell, it should be placed in Group 17.

Question 45.
Name one element which was not known during Mendeleev’s time, but a place was left vacant in Mendeleev’s periodic table.
Answer:
The element is Germenium (Ge) which was not known during Mendeleev’s time, but its properties were predicted by Mendeleev and accordingly a place was kept vacant for it in his periodic table.

Short Answer Type Questions :

Question 1.
What is the necessity of arrangingrelements in the periodic table?
Answer:
Necessity of arranging elements in the periodic table It was observed from the early days that there were few groups of elements each of which had almost identical chemical and physical properties. So, a systematic arrangement of elements is essential since it is difficult to remember the individual properties of elements.

Question 2.
What is the ‘law of triads’?
Answer:
Law of triads (Dobereiner, 1817) : In a triad of elements having similar properties, the atomic weight of the central element was merely the arithmetic mean of the atomic weights of the other two elements.

Question 3.
What is the ‘law of octaves’ ?
Answer:
Law of octaves (Newlands, 1864) : If the elements are arranged in the increasing order of their atomic weights, the eighth succeeding element was the repetition of the first one like the 8 th note of musical scale i.e. first and similar characteristics.

Question 4.
What is Mendeleev’s periodic law ?
Answer:
Mendeleev’s periodic law (1869) : The physical and chemical properties of elements are the periodic function of their atomic weights.

Question 5.
What is modern periodic law ?
Answer:
Modern periodic law (Moseley) : It states that the physical and chemical properties of elements are the periodic function of their atomic numbers.

Question 6.
What is periodicity ?
Answer:
Periodicity : It is the recurrence of elements with similar properties after certain regular intervals when these are arranged in the increasing order of their atomic numbers.

Question 7.
Define group and period of modern periodic table.
Answer:
Period: The horizontal rows along which elements occur in the periocic table in ascending order of atomic number having dissimilar chemical properties are called periods.
Group: The vertical columns in which elements of similar physical and chemical properties occur in the periodic table are called groups.

Question 8.
How many periods and groups are present in Mendeleev’s periodic table and in the long form periodic table?
Answer:
Mendeleev’s periodic table contains seven periods and nine groups. Long form periodic table contains seven periods and eighteen groups.

Question 9.
What are the structural features of long or extended form of the periodic table (Bohr’s table)?
Answer:
Bohr’s table has the following features :
(i) All the elements have been arranged in the increasing order of atomic members.
(ii) Elements with similar electronic configurations have similar properties and hence have been placed together at one place.
The periodic table consists of :
(a) Seven horizontal rows called periods
(b) Eighteen vertical columns called groups or families.
(c) Four blocks (s, p, d, f)

Question 10.
What are the defects of long form of the periodic table ?
Answer:
Defects of long form of the periodic table :
(a) Position of hydrogen. It does not resemble fully with alkali metals but has been placed along with them. It also resembles halogens.
(b) Position of lanthanides and actinides are not proper in the periodic table.
(c) According to electronic configuration, helium should be placed in s-block where as it is placed in p-block.

Question 11.
What is atomic volume?
Answer:
Atomic volume : Atomic volume of an element is the volume in cm³ occupied by one gram atom of the element in the solid state and hence it is also called gram-atomic volume.

Question 12.
Explain how the atomic size of the elements change in periodic table?
Answer:
Atomic size : The distance of the outermost orbit from the nucleus of spherically shaped atom is called the atomic size.
The atomic size gradually decreases from left to right of the period upto the group VIIB, again increases in the end element.

Question 13.
What is Covalent radius ?
Answer:
Covalent radius : It is defined as one half of the distance between the centres of nuclei of two similar atoms held together by a purely covalent single bond.

Question 14.
What is Van der Waal’s radius?
Answer:
Van der Waal’s radius : It is defined as one half of the internuclear distance between two similar, adjacent atoms belonging to two neighbouring molecules of the same substance in the solid state.

Question 15.
What is metallic radius ?
Answer:
Metallic radius : It is defined as one half of inter-nuclear distance between two nearest metal atoms in a metallic lattice is called metallic radius.

Question 16.
What is ionic radius ?
Answer:
Ionic radius : It is defined as the effective distance from the nucleus of an ion upto which it has an influence in the ionic bond.

Question 17.
What is lonisation energy (IE) or lonisation potential (IP) ?
Answer:
lonisation energy or lonisation potential : First ionisation energy or simply ionisation energy (IE) is defined as the amount of energy required to remove one valence electron from an isolated neutral gaseous atom resulting in the formation of a monovalent positive ion.

Question 18.
What is electron affinity ?
Answer:
Electron affinity (EA) : First electron affinity or simply electron affinity is the amount of energy released when one electron is added to a neutral gaseous atom to form a monovalent negative ion.

Question 19.
What is the definition of electronegativity ?
Answer:
Elecironegativity (Pauling’s definition): It is the attractive force which an atom, bonded by a co-valent bond exerts on the bond pair of electrons responsible for the co-valent bond.
The electro-negativity of the elements increase from left to right of the periods in a periodic table.

Question 20.
What are s-block elements ?
Answer:
s-block elements : These are the elements of IA or 1 group (alkali metals; configuration n s¹ ) and IIA or 2 group (alkaline earth metals ; configuration n s² ). These are so named because the last electron in them enters s-oribitals.

Question 21.
What are p-block elements ?
Answer:
p-block elements These are the elements in which the last electron enters p-orbital of valence shell. The elements with configurations n s² n p¹ to n s² n p⁶ constitute this block. Thus p-block consists of elements of group IIIA(13), IVA(14), VA(15), VIA (16), VIIA (17) and zero group (18).

Question 22.
What are d-block elements ?
Answer:
d-block elements: These are the elements in which the last electron enters a (n-1) d orbital. These have configuration. (n-1) d^1-10 n s^0-2. This block is situated in between s and p-block elements. d-block elements are also called transition elements.

Question 23.
What are f-block elements ?
Answer:
f-block elements: These are the elements in which the last electron enters a ( n-2) f-orbital. Lanthanoids and actinoids constitute the f-block and are also shown separately at the bottom of the periodic table. They have (n-2)f^1-14 (n-1) d^1-10 n s² configuration. Elements of f-blocks are also called inner-transition elements.

Question 24.
What are inert gases or noble gases ?
Answer:
Inert gases or noble gases: The elements which belong to the group 18 of the periodic table are called inert gases or noble gases. They have 8 electrons (except He ) in their outermost shell. Therefore, their combining capacity or valency is zero. Hence, they are inert in nature.

Question 25.
What are representative elements ?
Answer:
Representative elements: The elements in which only the outer s or p-electron sub shell is incompletely filled are called representative or normal elements. Elements of s or p-blocks excluding the inert gases are included in this category. These elements have the outer electronic configuration from ns¹ to np⁵.

Question 26.
What are transition elements ?
Answer:
Transition elements: These are the elements in which the last shell is not completely filled. These elements have the configuration (n-1) d^1-9 ns^1-2 i.e., these elements contain 1-9 electrons in the penultimate shell and 1-2 electrons in the valence shell. The elements having unfilled or partially filled d-orbitals are named transition elements because these present a transition (change) from the most electro-positive elements to the most electro-negative elements.

Question 27.
What are inner transition elements ?
Answer:
Inner transition elements : Lanthanides \(\left({ }_{53} \mathrm{Ce}-{ }_{71} \mathrm{Lu}\right)\) and actinides \(\left({ }_{90} \mathrm{Th}-{ }_{103} \mathrm{Lw}\right)\) tare collectively known as inner transition elements. In these elements, three outermost shells are not completely filled. The last electron in them enters in the (n-2) subshell.

Question 28.
What is diagonal relationship?
Answer:
Diagonal relationship : Elements of second and third row which are present diagonally have similar properties because on moving along the diagonal, the decrease and increase of size, electropositive character and polarizing power partly cancel each other.

Question 29.
What is the IUPAC Nomenclature of elements (z >100) ?
Answer:
IUPAC Nomenclature of elements (z >100) : Elements with atomic number beyond 100(z >100) have been named according to IUPAC system, which is connected with the elements atomic number. The first two letters tell us how many hundred (e.g. Un = one) the next three how many tens (e.g. nil = 0 ) the rest units (e.g. quad = 4, pent = 5, hex = 6, hept = 7 and so on).

Question 30.
Ca²+, K⁺, Cl^– have 18 extra nuclear electrons. How will they be arranged in the increasing order of size?
Answer:
Explanation : Size of iso-electronic ions decreases with increase in atomic number. Therefore increasing order of size is :
Ca²⁺< K⁺< Cl^–< S^2-

Question 31.
Explain the reason why the first ionization energy of Na is smaller than that of Mg and second ionisation energy of Mg is smaller than that of Na.
Answer:
Explanation : Electronic configuration of Na and Mg are 1s² 2s² 2p⁶ 3s¹ respectively. Therefore magnesium has higher first ionization potential than Na due to its higher value of nuclear charge and more stable configuration (fully filled s-orbital).
After removal of one electron, Na⁺ and Mg⁺ ions have configuration 1s² 2s² 2p⁶ and 1s² 2s² 2s² p⁶ 3s¹ respectively and now it will be easier to remove 3s¹ electron rather than electron is lower than that of Na.

Question 32.
Differentiate between covalent radius and Van der Wal’s radius.
Answer:
Difference between Covalent radius and Van der Waal’s radius : Covalent radius is one half of the distance between the centres of nuclei of two similar atoms held together by a purely covalent bond but van der waal’s radius is one half of the inter-nuclear distance between two similar adjacent atoms belonging to two neighbouring molecules of the same substance in the solid state.

Broad Answer Type Questions :

Question 1.
State the different periods with the elements.
Answer:
The different period swith the elements :

Question 2.
What are group and sub-groups?
Answer:
Groups : Mendeleev’s periodic taule shows that the elements with related chemical properties fall in c ne below the other forming vertical columns called groups. There are nine groups from group I to group VIII and 0 (zero). Sub-groups : Each of the groups from I to VII has been divided into two sub-groups A and B.

Question 3.
What are called alkali metals ? In which group do they belong ? State the similarity of their chemical properties.
Answer:
Alkali metals : Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb) and Caesium (Cs). These five metals are generally known as alkali metals. Position in periodic table: The alkali metals are included in the A subgroup of the first group (IA).
Similarity : (i) Alkali metals are strong electro positive.
(ii) The oxides of these metals are strongly basic.
(iii) Each has valency 1.

Question 4.
Where are the inert gas elements placed and why ?
Answer:
Position of inert gas elements in periodic table : He, Ne, Ar, Kr, Xe, and Rn. These are inert elements. They are each gaseous and monoatomic. These are chemically non-reactive. As these elements do not react, these have zero valency.
So they are included in 0 (zero) group of the periodic table.
Besides Helium, all the inert gases have eight (8) electrons in their outermost orbit. There are only 2 electrons in the outermost orbit of Helium.

Question 5.
What are halogen elements ? In which do they belong ?
Answer:
Halogen elements : The four strongly electro-negative non-metals fluorine (F), chlorine (Cl), bromine (Br) and iodine (I) form a family of closely allied elements known as the halogens meaning literally sea salf-producer as these elements react with most metals to form compounds similar to sea-salt, sodium chloride. Position in periodic table: Halogen elements are placed in group VIIB of periodic table. The electro-negative character of the elements increases from left to right in a period. So, the strongly electronegative elements are in the almost extreme right group i.e. in group VIIB of the periodic table.

Question 6.
Discuss the position of hydrogen in periodic table.
Answer:
Position of hydrogen in periodic table :
Reasons for placing in group IA :

1. Like the alkali metals, hydrogen is electro-positive.
2. Valency of hydrogen is I, alkali metals are also mon-valent.
3. During electrolysis of a fused chloride of an alkali metal, the alkali metal deposits at the cathode; in the electrolysis of dilute aqueous solution of hydrogen chloride, hydrogen collects at the cathode.
4. Like the alkali metals, hydrogen has reducing property and forms stable oxide, like water (H₂O).
5. Like hydrogen, each of the alkali metals, Li, Na, K, Rb, Cs, Fr possesses one valence-electron.

Reasons for placing in Group VIIB :

(i) Like the halogens, hydrogen is a non-metallic element.
(ii) Valency of hydrogen and that of each halogen is 1.
(iii) Halogen molecules are diatomic, a hydrogen molecule is also diatomic.
(iv) The halogens from metallic halides like, NaCl, KBr, Kl etc. Hydrogen also produces salt-like hydrides like LiH, NaH, CaH₉ etc with the strongly electropositive elements and hydrogen here acts as an electro-negative element.
(v) Atoms of halogen elements may transform to negative halide ions by taking one electron each. (e.g. X + e → X^– ; X = F, Cl, Br, I) and hydrogen atom also may transform to a negative hydride ion by capturing oen electron : H + e → H^–.
(vi) Like the hologens, hydrogen also can produce covalent comj unds reacting with electro-negative elements like S, O etc.
Due to such varied tendency for occupying a seat in the periodic table, hydrogen is often called a naughty element or a rogue elements.

Question 7.
Draw a diagram by which change of periodic properties are shown.
Answer:
Diagram.

Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 8.6 Organic Chemistry offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 8.6 Question Answer – Organic Chemistry

Very Short Answer Type Questions :

Question 1.
What is the common element of organic compounds ?
Answer:
Carbon is the common element of organic compounds.

Question 2.
What is Catenation ?
Answer:
Catenation is the property of organic compounds where a large number of carbon atom link together.

Question 3.
What is monomer ?
Answer:
Monomer is a small organic molecule that joins with other similar molecules to form a polymer.

Question 4.
What is mustard gas ?
Answer:
It is a gas produced from ethylene.

Question 5.
What is a primary alcohol ?
Answer:
It is a type of alcohol in which the carbon atom bearing the OH group con­tains at least 2 hydrogen atoms.

Question 6.
What is an unsaturated hydrocarbon ?
Answer:
It is an organic compound in which at least two carbon atoms join by covalent double or triple bond.

Question 7.
What is a saturated hydrocarbon ?
Answer:
It is hydrocarbon in which carbon atoms are linked with single covalent bond.

Question 8.
What is a functional group ?
Answer:
Functional group is a group of atoms present in organic compounds of a class determining almost the common properties of the compounds.

Question 9.
What type of bonding exists in organic compounds ?
Answer:
Covalent type of bonding exists in organic compounds.

Question 10.
What is DNA ?
Answer:
DNA stands for deoxyribonucleic acid.

Question 11.
What are biomolecules ?
Answer:
These are some organic molecules involved in metabolic process.

Question 12.
What is isomerism ?
Answer:
Isomerism is the property due to which a group of organic compounds of same molecular formula but differ from each other in their structural formulae and properties.

Question 13.
State one use of methane.
Answer:
Use of methane : As a domestic and industrial fuel.

Question 14.
State one use of ethylene.
Answer:
Use of ethylene : To prepare polythene.

Question 15.
State one use of acetylene ?
Answer:
Use of acetylene : To produce benzene, artificial rubber.

Question 16.
What are the essential two components of amino acids ?
Answer:
The essential two components of amino acids are carboxyl (-COOH) and an amino (-NH₂) group attached to the same carbon atom.

Question 17.
Name and write down the formula of a ketone.
Answer:
The name of a ketone is acetone (CH₃COCH₃).

Question 18.
Which gas burns in a carbide gas lamp ?
Answer:
Acetylene gas burns in a carbide gas lamp.

Question 19.
What change of litmus will occur in alcohol ?
Answer:
Alcohol is a neutral compound, so no change of colour of a litmus paper dipped in it occurs.

Question 20.
What is the functional group of alcohol ?
Answer:
Hydroxyl group (-OH) is the functional group of alcohol.

Question 21.
Which gas is known as marsh gas ? Why is it called so ?
Answer:
Methane gas is known as marsh gas. It is present in marshy (i.e. always wa­tery) lands, so it is called marsh gas.

Question 22.
Name three hydrocarbons available from coal gas.
Answer:
Methane, ethylene, acetylene are three hydrocarbons available from coal gas.

Question 23.
Give two examples of alkyne with corresponding formulae.
Answer:
Two alkyne :

• Acetylene (HC ≡ CH)
• Propyne (CH₃– C = C – H)

Question 24.
What is alkane ? Write down its general formula.
Answer:
An alkane is an open-chained saturated hydrocarbon.
The general formula of alkane : C_nH_{2n + n}(n – integer)

Question 25.
Name and draw structural formula of a saturated organic compound.
Answer:
Saturated organic compound :

Question 26.
Name and draw structural formula of an unsaturated organic compound.
Answer:
Unsaturated organic compound : Ethylene

Question 27.
Name and draw structural formula of an aromatic compound.
Answer:
Aromatic compound Benzene

Question 28.
Name three organic compounds used in daily life.
Answer:
Three organic compounds used in dialy life : Carbohydrates, proteins, glucose.

Question 29.
Name two plymers.
Answer:
Two polymers are :

• Polythene
• Teflon

Question 30.
What is hydrocarbon ? Name the simplest hydrocarbon.
Answer:
Hydrocarbon : A binary compound formed of carbon and hydrogen by covalency is called hydrocarbon.
Simplest hydrocarbon : Methane (CH₄).

Question 31.
What is PVC ? State its use.
Answer:
PVC : It is polyvinyl chloride, its monomer is vinyl chloride.
Uses of PVC : To prepare water and rain pipes, toys etc.

Question 32.
Why butane is used in LPG ?
Answer:
Butane is the most convenient fuel for domestic use because both isomers of butane (n-butane and isobutane) are easily liquefied and can be transported in steel cylinders easily.

Question 33.
How does the boiling point of alkane changes ?
Answer:
The boiling point generally increase with increase in the number of carbon atoms.

Question 34.
What is mineral oil ?
Answer:
Oil obtained from petroleum is called mineral oil.

Question 35.
What is fire damp ?
Answer:
The gas responsible for explosions in coal mines is methane and is also known as fire damp.

Question 36.
Why are the alkenes more reactive than alkanes ?
Answer:
The chemical reactivity of alkenes are mote than alkanes due to presence of π-electron in alkenes.

Question 37.
How many s and p bonds are present in ethylene ?
Answer:
Ethylene has one π-bond and five σ-bonds.

Question 38.
Why the hydrogens of alkynes are acidic in nature ?
Answer:
Hydrogen has appreciable acidic character when bond to a carbon atom of a(C = C) triple bond (in case of alkyne).

Question 39.
What are the end products of combustion of hydrocarbons ?
Answer:
End products of combustion of all hydrocarbons are carbon dioxide and water.

Question 40.
What is the most oxidised form of hydrocarbon ?
Answer:
RCOOH (R = alkyl group) represents the most oxidised form of hydrocarbons.

Question 41.
What is sabatier and senderens reaction ?
Answer:
Hydrogenation of unsaturated aliphatic hydrocarbons in presence of nickel catalyst is called sabatier and senderens reaction.

Question 42.
What is the condition for halogenation of alkanes ?
Answer:
Halogenation of alkanes does not occur in absence of light or heat.

Question 43.
What is aldose ?
Answer:
Carbohydrate containing aldehyde group is called aldose.

Question 44.
What is ketose ?
Answer:
Carbohydrate containing keto group is called ketose.

Question 45.
Give an example of a monosaccharide.
Answer:
Glucose (C₆H₁₂O₆)

Question 46.
Give an example of polysaccharide.
Answer:
Starch.

Question 47.
What is pyrofax ?
Answer:
Propane is used as a fuel under the name pyrofax.

Question 48.
What is an artificial camphor ?
Answer:
Hexachloroethane is called artificial camphor.

Question 49.
What is TEL ?
Answer:
TEL is commonly used antiknock compound tetraethyl lead, [(C₂H₅)₄ Pb].

Question 50.
What is AK – 33X ?
Answer:
To avoid lead pollution, a new compound called AK – 33X (cyclopentadienyl manganese carbonyl) is used as an antiknock these days.

Question 51.
What is dextrose ?
Answer:
Glucose is called grape sugar or dextrose.

Question 52.
What is fruit sugar ?
Answer:
Fructose is called laevolase or fruit sugar and is the sweetest sugar.

Question 53.
What is milk sugar ?
Answer:
Lactose is known as milk sugar.

Question 54.
What is amylum ?
Answer:
Starch is called amylum.

Question 55.
State an example of globular protein.
Answer:
Insulin is an example of globular protein.

Question 56.
What is nucleotide ?
Answer:
Both DNA and RNA are polymers of a basic repeating unit, called a nucle­otide.

Question 57.
What is the sugar present In RNA ?
Answer:
Sugar present in RNA is ribose.

Question 58.
What is the sugar present in DNA ?
Answer:
Sugar present in DNA is 2-deoxyribose.

Question 59.
What are the main functions of nucleic acids ?
Answer:
Main functions of nucleic acids are the direct synthesis of protein in living cells and transference of genetic information.

Question 60.
Who discovered the double helix structure of DNA ?
Answer:
The double helix structure of DNA was proposed by Watson and Crick (1953).

Question 61.
What is called gene ?
Answer:
DNA sequence that acts as a code for a specific protein or a polypeptide is called gene.

Question 62.
What is called an anabolism ?
Answer:
Anabolism is the process in which macro molecules are synthesised by the cell.

Question 63.
What is called catabolism ?
Answer:
Catabolism is the process in which macro molecules break into smaller ones.

Question 64.
What is metabolism ?
Answer:
Metabolism is the combination of anabolism and catabolism.

Question 65.
What is proteases ?
Answer:
Proteases is the breakdown of large protein molecules into peptides.

Question 66.
Who converts peptides into amino acids ?
Answer:
Peptidases convert peptides into amino acids.

Question 67.
What is soda lime ?
Answer:
Soda lime is a mixture of sodium hydroxide and calcium oxide (NaOH + CaO).

Question 68.
What is the source of acetylene ?
Answer:
The source of acetylene is calcium carbide (CaC₂) from which it is obtained by the action of water at ordinary temperature.
CaC₂ + 2H₂O → C₂H₂ + Ca(OH)₂.

Question 69.
Name one biodegradable polymer.
Answer:
One biodegradable polymer is cellulose.

Question 70.
Name the hydrocarbon formed when ethanol is heated with concentrated H₂SO₄
Answer:
When ethanol is heated with concentrated H₂SO₄, ethene (or ethylene) is formed.

Question 71.
What is the common name of ethyne?
Answer:
The common name for ethyne is acetylene.

Question 72.
What is the term used for the compounds which have same molecular formula but different structures?
Answer:
They are called isomers.

Question 73.
What is next homologue of C₂H₅OH?
Answer:
The next homologue of C₂H₅OH (Called ethanol or ethyl alcohol) is C₂H₇OH (propanol).

Question 74.
How is biopolymer protein biodegraded in nature?
Answer:
Proteins are degraded by some specific enzymes produced by some particular Phy. Sc.bacteria (e.g. Bacillus subtilis, Bacillus mycoides, Bacillus vulgaris etc) through ammonification.

Question 75.
How many hydrogen atoms are there in alkyne containing three carbon atoms?
Answer:
The general formula of alkyne is C_nH_2n-2
Here, n = 3
∴ Number of hydrogen atoms = 2n-2 = (2×3)-2=4

Question 76.
What is power alcohol?
Answer:
In countries having shortage of petrol, a mixture of petrol (80%), ethanol (20%) and benzene is used as fuel. This petrol mixed with alcohol is known as power alcohol.

Question 77.
Name two functional groups one containing carbon atom and the other devoid of carbon.
Answer:
Carbon containing functional group : carboxyl

Functional group devoid of carbon : Amino

Question 78.
Give the structural formula of propanal.
Answer:
CH₃ – CH₂ -CHO

Short Answer Type Questions :

Question 1.
What is organic chemistry ?
Answer:
Organic chemistry : All carbon containing compounds except oxides of carbon, metal carbonate, bicarbonate, hydrogen cyanide and metallic cyanides are organic compounds and the chemistry of organic compounds is called organic chemistry.

Question 2
What is Biochemstry ?
Answer:
Biochemistry : It is the branch of chemistry which deals with the com¬position and behaviour of living system.

Question 3.
What are Biomolecules ?
Answer:
Biomolecules : These are the macro-molecules like carbohydrates, amino acids, proteins, vitamins, fats, RNA, DNA etc., which are essential for the continuation of life process of biological species like plants and animals (including human beings) are called biomolecules.

Question 4.
What are Carbohydrates ?
Answer:
Carbohydrates These are the polyhydroxy aldehydes or ketones or these are the compounds which on acidic hydrolysis give polyhydroxy aldehydes or ketones. Their molecules are composed of carbon, hydrogen and oxygen. Carbohydrates are mainly used as food which give us energy to work.

Question 5.
What are Monosaccharides ?
Answer:
Monosaccharides : These are the compounds such as glucose and fructose which do not break into more simpler compounds on hydrolysis.

Question 6.
What are Disaccharides ?
Answer:
Disaccharides : These are the compounds which on hydrolysis give two monosaccharide units.
[Sucrose, Moltose and lactose (milk sugar)]

Question 7.
What are Polysacharides ?
Answer:
Polysaccharides : These are the compounds which on hydrolysis produce very large number of monosaccharide molecules. Cellulose and starch are two important examples of polysaccharides.

Question 8.
What is Moltose ?
Answer:
Moltose : It is obtained by the partial hydrolysis of starch by enzyme diastase present in malt.

Question 9.
What is Lactose ?
Answer:
Lactose : It occurs in the milk of all animals cow’s milk contains about 5% Lactose while human milk contains about 7% lactose.

Question 10.
What is Cellulose ?
Answer:
Cellulose It is the main structural material of wood and other plants. Cotton is about 80% cellulose.

Question 11.
What is Glycogen ?
Answer:
Glycogen : It is a higher sugar stored in liver. In case of emergency, this gets hydrolysed to glucose which then gets oxidised to produce energy.

Question 12.
What are Amino acids ?
Answer:
Amino acids : These are organic compounds containing both amino and carboxylic group in their molecules. They are represented by the general formula.

Question 13.
What are essential amino acids ?
Answer:
Essential amino acids : Human body can synthesis 10 out of 20 a-amino acids found in proteins. The remaining 10 must be present in our diet and are called essential amino acids.

Question 14.
What is Zwitter ion ?
Answer:
Zwitter ion In aqueous solution, the acidic carboxyl group donates a proton to the basic amino group to form an internal salt called a dipolar ion or zwitter ion. Although it is neutral overall, it contains both a positive and a negative charge.

Question 15.
What are Peptides ?
Answer:
Peptides These are condensation products of self-amides formed by the reaction of two or more amino acid molecules.

Question 16.
What is peptide linkage ?
Answer:
Peptide linkage : The bond

between the carboxyl group of an acid molecule and nitrogen of the other amino acid molecule is known as the peptide bond or peptide linkage.

Question 17.
What are Proteins ?
Answer:
Proteins These are complex nitrogeneous substances present in all forms of living matter. These are obtained by the condensation polymerisation of a-amino acids through the formation of peptide bonds. Actually proteins are polypeptides with very high molecular weights (more than 10,000). These are formed by the combination of more than 100 molecules of amino acids.

Question 18.
What is Denaturation ?
Answer:
Denaturation : After coagulation, proteins lose their physiological activity and certain other properties. This phenomenon is known as denaturation.

Question 19.
What are Enzymes ?
Answer:
Enzymes : These are also proteins which acts as catalyst in many bio-chemical reactions. Enzymes are specific in action due to their specific structural arrangement.

Question 20.
What is the biuret test ?
Answer:
Biuret test : To alkaline solution of proteins add a dilute solution of CuS04. Formation of violet colour confirms proteins.

Question 21.
What are Vitamins ?
Answer:
Vitamins : These are the biomolecules needed in small quantities, that regulate many biochemical function and prevent the development of many deficiency diseases.

Question 22.
What are Fats ?
Answer:
Fats : These are organic compounds composed of carbon, hydrogen and oxygen. They are made of glycerol and fatty (organic) acids. Fats may be of animal or vegetables origin.

Question 23.
What are the types of simple proteins ?
Answer:
Types of simple proteins :

• Albumins — e.g. milk, serum etc.
• Globumins — e.g. egg yolk, tissues etc.
• Glutemins — e.g. wheat, rice etc.
• Prolamins — e.g. barli, wheat etc.
• Scleroproteins — e.g. keratin, fibroin etc.

Question 24.
State examples of conjugated proteins and derived proteins.
Answer:
Conjugated proteins :
(a) Phosphoproteins
(b) Glycoproteins
Derived proteins : This type of protein is obtained after the partial hydrolysis of protein of very high molecular weight by acid, base or enzyme to simpler proteins.

Question 25.
What is DNA ?
Answer:
DNA : It is deoxyribonucleic acid. DNA molecule contains three different chemical constituents :
(a) Phosphoric acid
(b) Deoxyribose
(c) Pyridine like base adenine and guanine, pyrimidine like base thymine and cytosine. DNA consists of two strands of polynucleotides coiled around each other by hydrogen bond in the form of a double helix.

Question 26.
What is RNA ?
Answer:
RNA : It is consisted by ribose along with phosphoric acid and bases. In pyrimidine base uracil is present instead of thymine in RNA. RNA carries the message of DNA and acts accordingly. Mainly there are three types of RNA :

• m-RNA
• t-RNA
• r-RNA

t-RNA and m-RNA have taken an important role in the protein synthesis.

Question 27.
What is Catenation ?
Answer:
Catenation : The property by virtue of which carbon forms covalent linkage chains is called catenation.

Question 28.
What is Functional group ?
Answer:
Functional group An atom or a group of atoms which being present within the molecule of an organic compound, causes the compound to function or behave chemically in a particular way is called a functional group, e.g. alcohol (-OH), aldehyde (-CHO)

Question 29.
What are Hydrocarbons ?
Answer:
Hydrocarbons : These are organic compounds containing only carbon and hydrogen atoms in their molecules. They are divided into two classes.

• Saturated hydrocarbons
• Unsaturated hydrocarbons.

Question 30.
What are saturated hydrocarbons ?
Answer:
Saturated hydrocarbons : Saturated hydrocarbons are those in whose molecules the carbon atoms are joined to each other by single bond and the remaining valencies of the carbon atoms are satisfied by hydrogen atoms. e.g. Methane (CH₄), Ethane (C₂H₆).

Question 31.
What are unsaturated hydrocarbons ?
Answer:
Unsaturated hydrocarbons :
The compounds in which carbon atoms are connected among themselves by double bond or triple bond are called unsaturated hydrorcarbons.

Question 32.
What are Alkenes ?
Answer:
Alkenes Those unsaturated hydrocarbons containing double bond (=) between two adjacent carbon atoms in their molecules are called as alkenes.

Question 33.
What are Alkynes ?
Answer:
Alkynes : Those unsaturated hydrocarbons containing triple bonds (s) be­tween two adjacent carbon atoms in their molecules are called as alkynes.

Question 34.
What are Cyclic compounds ?
Answer:
Cyclic compounds : Organic compounds containing closed of atoms are called cyclic compounds. Cyclic compounds are of two types,

• Homocyclic compounds
• Heterocyclic compounds.

Question 35.
What are Homocyclic compounds ?
Answer:
Homocyclic compounds These are the compounds where all the atoms present in the cyclic compounds in the series are carbon atoms. These are of two types,

• Aromatic compounds
• Alicyclic compounds.

Question 36.
What are Aromatic compounds ?
Answer:
Aromatic compounds Aromatic compounds are those which have a hexagonal ring structure formed by six carbon atoms bonded each other by a single or double bonds.

Question 37.
What are Alicyclic compounds ?
Answer:
Alicyclic compounds : These compounds are the cyclic or ring compounds without having any benzene ring.

Question 38.
What are Heterocyclic compounds ?
Answer:
Heterocyclic compounds : Sometimes N, O, S atoms are linked along with carbon atoms in series during the formation of closed ring structure. These compounds are called heterocyclic compounds.

Question 39.
What are Homologous series ?
Answer:
Homologous series A homologous series may be defined as a group of compounds in which various members

• have similar chemical properties
• can be represented by the same general formula
• possess the same functional group the different members of homologous series are called homologues and the phenomenon is called homology.

Question 40.
What is Isomerism ?
Answer:
Isomerism In organic chemistry when the same molecular formula rep­resents two or more compounds which differ in their physical and chemical properties, then such compounds are called isomers and the phenomenon is called isomerism.

Question 41.
What are Structural isomers ?
Answer:
Structural isomers : Isomers that have same molecular formula but differ in the arrangement of atoms within the molecule are known as structural isomers.

Question 42.
What are Stereoisomers ?
Answer:
Stereoisomers The isomers that have the same constitution but different in the spatial arrangement of their atoms are called stereoisomers.

Question 43.
What are the types of structural isomers ?
Answer:
(a) Chain isomerism :

Question 44.
What is the “will-o-the wisp”?
Answer:
In marshy lands and in sewage sludge, methane gas is set free by the bacterial decomposition of vegetable matters under water. Methane itself is highly inflammable. Moreover, a little phosphine (PH₃) and diphosphine (P₂H₄) accompany the gas and make it spontaneously inflammable. Thus the ‘will-o-the-wisp’ results.

Question 45.
Draw position isomers of butene(C₄H₈)
Answer:
Position isomers of butene (C₄H₈)are shown below :

Question 46.
Name an organic compound which is
(a) used to illuminate country houses
(b) used to make polythene
(c) poisonous containing -OH group
(d) consumed as a drink
Answer:
(a) Acetylene
(b) Ethene
(c) Methanol
(d) Ethanol.

Question 47.
Which gas is produced when sodium carbonate reacts with acetic acid ?
Answer:
Acetic acid decomposes sodium carbonate to liberate CO₂
2CH₃COOH + Na₂O₂CO₃→ 2CH₃COONa + CO₂↑+ H₂O

Question 48.
How can traces of ethylene mixed with methane be identified?
Answer:
When the gas mixture is passed through reddish-brown solution of bromine in CCl₄the solution becomes colourless due to the formation of colourless 1, 2-dibromoethane if the gas mixture contains ehhylene.

This is a test for detecting ethylene and ethylenic unsaturation in the organic compounds.

Short Answer Type Questions 

Question 1.
State the difference between organic and inorganic compounds.
Answer:
Difference between organic and inorganic compounds :

Organic Compounds

• The catenation property of carbon atoms among themselves and other atoms give rise to limidess number of organic compounds.
• They form covalent bonds.
• They have low melting and low boiling point.
• These are not ionised at all.
• They show isomerism.
• They are soluble in organic solvents like alcohol, ether etc.

Inorganic compounds

• Due to absence of catenation property of its atoms the number of inorganic compounds formed by the rest of the elements is not so large .
• Inorganic compounds may be covalent or electrovalent.
• They have high melting and boiling point.
• Most of the inorganic compounds are electrolytes.
• They have high rate of reaction.
• Very few Inorganic compounds show isomerism.
• They are soluble in ionising solvent like water, but are insoluble in organic solvent.

Question 2.
State the following facts of Methane.
(i) Source/preparation
(ii) Important reaction
(iii) Uses
(iv) Structure
Answer:
The following facts of methane :

Question 3.
State the following facts of Ethylene.
(i) Source/preparation
(ii) Important reaction
(iii) Uses
(iv) Structure
Answer:
The following are of ethylene.

Question 4.
What are Polymers and what are Monomers. Give few examples.
Answer:
Polymer : Under suitable conditions, many molecules of alkene and alkyne combine together forming a very high molecular weight compound known as polymer. The small moleculers are known as monomers and this process is known as polymerisation.

Some common polymers

Question 5.
What are Biodegradable and Non-biodegradable materials.
Answer:
Biodegradable materials : Materials of vegetable and animal origin invariably decay and decompose into CO₂, H₂O, N₂ or NH₃ by the com­bined action of sometimes of natural agencies like air, water, subshine etc. These are called biodegradable materials.

Non-biodegradable materials : Synthetic materials like plastics, polythene, teflon, PVC etc, are not decomposed by these natural agencies even on for a long time. These are called non-biodegradable materials.

Question 6.
State the following facts of acetylene.
(i) Source/preparation
(ii) Important reaction
(iii) Uses
(iv) Structure
Answer:
The following facts of acetylene

Question 7.
Discuss about the hazards of using Polyethylene, Teflon and PVC.
Answer:
Explanation : Polyethylene, teflon and PVC are non-biodegradable material. These substances do not decompose or decay naturally on long standing. These articles are usually left in soil or water. This practice causes pollution of soil, water and air.

(a) Solid wastes containing PVC when incinerated (consumed by fire) produce the highly toxic substance dioxin. Soil contains two main bios, detrivore and decomposer which analyse or detoxify many bio-degradable substances.

(b) But the polyethylene, teflon, PVC etc. are not bio-digradable substances, they rather spoil detrivore and decomposer of soil. In presence of air and water these synthetic substances excreate some poisonous chemicals in top soil spoiling the minerals necessary for plants.

Question 8.
State possible alternatives to avoid the hazards due to polythene materials.
Answer:
Possible alternatives : The possible alternative that can eliminate the hazards of using polythene is to restrict their uses to a minimum extent. In places of polythene bags for carrying purchases, bags made of cloth, paper or jute should be used. Paper or dry leaf packets should be used instead of polythene packets to carry sweets and other edible solid materials.

The use of polythene glass, tea-cups etc. should be discontinued, and those made of hard paper or earthenwares should be used instead. Polythene sheets for covering should be replaced by thin terpaulin, waxed paper or tar-laminated papers, jute cloth etc.

Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 6 Current Electricity offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 6 Question Answer – Current Electricity

Very Short Answer Type Questions :

Question 1.
What is electric current?
Answer:
Electric current is general means a continuous flow of electrons, ions or any electrically charged particles through a medium.

Question 2.
What are conductors ?
Answer:
The substances through which electric charge flows easily are known as conductors.

Question 3.
What are non-conductors ?
Answer:
The substances which do not allow electric charge to pass through them are called non-conductors or insulators.

Question 4.
How can we define electric current in a quantitative way ?
Answer:
In a quantitative way we can say that the rate of flow of electric charge through any cross section of a conductor per unit time is called the electric current.

Question 5.
What do you mean by D.C. ?
Answer:
If the electric current always flow in the same direction then the current is called D.C. (Direct Current.)

Question 6.
What do you mean by A.C.?
Answer:
If the direction of current alternates i.e. changes periodically from one direction to opposite direction then the current is called A.C. (Alternating current).

Question 7.
What is electric cell?
Answer:
A device in which electrical energy is obtained from the chemical energy is known as electric cell.

Question 8.
What is negative electrode?
Answer:
The metal rod in which there is excess of negative charge is called negative electrode of cell.

Question 9.
What is positive electrode?
Answer:
The metal rod in which there is excess of positive charge is called positive electrode.

Question 10.
What is open circuit?
Answer:
When the electrodes of a cell are not connected by a conductor, externally, the cell is said to be in open circuit.

Question 11.
What is close circuit?
Answer:
When the electrodes are connected internally with a conductor, the cell is said to be in closed circuit.

Question 12.
What is emf of a cell?
Answer:
The potential difference between the electrodes of a cell in open circuit is called emf (electromotive force).

Question 13.
What is the direction of current in the external circuit of a cell?
Answer:
Current flows from positive electrode to negative electrode in the external circuit of a cell.

Question 14.
What is the emf of a simple voltaic cell?
Answer:
The emf of a simple voltaic cell is 1.08 volt.

Question 15.
What is the physical nature of electromotive force?
Answer:
Electromotive force is some energy.

Question 16.
What is the unit of charge in SI system?
Answer:
The unit of charge in the SI system is coulomb.

Question 17.
What is the SI unit of current strength?
Answer:
The SI unit of current strength is ampere.

Question 18.
What are the units of electromotive force and potential difference in SI system?
Answer:
The SI unit of both electromotive force and potential difference is volt.

Question 19.
What is the SI unit of resistance?
Answer:
The SI unit of resistance of Ohm.

Question 20.
State the cases in which Ohm’s law is not valid.
Answer:
Ohm’s law is not valid for current flowing through gases under low pressure, electrolytes and semi-conductors.

Question 21.
How does the resistance of a conductor depend on the cross section of the conductor?
Answer:
Resistance of the conductor decreases with increase of cross section.

Question 22.
In a system of resistors connected in parallel, how is the magnitude of the equivalent resistance related to the magnitude of the resistor of least value?
Answer:
Equivalent resistance is smaller than the resistance of smallest resistor.

Question 23.
How is the heat generated due to electric current through a resistor related to the strength of current?
Answer:
Heat is directly proportional to square of current.

Question 24.
How is the heat generated due to electric current in a resistor related to resistance of the resistor.
Answer:
Heat is directly proportional to resistance.

Question 25.
What is 1 B.O.T.?
Answer:
The total electric energy expended in 1 hour at the rate of 1 kilowatt is known as 1 B.O.T. (Board of Trade unit).

Question 26.
Which energy is converted to which other in an electric motor?
Answer:
In an electric motor, electric energy is converted to mechanical energy.

Question 27.
What is earthing?
Answer:
Earthing : It means to connect the metal case of an electrical appliance to the earth with the help of a metal wire.

Question 28.
What is the usual colour of a live wire?
Answer:
The usual colour of a live wire is red.

Question 29.
What is the usual colour of a neutral wire?
Answer:
The usual colour of a neutral wire is black.

Question 30.
What is the usual colour of the earthing wire?
Answer:
The usual colour of the neutral wire is green.

Question 31.
Which effect of electric current is demonstrated in an electromagnet?
Answer:
Magnetic effect.

Question 32.
How is current related to potential difference?
Answer:
Current is directly proportional to potential difference.

Question 33.
What is the unit of resistivity in CGS system?
Answer:
The unit of resistivity in CGS system is Ohm-Cm.

Question 34.
Current flows through a conductor from east to west, in which direction electrons flow through it?
Answer:
Electrons flow from west to east.

Question 35.
What is an electromagnet?
Answer:
An electromagnet is a temporary magnet produced by passing electtric current through an insulated copper wire coiled around a soft iron body.

Question 36.
What is the core of an electromagnet?
Answer:
The soft iron body around which an insulated copper wire is coiled is called the core of the electromagnet.

Question 37.
Mention two uses of electromagnet.
Answer:
Electromagnet is used in electric calling bell, electric motor.

Question 38.
What happens if the soft iron used in the electromagnet of an electric bell be replaced with steel?
Answer:
The bell will not work, since the steel body turns to a permanent magnet.

Question 39.
How does the strength of an electromagnet depend on the nubmer of turns of a solenoid?
Answer:
Number of turns of insulated wire per unit length of a solenoid increases strength of electromagnet.

Question 40.
What is the function of an electric switch?
Answer:
Electric switch is a very common and simple device used to stop or allow flow of electric current to an electric current to an electric appliance as and when needed.

Question 41.
What is voltmeier?
Answer:
A voltmeter is used to measure the potential difference between two points in a section of an electrical circuit.

Question 42.
What is an ammeter?
Answer:
An ammeter is used to measure the current flowing through an electric circuit.

Question 43.
What should be the resistance of an ideal ammeter?
Answer:
Ideally the resistance of ammeter should be zero.

Question 44.
What should be the reisstance of an ideal volmeter?
Answer:
Ideally the resistance of voltmeter should be infinity.

Question 45.
What are the metals used to prepare fuse wire?
Answer:
Usually fuses consist of fine wires made of an alloy of lead (75%) and a small amount of tin (25%).

Question 46.
What is the rating of a fuse wire?
Answer:
The maximum current that may be allowed to flow through fuse wire before it melts is called the rating of fuse wire.

Question 47.
What is the nature of electric charge on an ebonite rod, when it is rubbed with cut skin?
Answer:
Negative charge.

Question 48.
A glass rod is rubbed with silk. What type of charges do they acquire?
Answer:
Glass is positively charged and the silk is negatively charged.

Question 49.
What is the SI unit of electric charge ?
Answer:
Coulomb (C)

Question 50.
What is the least value of electric charge available?
Answer:
1.6 × 10^-19C

Question 51.
How many electrons will have a total charge of one coulomb?
Answer:
Number of electrons = \(\frac{q}{e}\) = \(\frac{1}{1.6 \times 10^{-19}}\) = 6.25 × 10¹⁸.

Question 52.
Name two basic properties of electric charge.
Answer:
(i) The electtric charge of an isolated system is conserved and (ii) the electric charge is quantised.

Question 53.
What is meant by conservation of charge?
Answer:
It means that the total electric charge in an isolated system remains constant.

Question 54.
How is the mass of a body affected on charging?
Answer:
The charging is due to transfer of electrons from one body to another. So, mass increases in the case of negatively charged body and decreases in the case of positively charged body.

Question 55.
In coulomb’s law, on what factors does the value of electrostatic force constant K depend?
Answer:
It depends upon the system of units used and on the interverning medium.

Question 56.
Electrostatic force between two charges is called central force. why?
Answer:
It acts along the line joining the centres of the charges, and hence, it is a central force.

Question 57.
Does a dipole experience a force, when placed in the non-uniform plectric field?
Answer:
Yes, it experiences a force.

Question 58.
What is electric flux ? Write its SI unit?
Answer:
The electric flux linked with a surface is the total number of lines passing through the surface. Its SI unit is Nm² C^-1.

Question 59.
What is electric potential?
Answer:
The electric potential at a point is the work done in bringing a unit positive charge from infinity to that point in the electric field.

Question 60.
What is electric potential energy?
Answer:
The electric potential energy is the work done in bringing charges from infinity to their respective positions to form the system.

Question 61.
Define electric potential difference between two points in an electric field.
Answer:
The electric potential difference between two points in an electric field is the work done in bringing a unit positive charge from one point to the other point.

Question 62.
Illustrate a condition in which electric field is zero but potential is not zero.
Answer:
Electric field inside a hollow charged sphere is zero but potential is not zero.

Question 63.
Illustrate a condition in which electric field is not zero but potential is zero.
Answer:
The electric field on the equatorial line of an electrical dipole is not zero but the potential is zero.

Question 64.
Define the unit of electric unit.
Answer:
The unit of current is ampere. It is the one coulomb of charge flowing through a conductor in one second.

Question 65.
What is the direction of conventional current?
Answer:
It is the direction opposite to the flow of electrons in a conductor under the influence of electric field.

Question 66.
What is current density?
Answer:
It is the current flowing per unit area of a conductor.

Question 67.
What is the direction of current density?
Answer:
Its direction is same as that of applied electric field.

Question 68.
What is meant by steady current?
Answer:
A current whose magnitude does not change with time.

Question 69.
What is meant by varying current?
Answer:
A current whose magnitude changes with time.

Question 70.
What is drift velocity?
Answer:
It is the average velocity with which a free-electron gets drifted in an conductor under the influence of an external electric field applied to the conductor.

Question 71.
How does the drift velocity of electrons in a metallic conductor vary with temperature?
Answer:
Drift velocity of a metal decreases with increase in temperature.

Question 72.
What do you mean by relaxation time or mean free time?
Answer:
It is average time interval between the two successive collisions between electron and ion in a conductor.

Question 73.
On what factors does the resistance of the conductor depend?
Answer:
The resistance varies with length of the conductor and inversely proportional to area of cross section of the conductor and increases with temperature of the conductor.

Question 74.
What is the difference between Ohmic and Non-Ohmic conductors?
Answer:
Ohmic conductors strictly obey Ohm’s law while Non-Ohmic conductors do not obey Ohm’s law.

Question 75.
What do you mean by conductivity of a material? Give its SI unit.
Answer:
It is the reciprocal of resistivity. Its SI unit is mho m^-1.

Question 76.
What is CFL ?
Answer:
CFL is compact fluorescent lamp.

Question 77.
What is LED ?
Answer:
LED is light emitting diode.

Question 78.
What is the value of EMF of a voltaic cell and that of a Leclanche cell ?
Answer:
The value of EMF of a voltaic cell is 1.08 volt and that of Leclanche cell is 1.5 volt.

Question 79.
What is the value of permitivity of vacuum?
Answer:
Its value is, ε₀ = 8.854 × 10^-12 C² N^-1 m^-2

Question 80.
What do you mean by EMF of a cell?
Answer:
EMF of a cell may be defined as the energy spent (or work done) per unit charge in taking one unit positive charge around the complete circuit.

Question 81.
What do you mean by internal resistance of a cell?
Answer:
The resistance offered by a cell to the flow of current when it passes through it, is called the internal resistance of that cell. It is generally represented by r.

Question 82.
Name of metal which behaves as a superconductor?
Answer:
Mercury below 4.2 K behaves as a superconductor.

Question 83.
Mention one use of superconductivity?
Answer:
Superconductons are used to construct very strong magnets.

Question 84.
Which effect of current is utilized in an electric bulb?
Answer:
The heating effect of current is utilized in an electric bulb.

Question 85.
Is Joule heating a reversible effect?
Answer:
The phenomenon of joule heating is an irreversible one-change of the direction of current does not reverse the heating effect.

Question 86.
Why are coils of electric toasters and irons made of an alloy rather than a pure metal ?
Answer:
The resistivity of an alloy is higher than the pure metal. Moreover, at higher temperature, the alloys do not melt readily. Hence, the coils of heating appliances such as electric toasters and irons are made of an alloy rather than a pure metal.

Question 87.
When an electric bulb is connected to a 12 V battery, it draws a current of 1A. What is the power of the bulb?
Answer:
Power of the bulb, P = 12 V × 1 A = 12 W

Question 88.
What is the full form of EER?
Answer:
The full form of EER is Energy Efficiency Ratio.

Question 89.
How can you define EER, say, for an air conditioner?
Answer:
Energy Efficiency Ratio (EER) for an air conditioner can be defined as follows: EER of AC = cooling capacity (in watt)/Power Consumption (in watt)

Question 90.
Show that, potential difference × electric current = electric power
Answer:
Electric power is the electric work done per unit time.
So, power P = Work done/time or, P = W/t
Putting W = V.Q = Vlt, we have, P = \(\frac{\mathrm{VIt}}{\mathrm{t}}\) = VI
∴ Electric Power (P) = Potential difference (V) × Electric current (I).

Question 91.
Which effect of current can be utilized in detecting a current carrying wire concealed in a wall?
Answer:
The electromagnetic effect can be utilized for the purpose.

Question 92.
Which rule is known as Motor rule?
Answer:
Fleming’s left hand rule is known as Motor rule.

Question 93.
Who first showed that a momentary electric current is set up in closed coll of wire by moving it near a magnet or in any other magnetic field?
Answer:
Michael Faraday (in 1831)

Question 94.
What type of energy transfer takes place in a dynamo?
Answer:
A dynamo converts mechanical energy into electrical energy and generates DC.

Question 95.
Mention a way to increase the magnitude of e.m.f generated in a generator.
Answer:
The magnitude of e.m.f. generated can be increased by increasing the strength of the magnetic field in the generator.

Question 96.
For a tube light, which circuit should be used?
Answer:
Since a tube light consumer less power, so it should be connected to the lighting circuit (5A).

Question 97.
For an air conditioner, which circuit should be used?
Answer:
Since an air conditioner consumes more power, so it must be connected to the 5 A power circuit.

Short answer type questions :

Question 1.
What do you mean by potential difference?
Answer:
Potential difference It is the electrical condition of a point in an electric field or on a current carrying conductor that indicates whether electrons will flow from it or it from another connected point.

Question 2.
What is the definition of coulomb ?
Answer:
Coulomb : It is the quantity of electric charge that passing through silver nitrate solution deposits 0.001118 g silver at the cathode.

Question 3.
What is the definition of ampere?
Answer:
Ampere : It is the current that flowing through silver nitrate solution for one second during electrolysis deposits 0.001118 g silver at the cathode.

Question 4.
What is the definition of ohm ?
Answer:
Ohm : If one ampere current flowing through a conductor establishes 1 volt potential difference between the two ends of the conductor, the resistance of the conductor is one ohm.

Question 5.
State Ohm’s law.
Answer:
Ohm’s law (1826) : The temperature and other physical conditions remaining constant the current flowing between any two points of a conductor is proportional to the potential difference between them.

Question 6.
Deduce the mathematical form of Ohm’s law.
Answer:
Mathematical form of Ohm’s law :
Let V_A and V_B are the potentials at the ends A and B of the conductor A B respectively.
So, the potential difference between the points is V_A – V_B=V (say).

Now, if current I flows through the conductor, then following ohm’s law, V α I
or, V = R I(R= constant, the resistance of conductor )
or, \(\frac{V}{I}\) = R

Question 7.
What is the definition of resistance from Ohm’s law ?
Answer:
Definition of resistance from Ohm’s law : The resistance of a conductor is a ratio of the potential difference between its ends to the current flowing through it.

Question 8.
On what factors does the resistance of a conductor depend ?
Answer:
Factors upon which the resistance of a conductor depends :
(i) Effect of length : Temperature, material and area of cross section remainning constant, the resistance (R) of a conductor is proportional to its length (1)
∴ R ∝ l (when temperature, material and cross-section are constant)
(ii) Effect of cross-section : Temperature, material and length remaining constant the resistance (R) of a conductor is inversely proportional to its area of cross-section (A)
∴ R ∝ \(\frac{1}{A}\) (When temperature, material and length are constant)

Question 9.
What is specific resistance ?
Answer:
Specific resistance : We know, R ∝ l when A is constant
R ∝ \(\frac{1}{A} \) when l is constant
When both length and the area of cross-section of a conductor vary, then from the law of joint variation, we can write,
R ∝ \(\frac{1}{A}\)
or, R = ρ \(\frac{1}{A}\) [ρ (rho) is the constant of proportionality and is known as the specific resistance of resistivity]
Now, if l = 1 and A = 1, then R = ρ

Definition: The specific resistance or resistivity of a material is numerically equal to the resistance of a conductor of the material of length 1 metre and area of cross-section 1 m².

Question 10.
Specific resistance of copper 20°C is 1.6 × 10^-6 ohm-cm, what do you mean by it ?
Answer:
Specific resistance of copper 20°C is 1.6 × 10^-6 ohm-cm}, it means: Resistance across the opposite faces of a copper cube of 1 cm side, at 20° C is 1.6 × 10^-6 ohm.

Question 11.
What do you mean by combination of resistance ?
Answer:
Combination of resistance : In different electrical circuit more than are resistance are connected together. This is known as combination of resistances. Usually two types of combination are used-
(i) Series combination
(ii) Parallel combination

Question 12.
Define equivalent resistance.
Answer:
Equivalent resistance : The single resistance, instead of multiple resistance in a circuit, keeps the voltage and current unchanged, is called equivalent resistance of those resistances.

Question 13.
What do you mean by series combination?
Answer:
Series combination: In this combination resistances are so connected that extreme end of one resistance is joined to the begining end of next resistance and so on. In this connection same current flows through all the resistances. If three resistors r₁ r₂ r₃ connected in series, the same current I passes through each then their equivalent resistance R will be.

Question 14.
What do you mean by parallel combination?
Answer:
Parallel combination : A number of resistors are said to be connected in parallel when they are placed side by side and their corresponding ends joined together so that the main current is distributed among them.

If the individual resistances is parallel combination are r₁ r₂ r₃ then their equivalent resistance R is given by
\(\frac{1}{R}=\frac{1}{r_1}+\frac{1}{r_2}+\frac{1}{r_3}\)
So, to create a low resistance out of few relatively high resistances, those needed to be connected to parallel combination. Equivalent resistance in parallel combination is lesser than the lowest of the individual resistances.

Question 15.
What is internal resistance of a cell ?
Answer:
Internal resistance: The small resistance offered by the electrolyte of a cell to the electric charges flowing through it from the negative to the positive plate is known as the internal resistance of the cell.

Question 16.
What is watt-hours ? Whose unit is it ?
Answer:
Watt-hour : If an elecrtrical machine of power one watt operates for one hour then one watt hour amount of energy is said to be spent.
1 watt-hour = 1 watt × 1 hour
= 1 watt × 3600 sec = 3600 J
Unit of electrical energy is watt-hour.

Question 17.
Define 1 kilowatt-hour ?
Answer:
If a machine of 1 kilo-hour operates for one hour the amount of energy spent is known as kilo-watt hour. This amount of energy is also known as Board of Trade Unit (B. O. T, units).

Question 18.
Why is nichrome wire used in electrically heated appliances ?
Answer:
(i) Explanation : Nichrome, an alloy of iron (24%), nickel (60%) and chromium (16%) was much larger resistance than copper and it is about 80 times. Thus, large quantity of heat produces when electricity flows through it. It neither melts nor gets oxidized even when it is red hot. For these reasons nichrome wire is used in most of electrically heated appliances.

Question 19.
What is short circuiting and what is overloading.
Answer:
Short circuiting : It means direct connection between the two terminals of a source of electricity or through a metallic wire of feeble resistance. As a result, large current flows through the connecting wire which melts due to overheating and therefore further flow of current stops.
Overloading : It is another dangerous effect which is caused by drawing excessive current when a number of high-powered electrical appliances are simultaneously switched on.

Question 20.
What is a fuse ? What is fuse rating ?
Answer:
Fuse : For the safety of the electrical gadgets one thin wire made of an alloy of lead (75 %) and tin (25%) and which has high resistance and low melting is kept in a insulator box of china clay. The thin coil is called fuse wire.
The wire is kept in series with the main circuit of the household electrical appliances.
If for some reason or other there is a surge of the current the household electical appliances may get burn. Under such condition the fuse wire melts and there by cut of the entire circuit and saves the domestic electrical equipments. Rating of fuse wire: The maximum current that may be allowed to flow through a fuse wire before it melts is called the rating of fuse wire.

Question 21.
What is earthing? How is a person saved from electric shock even if the live wire accidentally touches the metal body of an electric iron the person working with.
Answer:
Earthing : It means to connect a body or the metal case of an electrical appliance to the earth with the help of a metal wire, called, earth wire.
This wire protects a person using the appliance from electric shocks.
If the live wire by chance touches the metal part of an electrical appliance which has been earthed, the current passes directly to the earth through the earth wire.

Question 22.
What is Oersted’s experiment ?
Answer:
Oersted’s experiment : In this experiment, a conductor is held above and parallel to a freely rotatable pivoted magnetic needle. It is found that the magnetic needle deflects due to current flow in the conductor. The deflection increases with increase of current and it reverses when current is reversed.

Question 23.
State Ampere’s swimming rule.
Answer:
Ampere’s swimming rule : If a man be imagined to be swimming along a current carrying wire in the direction of the current (south to north) with his face turned towards a freely rotating magnetic needle, then the north pole of the needle will be deflected towards his left hand.

Question 24.
State Fleming’s left hand rule.
Answer:
Fleming’s left hand rule: If the thumb, the first finger and the middle finger of the left hand be held mutually perpendicular to each other in such a way that the first finger points in the direction of the magnetic field and the second finger to that of the current, then the thumb will indicate the direction at motion of the conductor.

Question 25.
Show how is Fleming’s left hand rule verified by Barlow’s wheel.
Answer:
Explanation : Barlow’s wheel is an arrangement to demonstrate action of magnet on current that verifies Fleming’s left hand rule.

According to the diagram, the current carrying conductor, the toothed wheel is situated in between the magnetic poles. So, when current is allowed to flow, the wheel rotates following Fleming’s left hand rule. On reversing the current the wheel rotates in oppsoite direction following the same rule.

Question 26.
On what factors does the relocing of rotation of Barlow’s wheel depend?
Answer:
Factors responsible for the speed of rotation :

1. Rotational speed increases with current and vice versa.
2. Rotational speed increases with intensity of magnetic field and vice versa.
3. If alternating current is used instead of Direct current, the wheel will try to reverse its direction with the change in direction of current resulting no rotation.

Question 27.
How can the direction of rotation of Barlow’s wheel be changed?
Answer:
Factors governing the direction of rotation of Barlow’s wheel :

1. The direction of rotation will reverse if direction of current is reversed keeping direction of magnetic field unchanged.
2. The direction of rotation will reverse if direction of magnetic field is reversed keeping direction of current unchanged.
3. The direction of rotation will remain unchanged in both direction of magnetic field and direction of current are reversed.

Question 28.
A bulb is marked ‘230 V-60 W’ what does it indicate?
Answer:
Explanation: When the bulb is used in an electrical line of potential difference 230 volts, 60 joules electrical Work per second is performed due to flow of electric current through the filament of the bulb.

Question 29.
What do you mean by the statement. ‘Potential difference between two points in an electric field is 5 volts’?
Answer:
Explanation: ‘Potential difference between two points in an electric field is 5 volts’- this statement means an external agent has to do 5 joules work to carry 1 coulomb positive charge from a point at lower potential to a point at higher potential in the electric field.

Question 30.
Why resistivity is also called specific resistance ?
Answer:
Explanation : Resistivity is also called specific resistance as resistivity of a material is the resistance offered by the material of specified dimensions unit length unit cross sectional area.

Question 31.
What is electric motor ?
Answer:
Electric Motor: The device or machine which converts the electrical energy into mechanical energy is known as Electric Motor.
An insulated copper coil, wound over a suitable frame rotates in a magnetic field when electric current passes through the coil.

Question 32.
How can the strength of the motor be increased ?
Answer:
The strength of an electric motor can be increased by :

1. increasing the current in the armature.
2. increasing the strength of magnetic field.
3. increasing the number of turns in the armature.

Question 33.
What is solenoid ?
Answer:

Solenoid: If many turns an insulated wire wound around a cylinder the resulting coil is known as solenoid. The soft iron body around which an insulated copper wire is coiled is known as the core of the electromagnet.

Question 34.
What is electromagnet ?
Answer:
Electromagnet: If soft iron is kept in a current carrying solenoid, then that soft iron behaves like a magnet so long as the current passes. This magnet is known as electromagnet.

Question 35.
How can the strength of electromagnet be increased ?
Answer:
The strength of electromagnet be increased by :

1. increasing the number of turns of solenoid.
2. increasing the current through the solenoid.
3. changing the core of the electromagnet.
4. if the core is ‘U’ shaped, then the distance between the poles is minimum.

Question 36.
State a few applications of eleciromagnet in daily life.
Answer:
Uses of electromagnets :

1. They are widely used in cranes for lifting and removing heavy beams etc. made of iron or steel in factories.
2. Physicians use special types of electromagent to remove small pieces of iron from the eye of a patient.
3. They are used in loudspeakers, receivers of telephone etc.

Question 37.
What is voltmeter ?
Answer:
Voltmeter : A voltmeter is used to measure the potential difference between two points in a section of an electrical circuit ; the voltmeter is connected parallel to the section.

Question 38.
What is ammeter ?
Answer:
Ammeter : It is used to measure the current flowing through an electric circuit where the ammeter is connected in series.

Question 39.
Why is e.m.f. (electromotive forces) of an electric cell is greater than p.d. (potential difference) ?
Answer:
Explanation : The difference of potential between two poles of a cell in open circuit is e.m.f. of the cell, the potential difference between the poles in closed circuit is p.d. (potential difference) of the cell. Now, in a closed circuit, a part of the e.m.f. is expended to overcome the internal resistance of the ce: is offered by the electrolyte of the cell. So, p.d. is less than the e.m.t. cell or e.m.f. is greater than p.d.

Broad Answer Type Questions

Question 1.
What is the difference between e.m.f. and p.d. ?
Answer:
Difference between e.m.f and p.d. :

e.m.f (Electromotive Foce)	p.d (Potential Difference)
i. It causes conversion of some other form of energy into electrical energy.	i. It causes conservation of electrical energy into some other form of energy.
ii. It is the potential difference across two terminals of an open circuit cell.	ii. It is the potential difference between two terminals of a closed circuit cell.
iii. The magnitude of e.m.f. is greater than p.d. in a cell.	iii. The magnitude of p.d. is lesser than e.m.f. in a cell.
iv. It is considered as the cause of p.d.	iv. Potential difference is the result/effect of e.m.f.
v. It does not depend on the resistance of the circuit.	v. Potential difference across any two points of a circuit depends on the resistance of that portion of the circuit.

Question 2.
State Joule’s laws of heating effect of current.
Answer:
Joule’s Laws (1841) :
(i) First law : The amount of heat produced in a conductor in a given interval of time is proportional to the square of the current passed. Thus if H be the amount of heat generated in a conductor having resistance R when current I passes through it in time t, then
H ∝ P² (when R and t are kept constant).

(ii) Second Law : The amount of heat produced by a given current in a given time is proportional of the resistance of the conductor.
H ∝ R (When I and t are kept constant)

(iii) Third Law : The amount of heat produced in a given conductor by a given current is proportional to the time for which the current passes.
H ∝ t (When I and R are kept constant)
Combining the three laws, we have
H ∝ I² R T (when I, R and t vary)
or, H = \(\frac{I^2 R T}{\mathrm{~J}}\)
(J = mechanical equivalent of heat = 4.2 joule/calorie)
If I be in ampere, R in ohm, t in second and H in calorie, then
H = \(\frac{I^2 R T}{4 \cdot 2}\)
∴ H = 0.24 F ² RT calorie

Question 3.
What is the difference between electromagnet and a natural or permanent magnet ?
Answer:
Difference between electromagnet and natural magnet :

Electromagnet	Natural magnet
i. The magnetism of this type of magnet almost disappears as soon as the current is stopped i.e. it is a temporary one.	i. If properly maintained magnetism of this type of magnet is almost permanent.
ii. It can be made very strong.	ii. It is usually not very strong.
iii. Strength of the magnet by changing the strength of the current.	iii. Strength of the magnet cannot be changed.
iv. By changing the number of turns per unit length of the coil, the strength of the magnet can be changed.	iv. Strength of the magnet cannot be changed.
v. By changing the direction of current polarity of the magnet can be easily reversed.	v. In this case polarity of the magnet cannot be reversed easily.

Question 4.
An electric heater works both in A.C. and D. C. lines but Barlow’s wheel works only in D. C.- Why ?
Answer:
Explanation Generation of heat in a resistor due to a current depends on magnitude of the current not on its direction. Moreover, the produced heat H ∝ I², so even if the oppositely directed current of A.C. be taken with negative direction, on being squared, it becomes positive. So, a heater can work both in A.C. and D.C.
the rotation of Barlow’s wheel in a given magnetic field depends upon the direction of current. The direction of rotation will reverse if direction of current is reversed keeping direction of magnetic field infact.
Now, in A.C., the direction of current reverses alternately and so frequently that, as soon as Barlow’s wheel is set to rotate in one direction, the reverse current flows into it tending to rotate it oppositely. This happens continuously and very frequently, so the wheel remains static.

Numerical Problems :

Example 1:
The resistance of a conductor is 100 hm; a current of 5 ampere is flowing through it. What will be the p.d. at the two ends of the conductor?
Answer:
R = 10 ohm
I = 5 ampere
V = p.d. = ?
We know,
V = RI
or, V = 10 × 5 = 50 volts

Example 2:
A current of 2A flows through a conductor. The p.d. across the conductor is 50 volts. What is the resistance?
Answer:
We know,
V = R I
or, R = \(\frac{V}{I}\) = \(\frac{50}{2}\)
I = 2 volts
R = 25 ohm

Example 3:
10 ampere current is allowed to a conductor for 1 minute. Find the amount of charge flown.
Answer:
I = 10 ampere
t = 1 minute = 60 sec
Q = ?
We know,
Q = I × t
or, Q = 10 × 60 = 600
∴ Q = 600 coulomb

Example 4:
Potential difference across two points of a conductor is 60 volts. Resistance of the conductor is 10 ohm. Find the’current through the conductor.
Answer:
V = 60 volts
R = 10 ohm
I = ?
We know,
V = R I
or, I = \(\frac{V}{R}\) = \(\frac{60}{10}\) = 6
or, I = 6 ampere

Example 5:
A current of 2 ampere is passed through a conductor of resistance 4 \mathrm{ohm}. Find the potential difference across the conductor.
Answer:
I = 2 unit
R = 2 unit
V = ?
We know,
V = I × R
or, V = 2 × 4 = 8
∴ V = 8 volts

Example 6:
Resistance of one conductor is double that of the other. What will be the ratio of current through these two conductor if they are subjected to same potential difference.
Answer:
Let the resistance of the conductors are R and 2 R. Let both of them are subjected to same potential difference of V. So, naturally currents in the conductors will be as follows :

Example 7:
2 units of current is flowing through a conauctor or of 2 units. What is the potential difference at the ends of the conductor?
Answer:
I = 2 ampere
R = 4 ohm
V = ?
We know,
V = R . I
or, V = 2 × 2 = 4 unit

Example 8:
The resistance per metre of a wire is 1.2 ohm and its specific resistance is 60.28 × 10^-8 ohm-m. Find the radius of the wire.
Answer:
R = 1.2 ohm
I = 1 meter
ρ = 60.28 × 10^-18ohm-m
A = ?
We know,
R = ρ \(\frac{1}{A}\) or, A= \(\frac{\rho l}{R}\)
or, A = \(\frac{60 \cdot 28 \times 10^{-8} \times 1}{1 \cdot 2}\)
∴ A 50.2 × 10^-8 m²
Again, if r be the radius of the wire,
πr² = A = 50.2 × 10^-8 or, r²=\(\frac{50 \cdot 2 \times 10^{-8}}{3 \cdot 14}\) 16× 10^-8 m²
∴ r = 4 × 10^-14 m = 0.04 cm

Example 9:
There are two copper wires of equal length. The radius of one is twice the other. Find the ratio of their resistances.
Answer:
r = radius of the wire
We know,

∴ The thinner wire has a resistance four times the resistance of the thicker wire.

Example 10:
The resistivity of a substance is 9 \times 10^-8 \mathrm{ohm} . \mathrm{m}. What length of the wire of that material, having diameter 0.3 cm} will give a resistance of 100 \mathrm{ohm} ?
Answer:
We know,

Example 11:
The resistance of wire of cross-section area 0.01 cm² is 10 ohm. What is the length of the wire? The specific resistance of the wire is 50 × 10^-6 ohm-cm.
Answer:
We know,
R = 10 ohm
A = 0.01 cm²
ρ = 50 × 10^-6 ohm-cm
l = ?
R = ρ \(\frac{1}{A}\) or, l = \(\frac{RA}{\rho}\)
or, l = \(\frac{10 \times 0.01}{50 \times 10^{-6}}\)
∴ l = 2000 cm

Example 12 :
The length and area of cross-section of a wire are double of these of another wire of same material. Find the ratio of their resistances.
Answer:
Let the length of wires be 2 l and l and their areas of cross. Section be 2 A and A respectively. If \rho be the resistivity of the material of the wires, then their resistance R₁ and R₂ will be given by
R₁= \(\frac{\rho 2 l}{2 A}\) and R₂ = \(\frac{\rho l}{A}\)
∴ \(\frac{R_1}{R_2}\) = \(\frac{1}{1}\) or, R₁ : R₂ = 1 : 1

Example 13 :
Find the specific resistance of the material of a wire of length 100 cm, area of cross-section 0.2 cm2 and resistance 2 ohm.
Answer:
R = 2 ohm
l = 100 cm
A = 0.2 cm²
ρ = ?
R = ρ × \(\frac{1}{A}\)
∴ ρ = \(\frac{R A}{l}\) = \(\frac{2 \times 0.2}{100}\) =40 ×s 10^-4 ohm-cm

Example 14 :
Three resistors 1 ohm, 2 ohm and 3 ohm are connected in parallel. What will be their equivalent resistance?
Answer:
We know, for parallel combination,

Example 15 :
Three wires of resistance 2 ohm, 3 ohm and 5 ohm are connected in series with a cell of e.m.f. 5 volt. What will be the current through each wire?
Answer:
We know, for series combination the equivalent resistance
R = r₁ + r₂ + r₃ = 2 + 3 + 5 = 10 ohm
We also know,
I = \(\frac{V}{R}\) = \(\frac{5}{10}\) = 0.5 A

Example 16 :
Find effective resistance of the resistors 2 ohm, 4 ohm, 5 ohm connected in (i) series and (ii) parallel.
Answer:
We know, for series combination equivalent resistance
R = r₁ + r₂ + r₃ = 2 + 4 + 5 = 11 ohm
We also know, for parallel combination equivalent resistance

Example 17 :
In a circuit 2 ohm and 3 ohm resistors are connected in series to the parallel arrangement of 2 ohm and 3 ohm resistors. Calculate the resistance of the circuit.
Answer:
Let R be the equivalent reistance of 2 ohm and 3 ohm arranged in parallel.
So, \(\frac{1}{R}\) = \(\frac{1}{2}\) + \(\frac{1}{3}\) = \(\frac{5}{6}\)
∴ \(\frac{1}{R}\) = \(\frac{5}{6}\) or, R = \(\frac{6}{5}\) = 1.2 ohm
Now, 2 ohm and 3 ohm resistors are connected in series with 1.2 ohm. So, the resistance of the circuit = (2 + 3 + 1.2) ohm = 6.2 ohm.

Example 18 :
A current of 0.5 ampere passes through a wire of resistance 2.5 ohm for 1 hour. Find the heat produced.
Answer:
I = 0.5 ampere
R = 2.5 ohm
t = 1 hr = 3600 sec
H = ?
We know, H = \(\frac{I^2 R T}{J}=\frac{I^2 R T}{4 \cdot 2}\)
∴ H=\(\frac{(0.5)^2 \times 2.5 \times 3600}{4.2}\) = 535.7 calorie

Example 19 :
Two electric bulbs marked 220V-60W are used daily for 5 hours for 10 days. If the price of each unit of electrical energy be 65 paise. What will be the cost for it ?
Answer:
From the problem we get, Total power of the two bulbs = 2 × 60 watt =120 watt
Electrical energy consumed per day = 120 watt × 5 hour = 600 watt-hour
∴ Total energy consumed in 10 days = 600 × 10 = 6000 watt hour
= \(\frac{6000}{1000}\) = 6 kilo watt-hour = 6 B.O.T. unit
∴ cost of electrical energy at 65 paise per unit = 6 × 65 paise = Rs. 3.90

Example 20 :
The same current passes for the same time through two wires the resistance of one is double that of the other. What is the ratio of quantities of heat developed in the two wries?
Answer:
Let the resistances of the wires be 2 R and R and the quantities of heat produced in them be H₁ and H₂respectively. Then from Joule’s second law we get,
\(\frac{H_1}{H_2}=\frac{2 R}{R}=\frac{2}{1}\) or, H₁: H₂ = 2: 1

Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 8.4 Inorganic Chemistry in the Laboratory and in Industry offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 8.4 Question Answer – Inorganic Chemistry in the Laboratory and in Industry

A. Ammonia

Very Short Answer Type Questions

Question 1.
Name the chemicals required for the preparation of ammonia in laboratory
Answer:
Chemicals required :

• Ammonium chloride (NH₄Cl)
• Quick lime (CaO) or dry slaked lime [Ca(OH)₂]

Question 2.
What is the characteristic smell of ammonia ?
Answer:
Characteristic smell of ammonia Pungent

Question 3.
What is the nature of aqueous solution of ammonia ?
Answer:
Nature of aqueous solution of ammonia : alkaline

Question 4.
State one method for identification of ammonia.
Answer:
Ammonia has a typical pungent smell.

Question 5.
Which particular substance is used to dry ammonia gas ?
Answer:
Ammonia is dried with calcium oxide (CaO).

Question 6.
What colour is obtained when ammonia burns in presence of oxygen?
Answer:
Ammonia burns in presence of oxygen with a greenish yellow flame forming nitrogen and water.
4NH₃ + 3O₂ = 2N₂ + 6H₂O

Question 7.
What is Nessler’s reagent ?
Answer:
Nessler’s reagent Nessler’s reagent is an alkaline solution (KOH) of po­tassium mercuric iodide [K₂Hgl₄]

Question 8.
What happens when red litmus paper is placed in aqueous solution of ammonia ?
Answer:
The aqueous solution of ammonia is basic in nature so it turns red litmus to blue.

Question 9.
State one use of ammonium sulphate.
Answer:
Use of ammonium sulphate : as fertilizer.

Question 10.
What is the amount of ammonia present in liquor ammonia ?
Answer:
35% (by weight)

Question 11.
Is ammonia heavier or lighter than air ?
Answer:
Ammonia is lighter than air.
[Vapour density of air = 144 ; vapour density of ammonia = 8-5 ]

Question 12.
State one use of liquid ammonia.
Answer:
Use of liquid ammonia : as a refrigerant in ice making.

Question 13.
Give an example of formation of solid by the combination of two gases.
Answer:
Ammonia gas reacts with hydrogen chloride gas forming solid ammonium chloride.
NH₃(gas) + HCl (gas) = NH₄Cl (solid)

Question 14.
How is ammonia collected in laboratory ?
Answer:
Collection of ammonia Ammonia is lighter than air, it may be collected by the downward displacement of air.

Question 15.
What colour is obtained when ammonia reacts with Nessler’s reagent?
Answer:
Ammonia produces brown colouration in Nessler’s reagent.

Question 16.
Which compound of nitrogen has fractional oxidation number ?
Answer:
Hydrazoic acid (HN₃)
Nitrogen has \(\left(-\frac{1}{3}\right)\) oxidation number in hydrazoic acid.

Question 17.
Which hydride of nitrogen has no oxidising property ?
Answer:
Ammonia has no oxidising property.

Question 18.
Which gas is obtained when a mixture of ammonium sulphate and sodium hydroxide is heated ?
Answer:
Ammonia (NH₃) gas.

Question 19.
How ammonium sulphate is obtained without using sulphuric acid ?
Answer:
CaSO₄ + 2NH₃ + CO₂ + H₂O = CaCO₃ + (NH₄)₂SO₄

Question 20.
Two gaseous compounds of nitrogen react with each other to form nitrogen. What are the two gaseous compounds of nitrogen ?
Answer:

Short answer type questions

Question 1.
Why is conc. H₂SO₄ not used for drying ammonia gas ?
Answer:
Ammonia is a basic compound. So it forms salt with cone. H₂SO₄.
For this reason cone. H₂SO₄ is not used for drying ammonia gas.
2NH₃ + H₂SO₄ = (NH₄)₂SO₄

Question 2.
Why is anhydrous CaCl₂ not used for drying ammonia gas ?
Answer
Ammonia forms an additive compound with anhydrous CaCl₂.
CaCl₂ + 8NH₃ = CaCl₂, 8NH₃ (additive compound)

Question 3.
Why is P₂O_s not used for drying ammonia gas ?
Answer:
Ammonia is a basic compound. P₂O_s is an acidic oxide. So it forms salt with P₂O₅ SO P₂O₅ is not used for drying ammonia gas.
6NH₃ + P₂O_s + 3H₂O = 2(NH₄)₃PO₄

Question 4.
Why CaO is used for drying agent of ammonia ?
Answer:
CaO is used for drying agent of ammonia : Ammonia is a basic com­pound. It is dried of using a basic drying agent i.e. Quick lime (CaO) which has no action on ammonia.

Question 5.
What is liquor ammonia ?
Answer:
Liquor ammonia A saturated (35% by weight) aqueous solution of am­monia (sp. gr. = 088) is called liquor ammonia.

Question 6.
Prove that ammonia has reducing property.
Answer:
Reducing property of ammonia : When ammonia is passed over strongly heated black cupric oxide which is reduced to red metallic copper and am­monia is oxidised to nitrogen.

Question 7.
State about solubility of ammonia in water.
Answer
Solubility of ammonia is water : Ammonia is highly soluble in water. One volume of water can dissolve about 1299 volumes ammonia at N.T.P A concentrated aqueous solution of ammonia is called ammonia.

Question 8.
What are the differences between liquid ammonia and liquor ammonia ?
Answer
Difference between liquid ammonia and liquor ammonia :
There is a sharp difference between liquid ammonia and liquor ammonia. The first one is the liquified ammonia gas which has formula NH₃, while the second one is the concentrated solution of ammonia which has formula NH₄OH.

Question 9.
How will you prove that ammonia contains nitrogen ?
Answer
Ammonia contains nitrogen : Ammonia gas when passed over heated cupric oxide produces colourless gas having no smell.
3CuO + 2NH₃ = 3Cu + 3H₂O + N₂
When the colourless gas is passed over heated magnesium, magnesium nitride (Mg₃N₂), the white powder produces.
3Mg + N₂ = Mg₃N₂
When the white powder is boiled with water it will produce pungent smell gas NH₃
Mg₃N₂+ 6H₂O = 3Mg(OH)₂ + 2NH₃↑
This reaction proves that the colourless gas is nitrogen. This reaction also proves that one of the constituents of ammonia is nitrogen.

Question 10.
What precautions should be taken to combat the effect of ammonia leaked from industries and ammonia tanks ?
Answer
Precautions for ammonia If accidentally, ammonia gas leaks from indus­tries and ammonia tanks, heavy shower of water should be applied in the atmosphere that is filled with the leaked gas. If at any time, tanks filled with ammonia gas are required to be shifted somewhere, the carrier of tanks must also carry plenty of water that may be used to spray in the air filled with accidental leakage of ammonia gas.

Question 11.
How does ammonia react with sodium ?
Answer
Reaction of ammonia with sodium Heated sodium metal at 400°C reacts with ammonia producing sodamide and hydrogen gas.
2NH₃ + 2Na = 2NaNH₂ + H₂↑
This reaction proves that ammonia contains hydrogen.

Question 12.
How does ammonia react with chlorine ?
Answer
Reaction of ammonia with chlorine : Ammonia reacts with chlorine in two ways.
(i) When ammonia is excess : Excess ammonia is oxidised by chlorine forming nitrogen and is reduced to hydrochloric acid. Hydrochloric acid thus formed combines with ammonia producing ammonium chloride.

(ii) When chlorine is excess : When excess chlorine reacts ammonia forming nascent nitrogen which again combines with chlorine producing nitrogen trichloride, an oily yellow explosive compound.
NH₃ + 3Cl₂ = 3HCl + NCl₃

Question 13.
Show with an equation what happens when ammonia is burnt in oxygen.
Answer:
Ammonia is burnt in oxygen Ammonia is neither combustible nor a supporter of combustion. But ammonia burns in presence of oxygen with a greenish yellow flame forming nitrogen and water.
4NH₃ + 3O₂ = 2N₂↑ + 6H₂O

Question 14.
How does aqueous ammonia react with aluminium chloride and ferric chloride solutions ?
Answer:
(i) Reaction of aqueous ammonia with aluminium chloride solution: Aqueous solution of ammonia (NH₄OH) reacts with aluminium chloride forming white gelatinus precipitate of aluminium hydroxide.
AlCl₃ + 3NH₄OH = Al(OH)₃↓(white) + 3NH₄Cl

(ii) Reaction of aqueous ammonia with ferric chloride solution :
Aqueous solution of ammonia (NH₄OH) reacts with ferric chloride solution forming brown precipitate of ferric hydroxide.
FeCl₃ + 3NH₄OH = Fe(OH)₃↓(brown) + 3NH₄Cl

Question 15.
State with reasons two precautions taken during preparation of ammonia in laboratory.
Answer:
Precautions taken during preparation of ammonia in laboratory :

• The components ammonium chloride (NH₄Cl) and calcium hydroxide [Ca(OH)₂] should be dry to avoid evolution of ammonia while mixing the two.
• The mixture of the components should fill about half the flask to leave enough space for easy passage of the evolved gas.

Question 16.
State some uses of ammonia.
Answer:
Uses of ammonia :

• It is used for the industrial preparation of nitric acid and sodium carbonate.
• Large quantities of ammonia are used in the manufacture of fertilizers, such as urea, ammonium phosphate etc.
• Ammonia is used as solvent.
• Liquid ammonia is used as a refrigerant in ice making.
• Ammonia is used as laboratory reagent.
• It is also used in pharmaceutical industries and also in the preparation of smelling salt.

Question 17.
Give an example of formation of a solid by combination of two gases.
Answer:
Formation of a solid by combination of two gases : Ammonia gas reacts with hydrogen chloride gas forming a solid ammonium chloride. This is an example of formation of a solid by the combination of two gases.
NH₃ (gas) + HCl (gas) = NH₄Cl (solid)

Question 18.
State how does ammonia react with HCl, H₂SO₄, HNO, acids.
Answer:
Reaction of ammonia with acids : Ammonia is a base, it readily reacts with an acid to form salt.
NH₃ + HCl = NH₄Cl
2NH₃ + H₂SO₄ = (NH₄)₂SO₄
NH₃ + HNO₃ = NH₄NO₃
Aqueous solution of ammonia reacts with acids to form salt and water.
NH₄OH + HCl = NH₄Cl(salt) + H₂O₃
2NH₄OH + H₂SO₄ = (NH₄)₂SO₄(salt) + 2H₂O
NH₄OH + HNO₃ = NH₄NO₃(salt) + H₂O

Question 19.
How is urea obtained from ammonia?
Ans. Preparation of urea from ammonia: Ammonia reacts with carbon dioxide at 200°C and 150 atm pressure to form urea.
CO₂ + 2NH₃ = CO(NH₂)₂ (urea) + H₂O

Question 20.
How does aqueous ammonia react with copper sulphate solution?
Answer:
Reaction of aqueous ammonia with copper sulphate solution When aqueous ammonia i.e. ammonium hydroxide is slowly added to a copper sul­phate solution, a pale blue precipitate of basic copper sulphate is first formed. On adding excess of ammonium hydroxide, the precipitate dissolves forming a deep solution of the complex compound called copper tetramine sulphate.
2CuSO₄+ 2NH₄OH = CuSO₄. Cu(OH)₂ + (NH₄)₂SO₄
CuSO₄ .Cu(OH)₂ + 6NH₄OH + (NH₄)₂SO₄ = 2[Cu(NH₃)SO₄+ 8H₂O

Broad Answer Type Questions

Question 1.
How ammonia is prepared in laboratory ?
Answer:
Laboratory preparation of Ammonia :
(a) Chemicals required : Ammonium chloride (NH₄Cl) and quick lime (CaO) or dry slaked lime [Ca(OH)₂

(b) Condition Normally ammonia gas is obtained in the laboratory by heating a mixture of ammonium chloride with slaked lime. Instead of using slaked lime quick lime may also be used. NH₄>Cl, Ca(OH)₂ or CaO should be in powdered form and dry. The round bottomed flask should be half filled with the mixture of the two for easy escape of ammonia gas formed.

(c) Collection Ammonia is lighter than air, it may be collected by the downward displacement of air. Ammonia is not collected through the downward displacement of water because, it is highly soluble in water.

(d) Equations of the reaction :
2NH₄Cl + Ca(OH)₂ = 2NH₃↑+ CaCl₂ + 2H₂O
2NH₄Cl + CaO = 2NH₃↑ + CaCl₂ + H₂O

(e) Precautions : The ingradients, the test-tube, the delivery pipes and the gas-jar should be absolutely dry. All the connections in the apparatus should be leak-proof.

(f) Drying of ammonia : As ammonia is a basic substance, it cannot be dried by acidic drying agents like cone. H₂SO₄ or P₂O_s. The gas is absorbed by fused CaCl₂ with the formation of an addition compound CaCl₂.8NH₃. So, fused CaCl₂ cannot be used to dry ammonia. It is best dried with the basic drying agent, quick lime (CaO).

Question 2.
Prove by experiment that ammonia is dissolved in water and produces alkaline solution.
Answer:
Fountain experiment :
Arrangement of the experiment : A flask is filled with dry ammonia gas and its mouth is corked. The flask is kept in inverted position and is damped to a stand. Through a hole in the cork one end of a glass tube is introduced inside the flask. This end of the tube inside the flask is shaped into a jet. The other end of the tube dips in some red litmus solution taken in a beaker.

Operation : Now ice or ether is poured upon the flask.

Observation : A blue fountain produces inside the flask.

Explination Due to evaporation of ether the flask is cooled. Ammonia gas inside the flask contracts, as a result there is a partial vacuum inside the flask. At this stage if stop cock is opened the red litmus solution rushes inside the flask and ammonia is dissolved in it. Due to vaccum created inside there is a formation of fountain and the solution becomes blue.

Conclusion : This experiment proves that ammonia is highly soluble in water and the aqueous solution is alkaline.

Question 3.
How is ammonia identified ?
Answer:
Identification of ammonia :
(a) Ammonia is easily detected by its pungent smell.

(b) A glass rod dipped in into hydrochloric acid is then held into ammonia a white fumes is observed due to formation of ammonium chloride.
NH₃ + HCl = NH₄Cl (white fumes)

(c) Ammonia turns moist red litmus paper into blue.

(d) Ammonia produces brown colouration or precipitate in Nessler’s reagent.

(e) A strip of filter paper, soaked in mercurous nitrate solution, when exposed to ammonia gas, turns black.

B. Sulphuretted Hydrogen (H₂S)

Very Short answer type questions 

Question 1.
Which acid is used to prepare H₂S gas in laboratory ?
Answer:
Dilute sulphuric acid.

Question 2.
During preparation of H₂S gas in laboratory, how Is the gas collected?
Answer:
By upward displacement of air.

Question 3.
What happens when H₂S gas is passed through acidified yellow ferric chloride solution ?
Answer:
Yellow ferric chloride solution reduces to colourless ferrous chloride solution.

Question 4.
How is H₂S gas dried In laboratory preparation ?
Answer:
By passing the gas through phosphorus pentoxide (P₂O₅).

Question 5.
How does H₇S gas smell ?
Answer:
It has a smell of rotten egg.

Question 6.
How does H₂S gas react with blue litmus ?
Answer:
It turns blue litmus red.

Question 7.
What gas is used in detecting metallic radical in laboratory ?
Answer:
Sulphuretted hydrogen (H₂S)

Question 8.
Is H₂S gas heavier or lighter than air ?
Answer:
H₂S gas is heavier than air.

Question 9.
Is H₇S combustible or a supporter of combustion ?
Answer:
H₂S is a combustible gas.

Question 10.
Why is an old silver made substance turned to black ?
Answer:
Due to formation of silver sulphide (Ag₂S).

Question 11.
What is the common use of hydrogen sulphide in laboratory ?
Answer:
For the identification of basic radical (metal ion).

Question 12.
Name the chemicals required for preparation of H₂S in laboratory.
Answer:
Chemicals required for preparation of H₂S :

• Ferrous sulphide (FeS)
• Dilute sulphuric acid (H₂SO₄)

Question 13.
Is HCl acid suitable for preparation of H₂S ?
Answer:
No. As HCl is very volatile.

Question 14.
Mention one identifying test for H₂S.
Answer:
Lead acetate paper turns black when it is held in H₂S gas.

Question 15.
What is the density of H₂S at NTP ?
Answer:
Density of H₂S gas is 1-53 g/L at NTP

Question 16.
Give the name of a gas which is soluble in cold water but insoluble in hot water.
Answer:
Hydrogen sulphide (H₂S)

Question 17.
Which gas is used to identify basic radical ?
Answer:
Hydrogen sulphide (H₂S)

Question 18.
What happens when H₂S gas is passed through a blue coloured solution of CuSO₂ ?
Answer:
Black precipitate of CuS is formed.

Question 19.
Is H₂S acidic or basic gas ?
Answer:
H₂S is acidic gas.

Question 20.
How many types of salts are formed by H₂S ?
Answer:
Since H₂S is a bibasic acid, it gives two types of salt, one is acid salt and other is normal salt.

Question 21.
Give the name of a poisonous gas.
Answer:
Hydrogen sulphide (H₂S).

Short Answer Type Questions

Question 1.
Name the chemicals required for preparation of H₂S in laboratory. Write down the equation of reaction.
Answer:
Chemicals required for preparation of H₂S in laboratory :
Ferrous sulphide (FeS) and dilute sulphuric acid (H₂SO₄)
Equation : FeS + H₂SO₄ = FeSO₄ + H₂S↑

Question 2.
Is HCl acid suitable for preparation of H₂S ? Give reason.
Answer:
HCl acid is not suitable for preparation of H₂S.
Cause : HCl acid is not chosen due to volatile nature of HCl. During the preparation, HCl vapour that may be formed will accompany the evolved H₂S and will make it impure.

Question 3.
Is HNO₃ acid suitable for preparation of H₂S? Give reason.
Answer:
HNO₃ acid is not suitable for preparation of H₂S.
Nitric acid cannot be used in the preparation, because it is an oxidising agent and H₂S is a reducing agent. Nitric acid will oxidise H₂S to sulphur and will thus hamper the reaction.

Question 4.
Mention one identifying test for H₂S.
Answer:
Identification of H₂S: Hydrogen sulphide is passed through a solution of sodium hydroxide solution and then sodium nitroprusside solution is added to it. The solution turns violet.

Question 5.
How does H₂S react with cone. HNO_a?
Answer:
Reaction of H₂S with cone HNO₃ :
H₂S-reduces cone. HNO₃ to brown nitrogen dioxide (NO₂) and is itself oxidised to sulphur.
Equation : H₂S + 2HNO₃ = 2NO₂↑ + S↓+ 2H₂O

Question 6.
How does H₂S react with cone. H₂SQ₄ ?
Answer:
Reaction of H S with cone. H₂SO₄ : H₂S) reduces cone. H₂SO₄ to SO₂ and is itself oxidised to sulphur.
Equation : H₂S + H₂SO₄ = SO₂↑ + S↓ + 2H₂O

Question 7.
Write down the reaction of H₂S with NaOH.
Answer:
Reaction of H₂S with NaOH : H₂S reacting with NaOH produces acid salt in the first step and normal salt in the second step along with water in both the steps.

Question 8.
Which substance is used for drying H₂S and why ?
Answer:
Drying of H₂S gas : The most suitable drying agent for H₂S is the acidic oxide P₂O₅, that does not react with H₂S which is also of acidic nature.

Question 9.
What is the density of H₂S and state about its solubility in water at ordinary temperature and in hot water.
Answer:
Density of H₂S : Density of the gas is T53 g/L at NTR
Solubility of H₂S in water : It is moderately soluble in water at ordinary temperature but insoluble in hot water.

Question 10.
What happens when H₂S is burnt in small and excess supply of oxygen ?
Answer:
H₂S is burnt in small supply of oxygen : During burning of H₂S if the supply of oxygen is low, the gas burns with a blue flame and deposits sulphur. 2H₂S + O₂ = 2S↓ + 2H₂O
H₂S is burnt in excess supply of oxygen : In an excessive supply of oxygen the gas burns with a blue flame and produces sulphur dioxide and water.

Question 11.
Show that H₂S is a reducing agent.
Answer:
Reducing property of H₂S : Hydrogen sulphide is a very good reducing agent. H₂S reduces acidified yellow solution of ferric chloride to colourless ferrous chloride.

Question 12.
What happens when H₂S is passed through acidified solution of FeCl_a?
Answer:
Yellow ferric chloride solution is reduced by H₂S giving rise colourless ferrous chloride and H₂S itself on oxidation gives a precipitate of sulphur.
Equation : 2FeCl₃ + H₂S = 2FeCl₂ + 2HCl + S₄

Question 13.
What happens when H₂S is passed through acidified solution of CuSO₄?
Answer:
If H₂S is passed through acidified blue coloured solution of CuSO₄ then black precipitate of cupric sulphide (CuS) is formed.
Example:

Question 14.
What happens when H₂S is passed through acidified solution of Pb(NO₃)₂
Answer:
If H₂S is passed through acidified colourless solution of Pb(NO₃)₂ then black precipitate of lead sulphide (PbS) is formed.
Example:

Question 15.
What happens when H₂S comes in contact with a paper soaked in lead acetate ?
Answer:
A paper soaked in lead acetate [Pb(CH₃COO)₂] turns black with H₂S gas due to formation of black lead sulphide (PbS).
Equation:

Question 16.
Mention the uses of hydrogen sulphide.
Answer:
Uses of hydrogen sulphide :

• H₂S is used as a reagent in the separation of metal ions in group analysis.
• H₂S is sometimes used as a reducing agent.

Broad answer type questions

Question 1.
Describe laboratory method of preparation of H₂S with the points:
(i) chemicals required
(ii) condition
(iii) equation of reaction
(iv) drying agent
(v) collection
Answer:
(i) Chemicals required Ferrous sulphide (FeS) and dilute sulphuric acid (H₂SO₄)
(ii) Condition Hydrogen sulphide is prepared in the laboratory by the action of dil. H₂SO₄ on pieces of ferrous sulphide (FeS) at ordinary temperature.
(iii) Equation of reaction : FeS + H₂SO₄ = FeSO₄ + H₂S↑
(iv) Drying agent The gas is passed through P₂O₅ to dry it.
(v) Collection : Because the gas is heavier than air it is collected over the upward displacement of air.

Question 2.
What precautions should be taken during preparation and handling of H₂S ?
Answer:
Precautions taken during preparation of H₂S : Hydrogen sulphide is a poisonous gas and is harmful at concentrations above 0-1% by volume in air. So, due precautions should be taken not to inhale the gas not to allow its prolonged contact with skin during handling.

During preparation of the gas caution must be taken so that excessive gas does not spread in the atmosphere of laboratory. To do this, sulphuric acid should be added in the wolfe’s bottle in small quantities and in steps.

C. Nitrogen

Very short answer type questions

Question 1.
Name the chemicals used In laboratory method of preparation of nitrogen.
Answer:
Chemicals required : Ammonium chloride (NH₄Cl) and sodium nitrite (NaNO₂).

Question 2.
State what you know about solubility of nitrogen in water.
Answer:
Solubility of nitrogen in water is about 23-5 ml/L at NTR It is almost half that of oxygen.

Question 3.
What is the density of nitrogen?
Answer:
Density of nitrogen 125 g/L at NTR

Question 4.
How is nitrogen prepared in laboratory dried?
Answer:
Nitrogen has is dried by passing the gas through concentrated sulphuric acid (H₂SO₄).

Question 5.
What is the percentage of nitrogen in air by volume?
Answer:
Percentage of nitrogen in air by volume : 77 17%

Question 6.
What would happen if there were no nitrogen in the atmosphere?
Answer:
In absence of nitrogen burning in atmosphere would be vigorous and uncontrollable.

Question 7.
What is the use of liquid nitrogen?
Answer:
Liquid nitrogen (b.p.-195’8°C) is used to produce low temperature in scientific research.

Question 8.
Is nitrogen heavier or lighter than air?
Answer:
Nitrogen is slightly lighter than air.

Question 9.
Give a name of nitrogen containing inorganic fertilizer.
Answer:
Nitrogen containing inorganic fertilizer : Ammonium nitrate (NH₄NO₃).

Question 10.
Which gas is used in gas-thermometer?
Answer:
Nitrogen gas is used in gas-thermometer.

Question 11.
Which gas is used in electric bulb?
Answer:
Nitrogen gas is used in electric bulb.

Question 12.
What is nitrogen trihydride?
Answer:
Nitrogen trihydride is ammonia

Question 13.
Which gas is presentjarge amount in atmosphere?
Answer:
Nitrogen gas is present large amount in atmosphere.

Question 14.
What is nitrolim?
Answer:
Nitrolim : Mixture of calcium cyanamide and carbon is known as nitrolim.

Question 15.
Which gas is used to create inert atmosphere during^hemical reactions.
Answer:
Nitrogen gas is used to create inert atmosphere during chemical reactions.

Question 16.
What are the two essential gaseous components of the atmospheric air ?
Answer:
Two essential gaseous components are :
(i) Oxygen
(ii) Nitrogen

Question 17.
Which plants absorb nitrogen directly from air ?
Answer:
A few leguminous plants such as pea, bean, clover etc. can absorb nitrogen directly from air.

Question 18.
What are the ways of fixation of nitrogen?
Answer:
There are two ways of fixation of nitrogen:
By electric discharge
Bio-chemical reaction through bacteria.

Short Answer Type Questions

Question 1.
How does nitrogen react with oxygen?
Answer:
Reaction of nitrogen with oxygen : Nitrogen reacts with oxygen forming nitric oxide under the influence of electric arc at a temperature of 3000°C.
\(\mathrm{N}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO} \text { – heat (Endothermic reaction) }\)

Question 2.
Why Is the solution of ammonium chloride and sodium nitrite is heated to produce nitrogen instead of heating ammonium nitrite directly?
Answer:
Nitrogen gas is not prepared by heating ammonium nitrite (NH4NO2) directly, for in that case rapid explosive dissociation of ammonium nitrite takes place.

Question 3.
How does nitrogen react with magnesium ?
Answer:
Reaction with magnesium : When turnings of magnesium metal are strongly heated in nitrogen gas, the metal directly combines with nitrogen to form magnesium nitride
(Mg₃N₂).
3Mg + N₂ = Mg₃N₂

Question 4.
What happens if magnesium nitride is boiled with water ?
Answer:
Magnesium nitride is boiled with water to form magnesium hydroxide and ammonia.
Mg₃N₂ + 6H₂O = 3Mg(OH)₂ + 2NH₃ 

Question 5.
What is nitrolim? How it is formed? Mention its important use.
Answer:
Nitrolim: When small lumps of white calcium carbide (CaC₂) are heated in nitrogen gas at about 1100°C, calcium cyanamide (CaNCN) is formed, along with the separation of carbon particles (black). The blackish brown mixture of the products (CaNCN + C) is commercially known as nitrolim. Use of nitrolim : It is largely used as a fertilizer.

Question 6.
State the uses of nitrogen.
Answer:
Uses of nitrogen :

• It is used in the industrial preparation of ammonia and nitric acid.
• It is used for the production of fertilizer, such as ammonium sulphate, am­monium nitrate.
• Liquid nitrogen (b.p. -195’8°C) is used as condenser.
• In many chemical reactions, nitrogen is used as inert medium.
• It is used in the preparation of electric bulb and gas thermometer.

Question 7.
Why gaseous nitrogen is chemically quite inactive at ordinary temperatures, but it is active at higher temperatures ?
Answer:
Chemical nature of gaseous nitrogen : The unreactivity of nitrogen at ordinary temperatures, is due to the structure of nitrogen molecule (N₂), in which two nitrogen atoms are bonded together by three covalent bonds (N ≡ N). The force of attraction of two nitrogen atoms so bonded is very high. So large amount of energy (generally heat energy) is required to break up this bond to set free the two nitrogen atoms so that they can enter into chemical combination.

Question 8.
State the physical properties of nitrogen.
Answer:
Physical properties of nitrogen :

• It is colourless gas without smell or taste,
• Density of the gas is 1.25 g/L at NTR
• It is slightly soluble in water.
  Solubility of nitrogen in water is about 23-5 ml/L at NTR

Broad Answer Type Questions 

Question 1.
Describe the laboratory method of preparation of nitrogen. State the following matters :
(a) chemicals required
(b) condition
(c) drying
(d) chemical equation
(e) collection of gas.
Answer:
Laboratory method of preparation of nitrogen :
(a) Chemicals required :

• Sodium nitrite (NaNO₂)
• Ammonium chloride (NH₄Cl)

(b) Condition : The chemicals ammonium chloride and sodium nitrite must not be in solid state but as solution. The mixture is heated gently to evolve nitrogen gas.

(c) drying : The nitrogen gas is dried by passing through a U-tube containing cone., sulphuric acid.

Chemical equation:

(e) Collection of gas : Though nitrogen gas is slightly soluble in water, it is collected by the downward displacement of water.

Question 2.
State briefly the significance of the presence of nitrogen in air.
Answer:
Significance of the presence of nitrogen in air : Nitrogen in air dilutes oxygen present therein. Oxygen is a very active oxidant. The mixture of nitrogen with oxygen in air moderates the intense activity of pure oxygen in the processes of respiration, combustion etc, which would have otherwise occurred very rapidly.

The intake of only oxygen during respiration would have caused increased rate of respiration, causing excessive burning of body tissues. This would have caused high and unchecked rise in the temperature of body, which results death. Without nitrogen in air, the combustion of earthly materials would have been explosively vigorous.

The huge amount (about 78% by volume) of nitrogen in air can be ab­sorbed by certain symbiotic bacteria, such as Rhizobium leguminouserum, R. japonicum etc. Nitrogen is converted to nitrogenous salts in nature by many chemical and biochemical process. Proteins, the complex nitrogenous compounds, which are absolutely essential for living beings are also indirectly formed from the nitrogen of air.

Question 3.
State the two possible ways of reaction of nitrogen with hydrogen, also write down the connected equations of reaction.
Answer:
First type Nitrogen combines with hydrogen under the influence of electric spark producing ammonia gas.

Second type : Nitrogen also combines with hydrogen at 550°C under 200 atmospheric pressure in presence of iron catalyst to form nitrogen gas.

Question 4.
State two important ways of fixation of nitrogen.
Answer:
Two ways of fixation of nitrogen :
By electric discharge : During electric discharge in the atmosphere nitrogen and oxygen present in air combine to produce nitric oxide. The produced nitric oxide is then oxidised by atmospheric oxygen to form nitrogen dioxide. Later this oxide upon missing with water vapour or rain water product nitric acid which falls upon our earth.

Nitric acid is then reacted with the bases present in the soil forming nitrate salts.

iii. Fixation of nitrogen due to bacteria Some micro organism and blue green algae convert nitrogen present in air to ammoiate salt by bio-chemical process. When the animal and plant bodies undergo decay most of the nitrogen (proteins) is liberated as ammonia which is oxidised in the soil by the combined action of nitrosifying and nitrifying becteria into nitrate to be again assimilated by plants. A portion of the fixed nitrogen is set free by the action of denitrifying bacteria of the soil.

(d) Hydrogen Chloride (Hydrochloric acid),
Nitric acid and Sulphuric acid

Very Short Answer Type Questions )

Question 1.
Why is concentrated sulphuric acid used to prepare HCl in laboratory ?
Answer:
Concentrated sulphuric acid is used to prepare HCl in laboratory because concentrated sulphuric acid is less volatile.

Question 2.
What is muriatic acid ?
Answer:
Muriatic acid is the commercial name of hydrochloric acid (HCl).

Question 3.
Why is not nitric acid used to prepare HCl ?
Answer:
Nitric acid is not used to prepare HCl as nitric acid is highly volatile and a strong oxidant.

Question 4.
State about solubility of HCl gas in water ?
Answer:
HCl gas is highly soluble in water.

Question 5.
Why is not hydrochloric acid used to prepare nitric acid ?
Answer:
Hydrochloric acid is not used to prepare nitric acid as hydrochloric acid is more volatile than nitric acid.

Question 6.
What is fuming nitric acid ?
Answer:
Fuming nitric acid is a product produced by dissolving excess nitrogen di­oxide in nitric acid.

Question 7.
What is acid rain ?
Answer:
Dissolved NO₂and SO₂ of atmosphere produce acids which come down along with rain. This is called acid rain.

Question 8.
What is oleum ?
Answer:
Oleum is sulphuric acid in which excess sulphur trioxide is dissolved.

Question 9.
What is stone cancer ?
Answer:
Corrosion of marble or stone due to acid rain is called stone cancer.

Question 10.
What is the commercial name of nitric acid ?
Answer:
The commercial name of nitric acid is aqua fortis.

Question 11.
How does copper react with sulphuric acid ?
Answer:
Copper reacts with hot and concentrated sulphuric acid.

Question 12.
Why does sugar of white colour turns to a black mass in contact with concentrated sulphuric acid ?
Answer:
Concentrated sulphuric acid absorbs the water molecules present in sugar molecules leaving behind black carbon.

Question 13.
What is passive iron ?
Answer:
Chemically inactive iron is called passive iron.

Question 14.
What is the commercial name of sulphuric acid ?
Answer:
The commercial name of sulphuric acid is oil of vitriol.

Question 15.
Which acid produces hydrogen reacting with metals Mg and Mn only?
Answer:
Dilute and cold nitric acid (HNO₃) produces hydrogen reacting with Mg and Mn.

Question 16.
Name an acid which has great affinity to water.
Answer:
Concentrated sulphuric acid (H₂SO₄) has great affinity to water.

Question 17.
Which acid is identified by ring test ?
Answer:
Nitric acid is identified by ring test.

Question 18.
Which acid turns blue copper sulphate to white anhydrous salt ?
Answer:
Concentrated sulphuric acid (H₂SO₄) turns blue copper sulphate to white anhydrous salt.

Question 19.
Among HCl, H₂SO₄ and HNO₃ acid which acid has the lowest boiling point ?
Answer:
HCl acid has the lowest boiling point.

Question 20.
What is aqua regia ?
Answer:
Aqua regia is a mixture of 3 volumes concentrated hydrochloric acid and 1 volume concentrated nitric acid.

Question 21.
Which acid is detected by AgNO₃ solution ?
Answer:
Hydrochloric acid is detected by AgNO₃ solution.

Question 22.
What is royal water ?
Answer:
Aqua regia is also known as royal water.

Question 23.
What is fuming sulphuric acid ?
Answer:
Fuming sulphuric acid or oleum is obtained when sulphur trioxide is passed over 98% sulphuric acid.

Question 24.
How is hydrogen chloride gas collected in laboratory ?
Answer:
Hydrogen chloride gas is heavier than air so it is collected by upward dis­placement of air.

Question 25.
Name one air pollutant gas.
Answer:
Air polutant gas is nitrogen dioxide (NO₂)

Question 26.
Which gas pollutes air form Goldsmith’s workshop ?
Answer:
Nitrogen dioxide (NO₂)

Question 27.
Which mineral acid has no reducing property ?
Answer:
Nitric acid (HNO₃)

Question 28.
What is the commercial name of nitric acid ?
Answer:
The commercial name of nitric acid is aquafortis.

Question 29.
State one use of aqua regia.
Answer:
Noble metals like gold, platinum are soluble in aqua regia.

Question 30.
State one use of sulphuric acid.
Answer:
Sulphuric acid is used to prepare fertilizer like ammonium sulphate [NH₂SO₄]

Question 31.
State one use of nitric acid.
Answer:
Nitric acid is used for the manufacture of high explosive like nitroglycerine.

Question 32.
Name a reducing acid.
Answer:
Hydrochloric acid (HCl) is an example of reducing acid.

Question 33.
What is the catalyst used during preparation of nitric acid by the Ostwald process ?
Answer:
Platinum gauze catalyst is used during preparation of nitric acid by the Ostwald process.

Question 34.
Which catalyst is used during preparation of sulphuric acid by contact process ?
Answer:
Platinum asbestos or vanadium pentoxide catalyst is used during preparation of sulphuric acid by contact process.

Question 35.
Which acid is detected by BaCl, solution ?
Answer:
Sulphuric acid (H₂SO₄) is detected by BaCl solution.

Question 36.
What is the basicity of sulphuric acid ?
Answer:
The basicity of sulphuric acid is 2.

Question 37.
Which acid is used as a cleaning agent in bathroom ?
Answer:
Muriatic acid (HCl) is used as a cleaning agent in bathroom.

Question 38.
Among HCl, H₂SO₄ and HNO which acid has the highest point?
Answer:
Sulphuric acid has the highest boiling point [338°C] among HCl, H₂SO₄ and HNO₃

Question 39.
Which acid is called ‘king of chemicals’ ?
Answer:
Sulphuric acid (H₂SO₄) is called ‘king of chemicals’.

Question 40.
Which acid is gas at ordinary temperature ?
Answer:
Hydrochloric acid.

Question 41.
Dense white fumes are formed when a glass-rod, moistened with strong ammonia solution, is held in a gas. Identify the gas.
Answer:
The gas is ammonia.

Question 42.
What is laughing gas ?
Answer:
Nitrous oxide (N₂O) is called laughing gas.

Question 43.
Can dry hydrogen chloride gas turn blue litmus paperred ?
Answer:
No. Dry hydrogen chloride gas turns a moist blue litmus paper red.

Question 44.
What is the molecular weight of nitric acid ?
Answer:
The molecular weight of nitric acid is 63.

Question 45.
What is the specific gravity of sulphuric acid ?
Answer:
The specific gravity of sulphuric acid is 1.84.

Question 46.
Name one metal ion that can be identified by using H₂S.
Answer:
Cu²⁺

Question 47.
What is commercial name of pyrosulphuric acid?
Answer:
Oleum (H₂S₂O₇)

Question 48.
What is the catalyst used for preparation of HNO₃ by ‘ostwald process’
Answer:
Platinum wie gauze is used as the catalyst for the purpose.

Question 49.
What is liquor ammonia?
Answer:
Liquor ammonia is a saturated solution of ammonia in water.

Question 50.
What is Nessler’s reagent?
Answer:
Alkaline solution of potassium tetra iodo mercurate, K₂[Hgl₄] is known as Nessler’s neagent.

Question 51.
What is aqua fortis?
Answer:
Nitric acid (HNO₃) was known to the alchemists as aqua fortis.

Question 52.
Why do old oil paintings turn black on exposure to H₂S?
Answer:
The paints used in oil paintings contain lead that react with weak dibasic H₂S to form black lead sulphide (PbS).

Question 53.
Name a gas which can be prepared in kipp’s apparatus.
Answer:
H₂S can be readily and intermittently prepared in kipp’s apparatus.

Question 54.
What happens when calcium cyanamide is heated with super heated steam?
Answer:
When calcium cyanamide is heated with super heated steam (especially in an autoclave), it is hydrolysed to form ammonia.

Question 55.
What happens when ammonia is burnt in air?
Answer:
When ammonia is burnt in air, it burns with a greenish-yellow flame forming nitrogen and steam.

Question 56.
H₂SO₄ is industrially produced by which process?
Answer:
H₂SO₄ is industrially produced by contact process.

Question 57.
Why H₂S gas is collected by upward displacement of air?
Answer:
H₂S is soluble in cold water and is heavier than air. So it is not collected over water and is collected by upward displacement of air.

Short Answer Type Questions

Question 1.
Describe the preparation of hydrogen chloride in laboratory with mention of
(i) chemical equation
(ii) collection
Answer:
Preparation of hydrogen chloride in laboratory : Chemical equation:
(i) If the mixture of sodium chloride and concentrated sulphuric acid is heated at 150°C – 200°C then sodium bisulphate and hydrogen chloride gas are produced.

(ii) If it is heated at 500°C then sodium sulphate and hydrogen chloride gas are evolved.

Collection : Since dry hydrogen chloride gas is heavier than air it is col­lected by upward displacement of air.

Question 2.
Why the reaction is kept at lower temperature during the preparation of hydrogen chloride in laboratory from sodium chloride and cone, sulphuric acid ?
Answer:
Reason In the laboratory the reaction is kept at lower temperature because:

• at high temperature the flask used in the preparation may be cracked.
• Sodium sulphate at higher temperature forms a hard crust and sticks to the glass. Its removal is then difficult.

Question 3.
Why hydrogen chloride is not collected over displacement of water?
Answer:
Reason : Hydrogen chloride is highly soluble in water. It has been found that at 0°C, 450 ml of hydrogen chloride is dissolved in 1 ml of water. So, it is not collected over displacement of water.

Question 4.
What is the compound necessary for drying of hydrogen chloride gas?
Answer:
Drying of hydrogen chloride : To remove water vapour, hydrogen chloride gas is passed over cone. H₂SO₄.

Hydrogen chloride is acidic nature. Hence, it cannot be dried over quick lime (CaO), caustic soda (NaOH) or caustic potash (KOH).

Question 5.
How is hydrochloric acid prepared ?
Answer:
Preparation of hydrochloric acid : Hydrochloric acid is a solution of hydrogen chloride gas in water. Cone, hydrochloric acid, as used in the laboratory is not 100% pure hydrochloric acid. It is about 38% solution of hydrogen chloride gas in water.

Hydrogen chloride gas is passed into a beaker containing cold water till the water is saturated with the gas. The contents of the beaker is a concentrated solution of hydrochloric acid.

Question 6.
Hydrochloric acid is not prepared by dissolving hydrogen chloride gas in water directly—why ?
Answer:
Reason As hydrogen chloride gas is highly soluble in water and the rate of dissolving of HCl gas in water is much higher than the rate of formation of HCl gas as a result there is a vacuum in the flask. To fill up the vacu­um water in the beaker enters into the flask and creates explosion when it contacts with sulphuric acid present in the flask.

Question 7.
Nitric acid is not used in the preparation of hydrochloric acid—why?
Answer:
Explanation :
(a) Nitric acid is not used because during the preparation of hydrogen chloride gas, nitric acid oxidises the evolved hydrogen chloride gas into chlorine gas.
Reaction HNO₃ + _;3HCl = NOCl + 2[Cl] + 2H₂O

(b) Hydrochloric acid (b. p. 86°C) and hydrogen chloride are volatile in nature. So they will be collected jointly in a receiver where nitric acid may oxidise hydrogen chloride into chlorine. On the other hand H₂SO₄(b.p. 338°C) is non-volatile; so, this is not happened.

Question 8.
State two physical properties of HC:
Answer:
Physical properties of HCl:

• It is a colourless gas with a choking smell and strongly fuming in moist air, hydrogen chloride is 127 times as heavy as air ; it neither burns nor supports burning.
• It is highly soluble in water. At 0°C, 450 ml of hydrogen chloride gas is dissolved in 1 ml of water.

Question 9.
How is pure hydrogen chloride prepared ?
Answer:
Preparation of pure hydrogen chloride Pure hydrogen chloride is obtained by the action of water upon silicon tetrachloride. Equation : SiCl₄ + 4H₂O = Si(OH)₄ + 4HCl

Question 10.
State the reaction of HCl with Na.
Answer:
Hydrogen chloride neither burns in air nor supports combustion. However burning sodium continues to burn in the gas with a bright yellow flame producing hydrogen and anhydrous sodium chloride.
Equation : 2Na + 2HCl = 2NaCl + H₂↑

Question 11.
Show the acidic property of hydrochloric acid.
Answer:
The aqueous solution of hydrochloric acid is a strong acid :

dissolves base metals, liberating hydrogen and forming metallic chlorides,
e.g. Zn + 2HCl = ZnCl₂ + H₂↑
The order of activity of the metals for liberating hydrogen may be stated as:
Ca > Mg > Al > Zn > Fe > Sn.

Question 12.
How copper and silver react with hydrochloric acid ?
Answer:
Generally, copper, silver are not attacked by hydrochloric acid. In presence of air, copper and silver react with very slowly producing corresponding chlorides and water.
Equations :

• 2Cu + 4HCl + O₂ = 2CuCl2₂ + 2H₂O
• 4Ag + 4HCl + O₂ = 4AgCl + 2H₂O

Question 13.
How does ammonia react with hydrogen chloride
Answer:
Reaction of ammonia with hydrogen chloride : Ammonia in contact with hydrogen chloride gives dense white fumes of solid ammonium chlo­ride. This reaction is an example of the formation of a solid product by the interaction of two gases.
Equation : NH₃(g) + HCl(g) = NH₄Cl(s)

Question 14.
What is reaction between Na₂CO₃ and HCl ?
Answer:
Reaction of Na₂CO₃ with HCl :
HCl reacts with Na₂CO_s to literate carbon dioxide.
Na₂CO₃ + 2HCl = 2NaCl + CO₂↑ + H₂O

Question 15.
State the action of hydrochloric acid with oxidising agent like MnO₂ and KMnO₄.
Answer:
Reaction of hydrochloric acid with MnO₂and KMnO₄
Manganese dioxide (MnO₂ oxidises hot and concentrated hydrochloric acid to greenwish yellow chloride.Potassium permanganate oxidises the hydrochloric acid at the ordinary tem­perature.

Question 16.
Show the presence of chloride ion in hydrochloric acid.
Answer:
Presence of chloride ion in hydrochloric acid : When hydrochloric acid is added to a solution of silver nitrate, a white precipitate of the chloride of silver is obtained. Silver chloride is insoluble in nitric acid but soluble in ammonium hydroxide.
Equation : AgNO₃ + HCl = AgCl↓ + HNO₃ 

Question 17.
How is hydrochloric acid identified?
Answer:
Identification of hydrochloric acid : When silver nitrate solution is added to hydrochloric acid taken in a test tube, curdy white precipitate of silver chloride is formed. The precipitate is insoluble in nitric acid but dissolves in ammonium hydroxide forming a clear solution of complex salt argento ammonium chloride. Equations :

• AgNO₃ + HCl = AgCl↓ + HNO₃
• AgCl + 2NH₄OH = [Ag(NH₃)₂]Cl + 2H₂O

Question 18.
State the identification of hydrogen chloride gas.
Answer:
Identification of hydrogen chloride gas : Dense white fumes are formed when a glass-rod, moistened with strong ammonia solution, is held in the hydrogen chloride gas.
Equation : NH₃(g) + HCl (g) = NH₄Cl (s)

Question 19.
What are the uses of hydrochloric acid ?
Answer:
Uses of hydrochloric acid :

• It is used in dyeing and calico-printing,
• It is used as a cleaning agent in galvaning and tinplating,
• It is used to prepare aqua-regia,
• It is used in the manufacture of glucose, glue and many useful metal-chlorides.

Question 20.
Describe the preparation of nitric acid in laboratory with mention of
(i) chemical required
(ii) chemical reaction.
Answer:
Preparation of nitric acid in laboratory :
Chemical required :

• Chille salt petre (NaNO₃) or nitre (KNO₃)
• Cone. Sulphuric acid.

Reaction occurs in two steps :

(a) If the reaction is kept at 200°C-300°C then sodium bisulphate and nitric acid are produced.

(b) At 800°C, sodium sulphate and nitric acid are formed in the reaction between sodium nitrate and concentrated sulphuric acid.
2NaNO₂+ H₂SO₄ = Na₂SO₄ + 2HNO₄

Question 21.
Why nitric acid is prepared at lower temperature (200°C) in laboratory?
Answer:
Nitric acid is prepared at lower temperature (200°C) in laboratory because :

• At high temperature nitric acid decomposes.
  4HNO₃ = 4NO₂ + O₂ + 2H₂O
• Nitric acid vapour attacks glass surface of the retort.
• Sodium sulphate (Na₂SO₄) formed at the higher temperature sticks to glass and is difficult to remove from the glass retort.

Question 22.
Why is cone, sulphuric acid used instead of cone, hydrochloric acid in the preparation of nitric acid in laboratory ?
Answer:
Choice of acid : In the preparation of an acid, the reacting acid must be less volatile than the acid to be prepared.Hence, cone. H₂SO₄(b.p. 338°C) is chosen because it is less volatile than nitric acid (b.p. 86°C). Hydrochloric acid is more volatile than nitric acid, so hydrochloric acid is not used. Beside this hydrochloric acid reacts with produced nitric acid to form nitrosyl chloride, chlorine and water.
3HCl + HNO₃ = NOCl + Cl₂ + 2H₂O

Question 23.
What is fuming nitric acid ?
Answer:
Fuming nitric acid : It is brown coloured liquid. It is actually cone. HNO₃ containing dissolved nitrogen dioxide (NO₂) gas. The dissolved nitrogen di­oxide spontaneously comes out of the liquid as brown fumes. That is why, it is called fuming nitric acid.

Preparation of fuming nitric acid : It is prepared by distilling cone, nitric acid with starch or arsenious oxide (As₂O₃).

Property and use of fuming nitric acid : Fuming nitric acid is a stronger oxidising agent than ordinary cone, nitric acid. It is used for many oxidation purposes where ordinary nitric acid does not give satisfactory results.

Question 24.
State the preparation of nitric acid by Ostwald process.
Answer:
Preparation of nitric acid by Ostwald process (1914) :

• In this process ammonia is oxidised in presence of heated (750°C-900°C) platinum gauze catalyst by oxygen in air to produce nitric oxide.
  4NH₃ + 5O₂ = 4NO↑ + 6H₂O + 218,660 cal
• The gases containing nitric oxide (NO) and steam (H₂ are cooled and then mixed with air to oxidise nitric oxide to nitrogen dioxide.
  2NO + O₂ = 2NO₂
• Nitrogen dioxide, is then absorbed in water to yield a 50% solution of nitric acid and nitric oxide.
  3NO₂ + H₂O = 2HNO₃ + NO↑

Question 25.
What are the physical properties of nitric acid ?
Answer:
Physical properties of nitric acid :

• Pure nitric acid is a colourless, fuming liquid of specific gravity 152 at 15°C,
• It boils at 86°C and freezes at -42°C into a transparent crystalline substance.
• It is highly soluble in water.

Question 26.
State the reaction of nitric acid with alkalis.
Answer:
Reaction of nitric acid with alkalis :
As nitric acid is a strong acid, it rapidly reacts with and neutralises alkali to form salt and water.
Equations :
(a) NaOH + HNO₃ = NaNO₃ + H₂O
(b) NH₄OH + HNO₃ = NH₄NO₃ + H₂O

Question 27.
State the reaction of nitric acid with metals.
Answer:
Reaction of nitric acid with metals :
(i) Reaction with iron : Iron is oxidised to ferric nitrate on reacting with hot concentrated nitric acid.
Equation : Fe + 6HNO₃ = Fe(NO₃)₃ + 3NO₂ + 3H₂O

(ii) Reaction with magnesium :

• Cold and moderately concentrated nitric acid on reaction with magnesium produces magnesium nitrate, nitric oxide and water.
  Equation : 3Mg + 8HNO₃ = 3Mg(NO₃)₂ + 2NO + 4H₂O
• Magnesium liberates hydrogen from cold and very dilute nitric acid.
  Equation : Mg + 2HNO₃ Mg(NO₃)₂ + H₂
• Reaction with copper: Hot concentrated nitric acid reacts with copper metal producing copper nitrate and nitrogen dioxide.
  Equation : Cu + 4HNO₃ = Cu(NO₃)₂ + 2NO₂ + 2H₂O

Question 28.
State the oxidising action of concentrated nitric acid.
Answer:
Oxidising action of concentrated nitric acid :
Cone. HNO₃ is a very good oxidising agent.
It oxidises many metals and non-metals.

(i) Cone. HNO₃ oxidises copper turnings to copper nitrate and itself is reduced to brown coloured nitrogen dioxide gas.

(ii) Concentrated HNO₃ oxidises charcoal i.e. carbon to carbon dioxide and is itself reduced to nitrogen dioxide.

Question 29.
What is passive iron?
Answer:
Passive iron: Cold and concentrated nitric acid or fuming nitric acid when comes in contact with iron produces passive iron. Passive iron is chemically inactive.

Cause if passivity : The nibic acid when comes in contact with iron, an insoluble coating of iron oxide (Fe₃O₄) forms on iron at initial stage. The coating makes iron chemically inactive.

Question 30.
What is aqua regia ? What is its use ?
Answer:
Aqua regia : A mixture of cone. HNO₃ (1 vol.) and cone, hydrochloric acid (3 vols.) is known as aqua regia.

Use of aqua regia : It dissolves gold and platinum.

Question 31.
What is ring test experiment of nitric acid ?
Answer:
Ring test experiment of nitric acid : A little amount of dilute nitric acid is taken in a test tube. Freshly prepared ferrous sulphate is added to it. Now cone. H₂SO₄ is taken in another test tube. cone. H₂SO₄ taken in a tube is carefully poured into the above liquid mixture so as to form a heavy layer at the bottom. A brown ring is formed at the junction of two liquids.

Thus, the reaction involved in ring tests as :

Question 32.
State uses of nitric acid.
Answer:
Uses of nitric acid :

• It is used in the production of explosives such as dynamite, gun cotton, nitro-glycerine, picric acid, and trinitro toluene (TNT).
• It is used to prepare aqua regia in electroplating and in battery.
• It is also used to prepare rayon, artificial silk and dyes.

Question 33.
What is acid rain ?
Answer:
Acid rain The oxides NO₂ and SO₂ reacting with moisture and oxygen of air correspondingly produce HNO₃ and H₂SO₄. The acids dissolve in rain water. The rain coming down on earth carrying these acids is known as acid rain. Function of acid rain : The acids present in the rain water damage buildings monuments, statues by corrosion. Soil also becomes acidic which causes degradation of soil that in turn causes decline in forest area and agricultural productivity.

Question 34.
Sulphuric acid is not prepared directly by adding water to SO₃ why ?
Answer:
Explanation : It is because of the fact that water is not used for absorbing SO₃ as the reaction is exothermic. Result is this that large amount of heat evolved will be a cause of most of SO₃ to be volatilised, the rest amount of it does not form any homogeneous mixture but a dense fog of H₂SO₄ particles is formed. H₂SO₄ is not easily available from the fog. Beside this at high temperature some parts of H₂SO₄ decompose to SO₂ and O₂. Hence water is not directly added to SO₃.

Question 35.
What is fumming sulphuric acid or oleum ?
Answer:
Fumming sulphuric acid or oleum : Fumming sulphuric acid or oleum is obtained when SO₃ is passed over 98% (approximately) sulphuric acid.
Equation:

Question 36.
State the effect of SO₂ pollution
Answer:
of SO₂ pollution ;

• SO₂ creates problems in eyes and also in lungs,
• Many diseases like asthama, bronchitis etc. effect if SO₂ is inhaled.

Question 37.
Historical monuments like Tajmahal is also affected by sulphuric acid – why ?
Answer:
Reason : Historical monuments like Tajmahal are damaged due to corrosion when rain carrying H₂SO₄ acid pour on these. Environmentalists say the corrosion of Tajmahal is due to presence of SO₂ in high concentration in the air of Agra. The SO₂ gas emitted from petroleum refinery situated on the other side of the Jamuna river reacts with oxygen and moisture of air to produce H₂SO₄.

Question 38.
What are possible remedies to save our historical monument—Tajmahal?
Answer:
Possible remedy :

• Banning of this factories in the neighbourhood region of Taj and also in Mothura is promulgated by an ordinance.
• Excessive use of motor vehicles should be restricted. Petroleum refining plant should be kept 90 km apart.
• Electrostatic precipitators which are used for treatment of the harmful emitted gas S0₂ before emission.

Question 39.
What is stone cancer ?
Answer:
Stone cancer : In atmosphere, Sulphur dioxide (SO₂) gas reacts with oxygen and water vapour producing sulphuric acid. The acid being dissolved in rain water comes down on marble walls. The marble walls thus corrode, the corrosion of the marble is called stone cancer.

Question 40.
State physical properties of H₂SO₄.
Answer:
Physical properties of H₂SO₄ :

• It is colourless, odourless heavy oily liquid.
• Its specific gravity is 1.84 and its b.p. (boiling point) is 338°C.
• It is soluble in water and it is a corrosive acid.

Question 41.
Water is not added on concentrated sulphuric acid to make it dilute — why ?
Answer:
Explanation : Huge amount of heat is produced if water is added to con­centrated sulphuric acid. As a result water all on a sudden being volatilised spreads all around and creates problem. So, cone. H₂SO₄ acid is slowly added to with constant stirring.

Question 42.
State the reaction of H₂SO₄ with alkalis.
Answer:
Reaction of H₂SO₄ with alkalis : As H₂SO₄ is a dibasic acid containing two replaceable hydrogen atoms, it reacts with bases and alkalis to produce two types of salts acid salts and normal salts and water.
Equation :

Question 43.
State the reaction of H₂SO₄ with carbonates and bicarbonates.
Answer:
Reaction of H₂SO₄ with carbonates and bicarbonates : At ordinary temperature it liberates carbon dioxide from carbonates and bicarbonates.
Equation :

Question 44.
State the reaction of H₂SO₄ with metals.
Answer:
Reaction of H₂SO₄ with metals :
Metals lying above hydrogen in the electrochemical series react with dilute sulphuric acid to form hydrogen gas.
Equation :
(a) Mg + H₂SO₄ = MgSO₄ + H₂↑
(b) Zn + H₂SO₄ = ZnSO₄ + H₂↑

Question 45.
State the oxidising property of concentrated sulphuric acid.
Answer:
Oxidising property of concentrated sulphuric acid :
(a) Reaction with metals : Hot and concentrated sulphuric acid oxidises metallic copper, silver, zinc etc. into their sulphates, itself being reduced to sulphur dioxide.
Equation :

(b) Reaction with non-metals Non-metals carbon and sulphur on being treated with hot concentrated sulphuric acid are oxidised to carbon dioxide, sulphur dioxide respectively.
Equation :

Question 46.
State the dehydration action of concentrated sulphuric acid.
Answer:
Dehydration action of concentrated sulphuric acid :
(a) Concentrated sulphuric acid chars sugar. The acid takes up all its hydrogen and oxygen in the form of water molecules from the compound separating black carbon as residue.
Equation :

(b) When a mixture of formic acid and concentrated sulphuric acid is heated carbon monoxide is produced by loss of water molecule from the formic acid.

Equation

Question 47.
What is the identification reaction of sulphuric acid ?
Answer:
Identification reaction of sulphuric acid : When barium chloride solution is added to dilute sulphuric acid, a white precipitate of barium sulphate insoluble in dilute or concentrated hydrochloric acid or nitric acid is obtained.
Equation :

Question 48.
State the uses of sulphuric acid.
Answer:
Uses of sulphuric acid :

• It is used for the preparation of different chemical compounds like HCl, HNO₃, ether, alcohol etc.
• It is used as an important raw material for dyes, medicine, plastic industries.
• It is used to prepare different explosives like trinitrotoluene (TNT) nitroglecer- ine etc.

Question 49.
Explain the following :
Concentrated nitric acid turns yellow in sun light.
Answer:
Explanation Nitric acid turns yellow because of its decomposition forming nitrogen dioxide (NO₂gas.
Equation : 4HNO₃= 4NO₂+ 2H₂O + O₂

Broad Answer Type Questions

Question 1.
State the contact process for the manufacture of sulphuric acid.
Answer:
Contact process for the manufacture of sulphuric acid :
Principle : (a) Formation of SO₂: SO₂ is prepared by burning sulphur or iron pyrites in excess of air.

(b) Formation of Sulphur trioxide (SO₃) SO₃ is prepared by the oxidation of sulphur dioxide with oxygen (from air) in presence of platinised asbestos or, V₂O₅ as catalyst at 450°C.
Equation:

(c) Formation of oleum : Now sulphur trioxide thus produced are not allowed to react with water directly. Sulphur trioxide absorbs concentrated sulphuric acid (98%) turning it as fumming sulphuric acid or oleum.
Equation :

(d) Dilution of oleum to sulphuric acid : Pure and concentrated sulphuric acid is produced by adding slowly requisite amount of water in fumming sulphuric acid.
Equation : H₂S₂O₇ + H₂O = 2H₂SO₄

Question 2.
State an experiment to illustrate the solubility of HCl in water and the acidic character of the aqueous solution.
Answer:
Fountain experiment : A round bottomed flask is fitted with a cork through which passes a long tube ending in a jet in­side the flask. The flask is filled with hydrogen chloride and clamped in an inverted position so that the other end of the tube dips in water coloured blue by litmus.

The flask is then cooled when the gas contracts inside. As a result, the blue solution rises up through the tube and enters the flask in the form of fountain. The blue litmus solution in the flask turns red. This experiment proves simultaneously the solubility of hydrogen chloride in water and the acidic character of its aqueous solution.

Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 3 Chemical Calculations offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 3 Question Answer – Chemical Calculations

Very Short Answer Type Questions

Question 1.
What is the molecular weight of ammonium phosphate ?
Answer:
149

Question 2.
How much CaO is obtained from 10 kg CaCO₃ ?
Answer:
5.6 kg

Question 3.
How much CaCO₃ will react with dil HCl to produce 22 g CO₂ ?
Answer:
50 g

Question 4.
How much hydrogen is required to produce 72 g water?
Answer:
8g

Question 5.
How much potassium chlorate is to be heated to produce as much oxygen as required to burn 6 g carbon completely?
Answer:
40.83 g

Question 6.
How much quantity of silver chloride (AgCl) can be obtained from 1.0 g silver nitrate?
Answer:
0.844 g

Question 7.
How many grams limestone are needed to get 48g CO₂ ?
Answer:
109.09 g

Question 8.
How much hydrogen is produced when steam is passed over 28 kg red hot iron?
Answer:
1.33 kg

Question 9.
What is mole number of a substance ?
Answer:
Mole number of a substance

Question 10.
What is the percentage of water in blue vitriol ?
Answer:
36.07%.

Question 11.
2 Mg + O₂ = 2 MgO; what type of chemical reaction is it?
Answer:
2 Mg + O₂ = 2 MgO is direct combination type of chemical reaction.

Question 12.
HCl + NaOH = NaCl + H₂ O; what type of chemical reaction is it?
Answer:
HCl + NaOH = NaCl + H₂ O is the type of neutralisation reaction.

Question 13.
Zn + CuSO₄ = ZnSO₄ + Cu; what type of chemical reaction is it?
Answer:
Zn + CuSO₄ = ZnSO₄ + Cu is the type of substitution reaction.

Question 14.
NH₄ CNO (8) CO(NH₂)₂; what type of chemical reaction is it?
Answer:
NH₄ CNO arrow CO(NH₂)₂ is the type of rearrangement reaction.

Question 15.
Give an example of double decomposition type of reaction.
Answer:
AgNO₃ + NaCl = AgCl + NaNO₃ is an example of double decomposition type of reaction.

Question 16.
State a limitation of a chemical equation.
Answer:
A reaction whether exothermic or endothermic is not known from a chemical equation.

Question 17.
Give an example of addition reaction.
Answer:
Carbon monoxide reacts with chlorine to form carbonyl chloride (COCl₂) is an example of addition reaction.

Question 18.
Give an example of a substitution reaction.
Answer:
Chlorine reacts with methane (CH₄) to form successively CH₃ Cl, CH₂ Cl₂, CHCl₃ and ultimately CCl₄ in presence of sunlight is an example of a substitution reaction.

Question 19.
Give an example of a thermal decomposition type of reaction.
Answer:
Calcium carbonate on heating decomposes into calcium oxide and carbon dioxide is an example of a thermal decomposition type of reaction.

Question 20.
Give an example of redox type of reaction.
Answer:

is an example of redox type of reaction.

Question 21.
Balance the following reaction: Fe + H₂ O(Fe₃ O₄ + H₂.
Answer:
Balanced equation of Fe + H₂ O arrow Fe₃ O₄ + H₂ is
3 Fe + 4 H₂ O = Fe₃ O₄ + 4 H₂

Question 22.
2 SO₂ + O₂ ⇌ 2 SO₃; what type of reaction is it ?
Answer:
2 SO₂ + O₂ ⇌ 2 SO₃ is an example of reversible type of reaction.

Question 23.
A + B²⁺ = A²⁺ + B; what type of reaction is it ?
Answer:
A + B²⁺ = A²⁺ + B is an example of oxidation-reduction type of reaction.

Question 24.
Balance the following reaction :
MnO₂ + HCI → MnCI₂ + CI₂ + H₂O
Answer:
Balanced equation of MnO₂ + HCl → MnCl₂ + Cl₂ + H₂O is
MnO₂ + 4 HCl = MnCl₂ + Cl₂ + 2 H₂O

Question 25.
Balance the following reaction :
Ag₂ SO₄ + BaCI₂ → BaSO₄ + AgCl.
Answer:
Balanced equation of Ag₂ SO₄ + BaCl₂ → BaSO₄ + AgCl is
Ag₂ SO₄ + BaCl₂ = BaSO₄ + 2 AgCl

Question 26.
Write the equation relating energy with mass.
Answer:
E = m c²

Question 27.
Write the relation between molecular mass and vapour density.
Answer:
Molecular mass = 2 × Vapour density.

Question 28.
Calculate the vapour density of oxygen relative to hydrogen.
Answer:
Vapour density of oxygen
= \(\frac{Molecular mass of oxygen}{2} = [latex]\frac{32}{2}\) = 16

Question 29.
6 g carbon on complete combustion produce how much volume of CO₂ at STP ?
Answer:

12g carbon on complete combustion produce 22.4 L CO₂ at STP
6g carbon on camplete combustion produce 11.2 L CO₂ at STP

Question 30.
One mole of zinc reacts with excess H₂ SO, to produce how many moles of hydrogen ?
Answer:
1 mole of hydrogen.

Short Answer type Questions :

Question 1.
What is empirical formula?
Answer:
Empirical formula : It is the formula of a compound which gives the simple whole number ratio of the atoms of various elements present in one molecule of compound.

Question 2.
What is molecular formula ?
Answer:
Molecular formula : It is the formula of a compound which gives the actual number of atoms of various elements present in one molecule of the compound.

Question 3.
What are the limitations of chemical formula ?
Answer:
Limitations of chemical formula :

1. It fails to convey whether the elements in a molecule are present in the form of atoms or ions.
2. It does not tell anything about the binding force that holds atoms in a molecule together.
3. It does not tell us about the arrangement of various atoms with respect to one another within the molecule.

Question 4.
What is structural formula ?
Answer:
Structural formula : A formula which gives the actual arrangement of the different atoms in the molecule or show how the different atoms in the molecule are linked together is called a structural or a graphic formula of the compound.

Question 5.
What is percentage of an element?
Answer:
Percentage of an element : Percentage of an element in a chemical compound is the number of parts by weight of it present in 100 parts by weight of the compound.

Question 6.
What are mass-mass relationship problems ?
Answer:
Mass-mass relation hip problems : In this type of problems, mass of one of the reactants/products is to be calculated if that of the other reactants/ products is to be calculated if that of the other reactants/ products are given.

Question 7.
What are mass-volume relationship problems ?
Answer:
Mass-volume relationship problems : In this type of problems, mass or volume of one of the reactants or products is calculated from the volume or mass of other substances.

Question 8.
What are volume-volume relationship problems ?
Answer:
Volume-volume relationship problems : In this type of problems, the volume of one of the reactants or products is to be calculated from the volume of some other reactant and product.

Question 9.
What is limiting reactant ?
Answer:
Limiting reactant : The reactant which is completely used and determines the amount of product formed is known as limiting reactant.

Question 10.
What is theoretical yield ?
Answer:
Theoretical yield : The theoretical yield of a product is the maximum yield obtainable as calculated on the basis of the amount of limiting reactant used.

Question 11.
What is percent yield?
Answer:
Percent yield : Percent yield which is the ratio of the actual yield to the theoretical yield multiplied by 100 .

Question 12.
What do you mean by chemical reaction ?
Answer:
Chemical reaction: Any chemical change in matter which involves the transformation of matter into a new substance or new substances is termed as chemical reaction.

Question 13.
Define reactants in a chemical reaction.
Answer:
Reactants: The substances with which a chemical reaction is started are called the reactants.

Question 14.
Define products in a chemical reaction.
Answer:
Products: The substances formed as the result of the chemical reaction are called the products.

Question 15.
Define direct combination reaction.
Answer:
Direct combination : The reaction in which two or more reactions combine directly forming molecules of new substance is called direct combination.
Example : Burning magnesium wire reacts directly with oxygen forming new molecules of magnesium oxide.
2 Mg + O₂ = 2 MgO

Question 16.
What is meant by decomposition reaction?
Answer:
Decomposition : When molecule of a substance is broken down or decomposed in a chemical reaction to form two (or more) new substances in presence of heat or electricity. It is called decomposition.
Example : (a) Calcium carbonate on heating decomposes into calcium oxide and carbon dioxide.

(b) Electricity is passed through acidulated water hydrogen and oxygen are produced due to decomposition of water.
2H₂O = 2H₂ + O₂

Question 17.
Define double decomposition reaction.
Answer:
Double decomposition : The reaction in which the constituents of the molecules of reactants Change their position and forming molecules of new substances is called double decomposition.
Example : AgNO₃ + NaCl = AgCl↓+ NaNO₃

Question 18.
What is meant by acid-base reaction or neutralisation reaction ?
Answer:
Acid-base reaction or neutralisation reaction : In this reaction an acid reacts with a base forming salt and water. Equivalent amount of an acid neutralises an equivalent amount of a base. This is known as neutralisation reaction.

Question 19.
Define oxidation-reduction type reaction.
Answer:
Oxidation-reduction reaction : The chemical reaction in which a chemical species loses electron(s) is an oxidation reaction and the reaction in which a chemical species gains electron(s) is called oxidation-reduction reaction.

Question 20.
What is meant by addition reaction?
Answer:
Addition reaction: The reaction in which one reactant molecule directly combines with other molecule of reactant forming new molecules of product without leaving any part of molecules of reactants is known as addition reaction.

Question 21.
Define substitution reaction.
Answer:
Substitution reaction: It is a chemical reaction in which one atom or molecule of a compound is replaced by another atom or molecule of another substance.
Example : Zn + CuSO₄ = ZnSO₄ + Cu

Question 22.
What is meant by rearrangement reaction?
Answer:
Rearrangement reaction: A reaction where a compound changes by internal arrangement of its atoms into another substance with different properties but having the same composition is known as rearrangement reaction.
Example : Ammonium cyanate changes to urea on heating.

Question 23.
Define chemical equation.
Answer:
Chemical equation : A brief representation of a chemical reaction by using symbols of atoms of the elements and formulae of molecules of reactants and products maintaining the balance in between is known as chemical equation. It reveals both the qualitative ancL quantitative aspects of a chemical change.

Broad Answer Type Questions :

Question 1.
What steps should be followed to solve a problem based on chemical equation by weight-weight method ?
Answer:
Following steps are followed :

1. First write down the complete balanced chemical equation.
2. The molecular weight of the reactants and products are to be calculated from their respective formulae by adding atomic weights of the concerned elements.
3. The unknown weight of the substance asked for in the question is to be calculated from the calculated weight in the equation.
4. Same units are to be used for all quantities.

Question 2.
What are the informations avallable from the formula CaCO₃ ?
Answer:
The formula CaCO₃ conveys the following informations :

1. It stands for calcium carbonate.
2. It tells that calcium carbonate is composed of calcium, carbon and oxygen elements.
3. It represents that a molecule of calcium carbonate.
4. It represents that a molecule of calcium carbonate is made up of One atom each of calcium and carbon and three atoms of oxygen.
5. It stands for 100 parts by weight of calcium carbonate i.e. its molecular weight and signifies that the ratio of calcium, carbon and oxygen by weight in it is 40: 12: 48.

Question 3.
What is the method of writing chemical equation ?
Answer:
Method of writing chemical equation :
i. Initially the symbols of atoms of elements and formulae of molecules of reactants and products are written.

ii. Symbols and formulae of the reactants are written in the left side and these for products are in the right side. An arrow mark (→) is placed between reactants and products. For more than one reactants and products a plus sign (+) is to be given between the reactants and also between the products.

iii. Number of atoms of the reactants in the left hand side must be equal to the number of atoms of the products in the right hand side so as to maintain the law of conservation of mass. To equalise both sides, proper multiplication is required so that the number of atoms in both sides are same.

iv. Now the equation is expressed by replacing the arrow sign by a sign of equal ( = ).

Question 4.
What informations are obtained from the chemical equations ?
Answer:
A chemical equation gives the following informations :
(a) Qualitative informations :

• From chemical equation, the naming of elements and compounds taking part in the reaction and also the products are known.
• From chemical equation, the symbols and the formulae of the reactants and products are also known.

(b) Quantitative informations :

• Number of atoms or molecules of the reactants and products involved in the reaction are known.
• How many parts of elements and compounds taking part in the reaction and producing are also known.
• If the reactants and products are all gaseous then at the same temperature and pressure the ratio in volumes is known.

Question 5.
What informations are obtained from the equation :
C + O₂ = CO₂
Answer:
The following informations are obtained from the equation :
C + O₂ = CO₂

(a) Qualitative informations :
i. From the above equation it is known that carbon combines with oxygen producing carbon dioxide.
ii. Their respective symbols and formulae are also known.

(b) Quantitative informations :
i. One carbon atom combines with one oxygen molecule producing one carbon dioxide molecule.
Hence total number of atoms in the left hand side is (1 + 2) = 3 and the number of atoms in the right hand side is also 3.
ii. One gram-atom carbon reacts with one gram-molecule of oxygen giving rise one gram-molecule of carbon dioxide.
12 g carbon combines with 32 g oxygen yield 44 g carbon dioxide.
Hence, total mass in the left hand side (12 + 32) g = 44 g is equal to the total mass in the right hand side 44 g. It proves law of conservation of mass.
iii. Again 12 g carbon combines with 32 g oxygen producing 22.4 litre of carbon dioxide at STP.

Question 6.
What informations are obtained from the equation :
2 H₂ + O₂ = 2 H₂O
Answer:
The following informations are obtained from the equation :
2 H₂O + O₂ = 2 H₂O

(a) Qualitative informations : The reactants are hydrogen and oxygen, water is the product.
(b) Quantitative informations :

1. Two molecules of hydrogen combine with one molecule oxygen to produce two molecules water.
2. Two volumes hydrogen and one volume oxygen combine to produce two volumes water at the same temperature and pressure and their ratio is 2 : 1 : 2
3. Two moles of hydrogen and one mole oxygen combine chemically to produce two moles water.

Question 7.
What informations are obtained from the equation :
3 H₂ + N₂ = 2 NH₃
Answer:
The following informations are obtained from the equation :
3 H₂ + N₂ = 2 N H₃
(a) Qualitative informations : The reactants are hydrogen and nitrogen, ammonia is the product.
(b) Quantitative informations :

1. Three molecules of hydrogen combine with one molecule nitrogen to produce two molecules ammonia.
2. Three volumes hydrogen and one volume nitrogen combine to produce two volumes ammonia at the same temperature and pressure and their ratio is 3 : 1 : 2.
3. Three moles of hydrogen and one mole nitrogen combine chemically to produce two moles ammonia.

Question 8.
What are the limitations of a chemical equation ?
Answer:
Limitations of a chemical equation :

1. Under what conditions a chemical reaction is occurred i.e. pressure, temperature, catalyst are not known.
2. A reaction whether exothermic or endothermic is not known from chemical equation.
3. Chemical equation cannot provide information about completion of the reaction or attainment of equilibrium.
4. A chemical equation does not give any idea about the reversibility of the reaction.
5. From a chemical equation, the time required for the completion of the equation is not known.
6. A reaction whether slow or fast does not know from the equation.
7. Equation does not provide information regarding the nature of the reactants and products viz. solid, liquid or gas.

Question 9.
What is meant by ‘balancing’ of a chemical equation ? Why it is necessary?
Answer:
Balancing of a chemical equation : It means making both the sides of the equation equal in respect of the kind and number of the atoms of the elements involved.
Balancing of a chemical equation is necessary : Due to the conservation of mass and indestructibility of matter, no atoms can be created or destroyed in a chemical reaction. Hence, the same kind of atoms in same numbers must be present in both the sides of the chemical equation.

Question 10.
Explain the method of balancing a chemical equation by trial and error method.
Answer:
Balancing of a chemical equation by trial and error method :
(i) In this method the proper numbers are putting before reactants and products so that the number of atoms in both sides are equal.
(ii) In doing so, we must cautious to see that all the reactants and products exist as molecules, and not as atoms, as free existence of atoms is not possible.

Question 11.
Balance the equation KClO₃ ⟶ KCl + O₂ by trial and error method.
Answer:
KClO₃ ⟶ KCl + O₂; it is seen that the number of atoms of oxyen in left hand side is 3 whereas in the right hand side it is 2. To equalize the number of atoms of oxygen in both sides it requires to multiply KClO₃ by 2 and oxygen by 3.
2 KClO₃ ⟶ KCl + 3 O₂. So as to balance this equation if KCl is multiplied by 2 then the equation is properly balanced.
2 KClO₃ = 2 KCl + 3 O₂

Question 12.
Write the following as balanced equations.
(i) Cu + HNO₃ ⟶ Cu(NO₃)₂ + NO + H₂ O
(ii) Pb(NO₃)₂ ⟶ PbO + NO₂ + O₂
(iii) Al + NaOH + H₂ O ⟶ NaAlO₂ + H₂
(iv) CuO + NH₃ ⟶ Cu + N₂ + H₂ O
Answer:
Balanced equations are :
(i) 3 Cu + 8 HNO₃ = 3 Cu(NO₃)₂ + 2NO + 4H₂ O
(ii) 2 Pb(NO₃)₂ = 2 PbO + 4 NO₂ + O₂
(iii) 2 Al + 2 NaOH + 2 H₂ O = 2 NaAlO₂ + 3H₂
(iv) 2 NH₃ + 3 CuO = 3 Cu + 2 N₂ + 3H₂O

Numerical problems :

Working formula :

(i) Molecular weight (M) = n × Emperical formula
(ii) Atomic weight of a gaseous element = \(\frac{\text { Actual yield }}{\text { Theoretical yield }} \times 100\)
Problems related to mass-mass relationship

Example 1:
How many grams of oxygen evolve when 122.5 g potassium chlorate is heated ? (Given, K = 39, Cl = 35.5, O = 16)
Answer:
The balanced equation is :
2 KClO = 2 KCl + 3 O₂
2[39 + 35.5 + 3 × 16] g & 3[2 × 16] g
= 245 g = 96 g
By heating 245 g KClO₃ 96 g O₂ is obtained
∴ By heating 122.5 g KClO₃ \(\frac{96 \times 122.5}{245}\) = 48 g O₂ is obtained

Example 2:
2.6 g zinc is treated with excess dil H₂ SO₄; how many gram oxygen combines with the evolved hydrogen?
Answer:
The balanced equation for production of hydrogen is :
Zn + H₂ SO₄ = ZnSO₄ + H₂
65g (2 × 1) g = 2g
So, 65 g zinc produces 2 g hydrogen
∴ 2-6 zinc produces \(\frac{2 \times 2.6}{65} \mathrm{~g}\) = 0.089 g hydrogen
Now, the reaction where hydrogen and oxygen combine is :
2 H₂ + O₂ = 2 H₂ O
So, 4 g hydrogen combine with 32 g oxygen 0.08 g hydrogen combine with \(\frac{32 \times 0.08}{4} \mathrm{~g}\) = 0.64 g oxygen

Example 3:
What is the observed loss in weight of 5 g calcium carbonate when it undergoes thermal decomposition?
Answer:
The balanced equation is :
CaCO₃ = CaO + CO₂
(40 + 12 + 16 × 3)g (12 + 16 × 2)g
= 100g = 44g
Loss in weight in the weight of CO₂ that escapes
100 g CaCO₃ produces 44g CO₂
∴ 5 g CaCO₃ produces \(\frac{44 \times 5}{1000}\) g = 2.2g CO₂

Example 4:
What is the percentage of ammonia in that quantity of ammonium chloride that can produce 5g ammonia?
Answer:
The balanced equation of reaction is :
2 NH₄ Cl + CaO = 2 NH₃ + CaCl₂ + H₂ O
2[14 + 1 × 4 + 35.5] g 2[14 + l × 3] g
= 107 g = 34 g
So, 34 g ammonia is obtained form 107 g NH₄ Cl

Example 5:
What weight of potassium chlorate of 96% purity will yield 4.8 g oxygen on complete thermal decomposition?
(Given, K = 39, Cl = 35.5, O = 16)
Answer:
The balanced equation is :
2 KClO₃ = 2 KCl + 3 O₂
245 g 96 g
∴ 96 g oxygen is obtained from 245 g KClO₂ of 100% purity
∴ 4.8 g oxygen is obtained from \(\frac{245 \times 4 \cdot 8}{96}\) g
= 12.25 g KClO₃ of 100% purity.
Let x gram of 96% purity contains 12.25 g KClO₃ of 100% purity
∴ \(\frac{96}{100}\).x = 12.56
or, x = \(\frac{12 \cdot 25 \times 100}{96}\) = 12.76 (approx)
So, the required quantity of KClO₃ = 12.76g

Example 6:
On strong heating limestone decomposes into quicklime and carbon dioxide. How much quantity of limestone will produced on complete decomposition, 30 g of quicklime by the above reaction?
Answer:
The balanced equation is :
CaCO₃ = CaO + CO₂
[40 + 12 + 3 × 16] g [40 + 16] g
= 100 g = 56 g
So, 56 g CaO is obtained by the complete decomposition of 100 g CaCO₃
∴ 30 g CaO is obtained by the complete decomposition of
\(\frac{100 \times 30}{56}\)g = 53.6 g CaCO₃
Thus 53.6 g limestone will have to be decomposed.

Example 7:
How many grams of magnesium metal will give 1.2 g hydrogen on complete reaction with dilute H₂ SO₄ (Mg = 24, H = 1)
Answer:
The balanced equation is :
Mg + H₂ SO₄ = MgSO₄ + H₂
24 g (1 × 2) g = 2 g
So, 2 g H₂ is obtained from 24 g Mg
∴ 1.2 g H₂ is obtained from \(\frac{24 \times 1.2}{2}\)g Mg = 14.4 g Mg
So, 14.4 g Mg will be required.
Problems based on mass-volume relationship

Example 8:
What volume of carbon dioxide measured at 300 K and 720 mm pressure be obtained on treatment of 1 g CaCO₃ with dilute HCl ?
Answer:
The balanced equation is :
CaCO₃ + 2 HCl = CaCl₂ + H₂O + CO₂
1 mol(40 + 12 + 3 × 16) g        1 mol (22.4 lit at NTP)
= 100 g
So, 100g CaCO₃ gives 22.4 lit CO₂ at NTP
1g CaCO₃ gives 0.224 lit CO₂ at NTP

Reducing the volume to the given condition applying gas equation,

P₁ = 760 mm
V₁ = 0.224 lit
T₂ = 273 K
P₂ = 720 mm
V₁ = ?
T₂ = 300 K

= 0-2598 lit = 259-8 ml
Hence, 259.8 ml CO₂ will be obtained at 300 K and 720 mm pressure on treatment of 1 g CaCO₃ with HC 1.

Example 9:
How much potassium nitrate should be heated to get enough oxygen required to completely burn 56 lit of hydrogen at NTP ?
Answer:
The balanced equation is :

= 2 × 22-4 lit
= 44.8 lit (at NTP)
So, 44.8 lit H₂ requires 22.4 lit O₂ at NTP
56 lit H, requires \(\frac{2 \cdot 24 \times 56}{44 \cdot 8}\) at NTP
= 28 lit O₂ at NTP

The other balanced equation is :

= 202 g
Now, 22.4 lit O₂ at NTP are obtained by heating 202 g KNO₃
∴ 28 lit O₂ at NTP are obtained by heating \(\frac{202}{22.4}\) × 28 g KNO₃
= 252.5 g KNO₃

Problems based on volume-volume relationship.

Example 10:
In the Ostwald process for the manufacture of nitric acid, ammonia gas is burnt in oxygen in the presence of a pt-catalyst. What volume of O₂ is required and what volume of NO is formed in the combustion of 500 lit of NH₃.
Answer:
The balanced equation is :

(i) 4 lit of NH₃ requires 5 lit of O₂ for combustion
500 lit of NH₃ requires \(\frac{5 \times 500}{4}\) lit = 625 lit O₂
(ii) 4 lit of NH₃ produces 4 lit NO
∴ 500 lit of NH₃ produces \(\frac{4}{4}\) × 500 lit NO = 500 lit NO

Example 11:
Calculate the volume of oxygen necessary to burn completely 5 lit butane gas. What is the volume of carbon dioxide formed?
Answer:
The balanced equation is :

So, 2 lit of butane at NTP requires 13 lit O₂ at NTP
∴ 5 lit of butane at NTP requires \(\frac{13 \times 5}{2}\) lit = 32.5 lit of O₂ at NTP.
Also 2 lit of butane at NTP produce 8 lit CO₂ at NTP
∴ 5 lit of butane of NTP produce
= \(\frac{8}{2}\) × 5 lit = 20 lit CO₂ at NTP

Detailed explanations in West Bengal Board Class 10 Physical Science Book Solutions Chapter 8.5 Metallurgy offer valuable context and analysis.

WBBSE Class 10 Physical Science Chapter 8.5 Questionuestion Answer – 8.5 Metallurgy

Very Short Answer Type Questions

Question 1.
Which metal is present in the earth’s crust in largest percentage ?
Answer:
Aluminium.

Question 2.
What is stainless steel ?
Answer:
Stainless steel is an alloy of iron with chromium and nickel.

Question 3.
What is the purpose of galvanising an article ?
Answer:
The purpose of galvanising an article to protect the article from corrosion.

Question 4.
What is the action of alkali on iron ?
Answer:
Iron does not react with any alkali.

Question 5.
How hydrogen gas may be prepared using aluminium ?
Answer:
Hydrogen gas may be prepared by boiling aluminium powder with alkali.

Question 6.
What is the basic component of chuni (ruby), panna (emarald) etc.?
Answer:
The basic component of chuni and panna is Al₂O₃.

Question 7.
What is an ore ?
Answer:
Ores are the minerals from which the metals can be extracted conveniently and profitably.

Question 8.
Name a metal that reacts both with an acid and alkali to produce salt and hydrogen.
Answer:
Zinc or Aluminium.

Question 9.
Name the chief ore of Zinc and write down its formula.
Answer:
The chief ore of Zinc is Zinc blende. Formula of zinc blende ZnS

Question 10.
Burning of which metal cannot be extinguished with CO₂ gas ?
Answer:
Burning of magnesium cannot be extinguished with CO₂ gas.

Question 11.
Which metals are present in brass ?
Answer:
Copper and Zinc are present in brass.

Question 12.
Name an alloy of magnesium.
Answer:
Electron is an alloy of magnesium.

Question 13.
Which type of iron is used in the core of an electromagnet ?
Answer:
Soft iron is used in the core of an electromagnet.

Question 14.
Which metal is commonly used for galvanisation ?
Answer:
Zinc is commonly used for galvanisation.

Question 15.
Name a metal that produces amphotaric oxide.
Answer:
Aluminium or Zinc produces amphoteric oxide.

Question 16.
Name two metals which do not react with alkali.
Answer:
Copper, iron do not react with alkali.

Question 17.
Which metal can produce hydrogen from dilute nitric acid ?
Answer:
Magnesium can produce hydrogen from dilute nitric acid.

Question 18.
Name the chief ore of magnesium.
Answer:
The chief ore of magnesium is Magnesite (MgCO_s).

Question 19.
Name the principle ore of aluminium.
Answer:
The principle ore of aluminium is Bauxite (Al₂O₃, 2H₂O),

Question 20.
Name two alloys of aluminium.
Answer:
Two alloys of aluminium are :

• Duralumin
• Aluminium bronze

Question 21.
What is metallurgy ?
Answer:
Metallurgy is the process of extracting metals from their ores.

Question 22.
What is gangue ?
Answer:
Gangue or matrix are the rocky and earthly impurities associated with the minerals.

Question 23.
What is slag ?
Answer:
Slag is the light and fusible material obtained by the combination of flux with gangue.

Question 24.
What is Flux ?
Answer:
Flux is the substance which combines with gangue to form light and easily fusible material called slag.

Question 25.
What is thermite ?
Answer:
Thermite is the mixture of metal oxide and the aluminium powder.

Question 26.
What is amalgamation ?
Answer:
Amalgamation is the process in which finely powdered ore is brought into contact with mercury which combines in the ore to form amalgam.

Question 27.
Why alkali metals are not found in free state in nature ?
Answer:
Due to high reactivity, alkali metals do not occur free in nature.

Question 28.
What is called fusion mixture ?
Answer:
A mixture of Na₂CO₃ and K₂CO₃ is called fusion mixture.

Question 29.
What is Black ash ?
Answer:
Mixture of Na₂CO₃ and CaS is called black ash.

Question 30.
What is Lime light ?
Answer:
On heating in oxy-hydrogen flame, lime becomes incandescent and emits bright white light, called lime light.

Question 31.
What is American baking powder ?
Answer:
Pure Ca(H₂PO₄)₂ is used as American baking powder.

Question 32.
What is the use of MgSO₄, 7H₂O?
Answer:
MgSO₄, 7H₂O is used as a purgative in medicine.

Question 33.
What is Hydrolith ?
Answer:
Calcium hydride is known as hydrolith.

Question 34.
What is the constituent of bones and teeth ?
Answer:
Calcium phosphate is the constituent of bones and teeth.

Question 35.
What is the most abundant metal next to aluminium ?
Answer:
Iron is the most abundant metal, next to aluminium.

Question 36.
What is Cementite ?
Answer:
Iron carbide (Fe₃C) is known as cementite.

Question 37.
What is Green vitriol ?
Answer:
FeSO₄,7H₂O is called green vitriol.

Question 38.
What is called Mohr’s salt ?
Answer:
FeSO₄,(NH₄)₂SO₄, 6H₂O is called Mohr’s salt.

Question 39.
What is Kipp’s base ?
Answer:
Mixture of FeS + H₂SO₄ is called Kipp’s base.

Question 40.
What is Invar ?
Answer:
Invar is an alloy of steel containing 36% nickel.

Question 41.
What is Spiegeleisen ?
Answer:
Spiegeleisen is an alloy of iron, manganese and carbon used in steel making.

Question 42.
What is Matte ?
Answer:
Matte contains Cu₂S + FeS.

Question 43.
What is Blister Copper ?
Answer:
Blister Copper contains (96 -98)% copper with small amounts of Ag and Au as impurity.

Question 44.
What is called Fool’s gold ?
Answer:
CuFeS₂ is called Fool’s gold.

Question 45.
What Nila thotha ?
Answer:
Blue vitriol (CuSO₄, 5H₂O) is called ‘Nila thotha’.

Question 46.
What is Bordeaux mixture?
Answer:
Mixture of CuSO₄ solution and lime called Bordeaux mixture is used as fungicide.

Question 47.
What is Philosopher’s wool ?
Answer:
Zinc oxide is called philosopher’s wool, zinc white or Chinese white.

Question 48.
What is the nature of ZnO ?
Answer:
ZnO being amphoteric in nature dissolves both in acids and alkalis.

Question 49.
What is Lithopone ?
Answer:
Lithopone (ZnS + BaSO₄) is used as white paint.

Question 50.
What is the use of ZnS ?
Answer:
ZnS is used for preparing luminous dials for watches and X-ray screens.

Question 51.
What is German silver ?
Answer:
German silver is an alloy of Cu (60%), Zn (20%) and Ni (20%). It does not contain silver.

Question 52.
What is White vitriol ?
Answer:
Zinc sulphate hepta hydrate (ZnSO₄, 7H₂O) is called white vitriol

Question 53.
Which metal is common in both bell metal and bronze?
Answer:
Bell metal and bronze are both allloys of copper and tin.

Question 54.
What is the non metallic component present in stainless steel?
Answer:
The non-metallic component of stainless steel is carbon (c).

Question 55.
What is the reason behind Wilson’s disease?
Answer:
This occurs due to abnormal metabolism of copper and as a result, free copper in the plasma enters different tissues, binds with proteins and gets deposited in liver, kidney and brain.

Question 56.
Write the chemical reaction involved in thermite process.
Answer:
The chemical reaction involved is as follows :
Fe₂O₃ + 2Al → 2Fe + Al₂O₃ + heat

Question 57.
What is anodizing ?
Answer:
Anodizing is a process by which a thick, protective layer of aluminium oxide is applied on the aluminium metal surface to protect it from corrosion.

Question 58.
Why does a new aluminium vessel lose its shine?
Answer:
In presence of air, a thin layer of aluminium oxide is formed on the surface of metallic aluminium. So, the aluminium vessel loses its shine.
4Al + 3O₂ = 2Al₂O₃

Question 59.
What is the principle behind extracting less reactive metals?
Answer:
Metals with less reactivity are extracted by heating their oxides.

Question 60.
What is the principle behind extracting highly reactive metals?
Answer:
Metals of high reactivity are extracted by the electrolytic reduction of their molten chlorides or oxides. During electrolysis, the pure metal is produced at the cathode.

Question 61.
What is the principle behind extracting moderately reactive metals?
Answer:
Metals which are moderately reactive are extracted by reduction of their oxides with carbon (or zinc or iron etc.)

Question 62.
Rusting is a redox process. What is the oxidation reaction?
Answer:
The oxidation process is the oxidation of metallic ion to Fe²⁺ and finallly to Fe³⁺ ion occurring at the anode.

Short Answer Type Questions:

Question 1.
Concentrate Nitric acid can be kept in vessel made of aluminium why?
Answer:
Reason Concentrate Nitric acid does not react with aluminium, so it can be kept in aluminium vessel.

Question 2.
Should we take or not ‘pickle’ wrapped to aluminium foils ?Give reasons.
Answer:
Reason : Pickle contain organic acetic acid known as vinegar, which reacts with aluminium foil to produce aluminium salts which are harmful to our health. So pickle’s wrapped in aluminium foils should be taken.

Question 3.
What happens when a spoon made of iron is introduced in acidified CuSO₄ solution ?
Answer:
Explanation : Spoon made of iron reacts with acidified CuSO₄ solution precipitation metallic copper and blue copper sulphate solution turns green due to formation of ferrous sulphate.
Equation : CuSO₄ + Fe = FeSO₄ + Cu↓

Question 4.
In the burning of magnesium carbon-dioxide is not used as a fire ex­tinguisher why ?
Answer:
Explanation : Burning Magnesium produces heat which breaks carbon dioxide to carbon and oxygen. This oxygen enhance magnesium burning. SO₂, CO₂ is not used to extinguish magnesium burning.
Equation : Mg + CO₂ = MgO + C

Question 5.
Rain damages lajmahal. Do you agree ? Give reason.
Answer:
Reason : Rain water contains nitric acid. The nitric acid is formed by natural ways in the following manner. Nitrogen reacts with oxygen, both present in v air, by thunder to form nitric oxide. Nitric oxide further reacts with oxygen to form nitrogen dioxide.

Nitrogen dioxide dissolves in rain water to produce nitric acid. Tajmahal is made of lime stone i.e. Calcium carbonate (CaCO₃). Nitric acid (HNO₃) reacts with CaCO₃ to form Ca(NO₃)₂. Thus rain damages Tajmahal.
Equation : CaCO₃ + 2HNO₃ = Ca(NO₃)₂ + CO₂+ H₂O

Question 6.
What is Thermite ? What is its use ?
Answer:
Thermite : Thermite is a mixture of aluminium powder and ferric oxide.
Use : It is used for welding purposes.

Question 7.
State what happens when :
Zn is added to caustic soda solution
Answer:
Explanation : Zinc reacting with caustic soda solution produces sodium zincate and hydrogen gas.
Equation : Zn + 2NaOH = Na₂ZnO₂ + H₂↑

Question 8.
State what happens when :
Steam is passed over red hot iron.
Answer:
Explanation : When steam is passed over red-hot iron (600°C – 800°C), hydrogen is set free and iron is oxidised to ferrosoferric oxide.
Equation : 3Fe + 4H₂O = Fe₃O₄ + 4H₂↑

Question 9.
State what happens when :
Steam is passed over red hot zinc.
Answer:
Explanation : When steam is passed over red hot zinc, zinc oxide and hydrogen gas form.
Equation : Zn + H₂O= ZnO + H₂↑

Question 10.
What compounds are formed when magnesium is burnt in air ?
Answer:
Explanation : Magnesium oxide (MgO) and magnesium nitride (Mg₃N₂) are formed when magnesium is burnt in air.
Equation :
(a) 2Mg + O₂ = 2MgO
(b) 3Mg + N₂ = Mg₃N₂

Question 11.
What is Galvanisation ? State one use of Zinc.
Answer:
Galvanisation : It is a process of coating an article with zinc. The purpose of galvanisation an article is to protect it from corrosion. Iron articles are galvanised to protect the articles from rusting.
Use of Zinc : Zinc is largely used to prepare zinc white, a paint.

Question 12.
‘All ores are minerals but all minerals are not ores’ — Explain.
Answer:
Explanation : Compounds of a metal which exist in combination with similar compounds of other metals are known as minerals. A metal may occur in many minerals. The particular mineral from which a metal may be conveniently and eco­nomically extracted is called the ore of the metal.

Question 13.
What is Stainless steel ? State one use of it.
Answer:
Stainless steel : It is an alloy which composes Iron (Fe) = 73%, Chro­mium (Cr) = 18% and Nickel (Ni) = 8% and Carbon (C)
Uses of stainless steel : It is broadly used to make instruments.

Question 14.
What is Philosopher’s wool ?
Answer:
Philosopher’s wool : Zinc oxide is called philosopher’s wool, zinc white or Chinese white. It is a white powder which becomes yellow on heating and again becomes white on cooling. It is used as a white fluorescent paint because it is not darkened by hydrogen sulphide.

Question 15.
What is an alloy? Name one alloy.
Answer:
Alloy : An alloy is a homogeneous mixture (or, sometimes a heterogeneous combination) of two or more metals, behaving as a single metal in most of its physical properties.
Example : Bronze (Cu : 90% ; Sn : 10%)

Question 16.
State the advantages of an alloy over pure metal.
Answer:
Advantages of an alloy over pure metals :

• Increase of hardness.
• Increase in resistance to corrosion.
• Increase in fusibility or decrease in melting point.
• Improvement of casting property.

Question 17.
Two metals A and B produce hydrogen when react with hot NaOH solution. A does not react with H₂SO₄ but B produces a salt and hy­drogen gas reacting with H₂SO₄ Identify A and B.
Answer:
Identification : The metal A is aluminium and the metal B is zinc both of which react with hot NaOH solution to produce hydrogen.

Aluminium does not react with H₂SO₄ but zinc reacts with H₂SO₄ to produce salt and hydrogen.
Equation : Zn + H₂SO₄ = ZnSO, + H₂↑

Question 18.
What is the difference between mineral and ore of a metal ?
Answer:
Difference between mineral and ore of a metal :

Mineral	Ore
Compounds of a metal which exist in combination with similar compounds of other metals are known as minerals A metal may occur in many minerals.	The particular mineral from which a metal may be conveniently and economically extracted is called the ore of the metal.

Question 19.
Why alumina (Al₂O₃)cannot be reduced by carbon ?
Answer:
Explanation At high temperature, Al₂O₃ reacts with carbon to form alu­minium carbide.
Equation : \(2 \mathrm{Al}_2 \mathrm{O}_3+9 \mathrm{C} \rightleftharpoons \mathrm{Al}_4 \mathrm{C}_3+6 \mathrm{CO}\)

Question 20.
Why aluminium cannot be obtained by the electrolysis of fused AlCl₃?
Answer:
Explanation Aluminium cannot be obtained by the electrolysis of fused AlCl₃ since it is covalent solid and sublimes at 453K.

Question 21.
Although less conducting than copper, aluminium is used for power transmission. Why ?
Answer:
Explanation : Aluminium being lighter and cheaper than copper is used for power transmission.

Question 22.
What is the role of cryolite (Na₃AlF₆) in the electro-chemical reduc­tion of Al₂O₃ during the preparation of aluminium ?
Answer:
Explanation : Cryolite (Na₃AlF₆) is added to alumina ;

• to decrease its melting point from 2273K to 1173K.
• to increase its electrical conductivity.

Question 23.
Why aluminium acts as a good reducing agent ?
Answer:
Explanation : Reducing character of a substance depends upon its affinity for oxygen. Aluminium due to its high affinity for oxygen is a good reducing agent. It reduces a large number of oxides of other metals. e.g. 2Al + Fe₂O = Al₂O₃ + 2fe + heat.

Question 24.
Give reasons for the following:
Although aluminium is above hydrogen in electrochemical series, it is stable in air and water.
Answer:
Explanation : Aluminium reacts readily with air and water and a thin layer of its oxide gets deposited on its surface. This oxide coating protects the underlying metal from further action.

Question 25.
Aluminium containers can be used to store cone. HNO₃
Answer:
Explanation : Aluminium on treatment formation of a protective coating of its oxide. Thus aluminium containers can be used to transport cone. HNO₃

Question 26.
Finely powdered aluminium on exposure to air becomes hazadous. Why
Answer:
Explanation : Aluminium due to its great affinity for oxygen forms Al₂O₃ and the reaction is highly exothermic. Finely divided aluminium powder due to its large surface area, reacts vigorously with air and is hazardous.

Question 27.
Explain the following :
Anode mud in copper refining contains silver and gold.
Answer:
Explanation Silver and gold being less electropositive than copper are not ionised under the applied voltage and get deposited in the anode mud.

Question 28.
Explain the following :
Copper metal is largely used to make electrical cables.
Answer:
Explanation : Copper mainly used in making electrical cables because it is a good conductor. Moreover, being a noble metal, it is not affected by the atmosphere.

Question 29.
In moist air, copper corrodes to produce a green layer on the surface. Explain.
Answer:
Explanation : In presence of moist air, a thin layer of green basic copper carbonate is formed on the surface of copper leading to its corrosion.

Question 30.
Copper salts are coloured where as Zinc salts are colourless. Why
Answer:
Reason Copper salts are coloured because of the presence of an unpaired electron in Cu²⁺. This electron absorbs radiations of orange colour from white light for excitation from one energy level to another with the same d-subs shell. Hence, transmitted light appears blue. On the other hand, zinc salts are white because of the absence of vacant orbitals to which the electrons can be excited.

Question 31.
Explain why lime stone is used in the manufacture of pig iron from haematite.
Answer:
Explanation On heatingTime stone decomposes to give CaO which then combines with silica to form slag. Equation :
(a) CaCO₂ \(\rightleftharpoons\) CaO + CO₂
(b) SiO₂ + CaO = CaSiO₃ (slag)

Question 32.
What is the difference between cast iron. wrought iron and steel?
Answer:
Explanation The three forms differ in the percentage of carbon. Cast iron contains (2 -4-5)% carbon, wrought iron contains about 0-25% carbon, while steel contains (0T-T5)% carbon.

Question 33.
What is amalgam? Give example!
Answer:
Amalgam : If one of the components of an alloy is mercury then this alloy.

Broad Answer Type Questions

Question 1.
State the following:
(i) Chief one
(ii) Important properties and equations
(iii) Uses of:
(a) Aluminium
(b) Copper
(c) Iron
(d) Magnesium
(e) Zinc.
Answer:
List of chief ore, propetites, uses of Al, Cu, Fe, Mg, Zn :

Question 2.
State some alloy. with their composition and use :
Answer:
Common alloys of Al, Mg, Zn

Well structured WBBSE Class 10 Physical Science MCQ Questions Chapter 4 Thermal Phenomena can serve as a valuable review tool before exams.

Thermal Phenomena Class 10 WBBSE MCQ Questions

Multiple choice questions (MCQ) :

Question 1
The Fahrenheit and kelvin scales of temperature will the same reading at
(A) -40
(B) 313
(C) 574.25
(D) 732.25
Answer:
(B) 5 ?

Question 2
At what temperature, volume of an ideal gas at 0°C becomes triple?
(A) 182°C
(B) 819°C
(C) 546°C
(D) 646°C
Answer:
(C) 546°C

Question 3.
The specific heat of ice at 0°C melting into at 0°C is:
(A) zero
(B) infinity
C) more than zero
(D) less than zero
Answer:
(B) infinity

Question 4.
Boiling water is changing into steam. The specific heat of boiling water is:
(A) Zero
(B) One
(C) infinity
(D) less than one
Answer:
(C) infinity

Question 5.
Which of the following has the highest specific heat?
(A) copper
(B) water
(C) hydrogen
(D) silver
Answer:
(C) hydrogen

Question 6.
One gram of ice at 0°C is added at 5 g of water to 10°C. Final temperature of the mixture is:
(A) -5°C
(B) 5°C
(C) 0°C
(D) none of these
Answer:
(A) -5°C

Question 7.
The specific heat of an ideal gas varies with temperature T as :
(A) T¹
(B) T²
(C) T^-1
(D) T⁰
Answer:
(D) T⁰

Question 8.
22 g CO₂ at 27°C is mixed with 16 g of oxygen at 37°C. The temperature of the mixture is :
(A) 32°C
(B) 27°C
(C) 37°C
(D) 30°C
Answer:
(A) 32°C

Question 9.
A ballon contains 500 m³ of He at 27°C and 1 atmospheric pressure. The volume of He at -3°C and 0.5 atmospheric pressure will be:
(A) 700 m³
(B) 900 m³
(C) 1000 m³
(D) 500 m³
Answer:
(B) 900 m³

Question 10.
The specific heat of a gas in a gas in an isothermal process is:
(A) infinite
(B) zero
(C) negative
(D) remains constant
Answer:
(A) infinite

Question 11.
100 g of ice is mixed with 100 g of water at 100°C. The final temperature of the mixture is:
(A) 10°C
(B) 20°C
(C) 40°C
(D) 30°C
Answer:
(A) 10°C

Question 12.
Heat given to a body which rises its temperature by 1°C is:
A water equivalent
(B) specific heat
(C) thermal capacity
(D) temperature gradient
Answer:
(C) thermal capacity

Question 13.
During the adiabatic process, the pressure of a gas is found to be proportional to the cube of its absolute temperature.
The ratio \(\fracC_p}C_v}\) for gas is :
(A) \(\frac{4}3}\)
(B) 2
(C) \(\frac{5}3}\)
(D) \(\frac{3}2}\)
Answer:
(D)

Question 14.
A gaseous mixture consists of 16 g of Helium and 16 g Oxygen. The ratio \(\fracC_p}C_v}\) of the mixture is :
(A) 1.54
(B) 1.4
(C) 1.63
(D) 1.59
Answer:
(C) 1.63

Question 15
Two bars of copper having same length but unequal cross-section are heated to the same temperature. The change in length will be:
(A) equal in both bars
(B) more in thicker bar
(C) more in thinner bar
(D) cannot say
Answer:
(A) equal in both bars

Question 16
A body cools from 60°C to 50°C in 10 min. If room temperature be 25°C, temperature of the body at the end of next 10 min will be:
(A) 38.5°C
(B) 40°C
(C) 45°C
(D) 42.85°C
Answer:
(D) 42.85°C

Question 17
A body takes T minutes is cool from 62°C to 61°C when the surrounding temperature is 30°C. The time taken by the body to cool is 30°C. The time taken by the body to cool 46°C to 45°C is
(A) greater than T minute
(B) equal to T minute
(C) less than T minute
(D) equal to T/2
Answer:
(A) greater than T minute

Question 18
If the temperature of a block body is doubled, the wavelength at which the spectral radiancy has its maximum is :
(A) doubled
(B) halved
(C) quadrupled
(D) unchanged
Answer:
(B) halved

Question 19
A black body has maximum wavelength 1 m at 2000 K. Its corresponding wavelength at 3000 K will be :
(A) \(\frac{3}{2}\) λ m
(B) \(\frac{2}{3}\) λ m
(C) \(\frac{16}{81}\) λ m
(D) \(\frac{81}{16}\) λ m
Answer:
(B) \(\frac{2}{3}\) λ m

Question 20.
A body cools from 50°C to 40°C in 5 minutes. Its temperature comes down to 33.33°C in next 5 minutes. The temperature of surrounding is:
(A) 15°C
(B) 20°C
(C) 25°C
(D) 10°C
Answer:
(B) 20°C

Question 21
The rate of cooling at 600 K, if surrounding temperature is 300 K is R. The rate of cooling at 900 K is :
(A) \(\frac{16}{3}\) R
(B) 2 R
(C) 3 R
(D) \(\frac{2}{3}\) R
Answer:
(A) \(\frac{16}{3}\) R

Question 22
If I_m denotes the wavelength at which the radiative emission from a black body at a temperature TK is maximum, then
(A) λ_m ∝ T
(B) λ_m ∝ T^-1
(C) λ_m ∝ T²
(D) λ_m does not depend on T.
Answer:
(B) λ_m ∝ T^-1

Question 23
Two spheres made of same material have radii in the ratio 1 : 2. Both are at same temperature. Ratio of heat radiation energy emitted per second by them is:
(A) 1 : 2
(B) 1 : 4
(C) 1 : 8
(D) 1 : 16
Answer:
(B) 1 : 4

Question 24.
The coefficient of linear expansion of a solid is :
(A) 3 γ
(B) 2 γ
(C) γ
(D) γ / 3
Answer:
(D) γ / 3

Question 25.
A good insulator of heat is
(A) Copper
(B) Mercury
(C) trapped air
(D) Iron
Answer:
(C) tropped air

Question 26.
A bimetallic strip bends on heating due to :
(A) Uneven expansions
(B) Same expansion
(C) No expansions
(D) None of these
Answer:
(A) Uneven expansions

Question 27.
The coefficient of linear expansion of a solid depends on :
(A) unit of length
(B) scale of temperature
(C) density of the material
(D) None of these
Answer:
(B) scale of temperature

Question 28.
A bimetallic strip bends upon heating because of
(A) same expansion
(B) uneven expansion
(C) no expansion
(D) twisting
Answer:
(B) uneven expansion

Question 29.
If the value of coefficient of linear expansion is 1.5 × 10^-4 ° C^-1 then value of coefficient of superficial expansion is :
(A) 4.5 × 10^-4 °C^-1
(B) 3.0 × 10^-4 ° C^-1
(C) 6.0 × 10^-4 ° C^-1
(D) 7.5 × 10^-4 ° C^-1
Answer:
(B) 3.0 × 10^-4 ° C^-1

Question 30.
When a solid metallic sphere is heated, the largest percentage increase occurs in its.
(A) Diameter
(B) Surface area
(C) Volume
(D) Density
Answer:
(C) Volume

Question 31.
For a liquid, the coefficient of apparent expansion (δ_a) and coefficient of real expansion (γ) are related as :
(A) δ_a = γ_r
(B) γ_a > γ_ru
(C) γ_a < γ_r
(D) γ_a / γ_r = constant
Answer:
(C) γ_a < γ_r

Question 32.
Coefficient of linear expansion of the following metals are in the order
(A) aluminium < copper < iron
(B) copper < iron < aluminium
(C) copper < aluminium < iron
(D) aluminium > copper > iron
Answer:
(D) aluminium > copper > iron

Question 33.
The thermal conductivity of a rod is 2. what is its resistivity?
(A) 0.5
(B) 1
(C) 0.25
(D) 2
Answer:
(A) 0.5

Question 34.
Thermal conductivity of which of the following is the maximum?
(A) copper
(B) silver
(C) diamond
(D) platinum
Answer:
(C) diamond

Question 35.
The magnitude of thermal conductivity of the following substances are in the order.
(A) silver > aluminium > glass > wood
(B) aluminium > silver > glass > wood
(C) silver > aluminium > wood > glass
(D) aluminium > silver > wood > glass
Answer:
(A) silver > aluminium > glass > wood

Question 36.
A liquid which is a good conductor of heat is :
(A) kerosin
(B) mercury
(C) water
(D) turpentine
Answer:
(B) mercury

Question 37.
For an ideal heat insulator, value of K is :
(A) zero
(B) 1
(C) 100
(D) α
Answer:
(A) zero

Fill in the blanks :

1. Heat is a form of _________.
Answer:
energy.

2. Three different types of motions are translational motion, vibrational motion and ___________.
Answer:
Rotational motion.

3. SI unit of heat is __________.
Answer:
Joule.

4. 1 calorie = __________ Jule.
Answer:
4.18

5. Temperatures are measured with a __________.
Answer:
thermometer.

6. ______ is the upper fixed point in Fahrenheit scale.
Answer:
212° F

7. Three types of expansions in solids are, linear expansion, superficial expansion and __________.
Answer:
volume expansion.

8. Real expansion of the liquid = expansion of the vessel + __________.
Answer:
apparent expansion of the liquid.

9. γ_s = γ_n + ________.
Answer:
γ₈

10. The volume of water is minimum at ______.
Answer:
4°C

11. The density of water is maximum at ______.
Answer:
4°C.

12. From Charle’s Law, we find γ_p = ______ °C^-1.
Answer:
\(\frac{1}{273}\)

13. From pressure law, we find γ_y= ________ °C^-1.
Answer:
\(\frac{1}{273}\)

14. Specific heat of water in SI system is ________.
Answer:
4200 Jkg^-1 K^-1.

15. The unit of thermal conductivity in SI system is ________.
Answer:
Jm^-1 s^-1 K^-1.

16. The unit of thermal conductivity in CGS system is ________.
Answer:
cm² s^-1

17. Carbon dioxide is a ________ gas.
Answer:
green house.

18. The expansion of a substance on heating is called ________ expansion.
Answer:
thermal.

19. The coefficient of linear expansion of a solid does not depend on unit of ________.
Answer:
length.

20. Thermal resistivity is the _______ of thermal conductivity.
Answer:
reciprocal.

21. In charles’ law, a _______ mass of gas is taken.
Answer:
given.

22. A liquid good conductor of heat is ________.
Answer:
mercury.

23. In summer the pendulum clock becomes ________.
Answer:
slower

24. The unit of γ (i.e, coefficlent of cubical expansion) in S.I unit is ________.
Answer:
K^-1

25. Material of the rod remaining same, longer the rod, ________ will be the increase in length of the rod for same increase in temperature.
Answer:
more.

26. If the value of α is 24 × 10^-6 °C^-1, then its value in S.I. unit is ________.
Answer:
24 × 10^-6 K^-1

27. Unit of β (coefficient of superficial expansion) is ________.
Answer:
°C^-1 or K^-1

28. For a particular solid substance, magnitude of β has the value of α [symbols have their usual meaning].
Answer:
twice

29. For two rods of same length and same area of cross-section, if temperature is raised by same amount, iron rod will expand ______ compared to that of the aluminium rod.
Answer:
less

30. The reciprocal of thermal conductivity is known as ________.
Answer:
thermal resistivity.

31. The S.I unit of thermal conductivity is ________.
Answer:
jm^-1.k^-1.s^-1

32. Diamond has ________ value of K (i.e., coefficient of thermal conduction) than copper.
Answer:
higher

33. Brass is a ________ conductor of heat.
Answer:
good

34. In solids, heat passes from hotter region to colder region by ________ processes.
Answer:
conduction

State whether the following statement is True or False : VSA

1. In winter the pendulum clock becomes slower.
Answer:
False

2. β (i.e. coefficient of superficial expansion) is the characteristic of the material.
Answer:
True

3. For an ideal gas, (δ i.e., coefficient of cubical expansion) = 1 / 273
Answer:
True

4. α, β and δ are related as follows α : β : δ = 1 : 2 : 3
[Symbols have their usual meaning]
Answer:
True

5. Real expansion of the liquid = Apparent expansion of the liquid+volume expansion of the container.
Answer:
True

6. The seasonal changes in a pendulum clock are due to the expansion or contraction of solid substances.
Answer:
True

7. The S.I. unit of thermal conductivity is jm^-2 ks^-1
Answer:
False

8. Usually metals are good conductors of heat than gases and nonmetals.
Answer:
True

9. Diamond has low value of K (i.e. coefficient of thermal conduction)
Answer:
False

10. In solids, heat passes from hotter region to colder region by convection processes.
Answer:
False

11. A substance with a large thermal conductivity is a good conductor while the one with a small thermal conductivity is a poor heat conductor.
Answer:
True

Well structured WBBSE Class 10 Physical Science MCQ Questions Chapter 8.4 Inorganic Chemistry in the Laboratory and in Industry can serve as a valuable review tool before exams.

Inorganic Chemistry in the Laboratory and in Industry Class 10 WBBSE MCQ Questions

(a) Ammonia

Multiple Choice Questions :

Question 1.
Ammonia is : ……………
(A) acidic
(B) basic
(C) neutral
(D) amphoteric
Answer:
(B) basic

Question 2.
The reaction N₂ + 3H₂ = 2NH₃ is ……………
(A) exothermic
(B) endothermic
(C) neither of the two
(D) Both of the two
Answer:
(A) exothermic

Question 3.
Liquid ammonia is used in refrigerators because : ……………
(A) It has a high dipole moment
(B) It has a high heat of evaporation
(C) of its basicity
(D) of its stability
Answer:
(B) It has a high heat of evaporation

Question 4.
High heat of vaporization of ammonia is due to its : ……………
(A) basic nature
(B) polar nature
(C) hydrogen bonding
(D) high solubility
Answer:
(C) hydrogen bonding

Question 5.
In the Ostwald process for the manufacture of HNO₃
(A) air is blown into an electric arc
(B) ammonia is catalytically oxidized
(C) chile saltpetre is treated with cone. H₂SO₄
(D) NaNO₃ is treated with cone. H₂SO₃
Answer:
(B) ammonia is catalytically oxidized

Question 6.
Which of the following statements is correct for the manufacture of ammonia by Haber’s process ?
(A) Low temperature, high pressure, presence of catalyst.
(B) High temperature, high pressure and catalyst
(C) Low temperature and pressure
(D) High temperature and low pressure
Answer:
(A) Low temperature, high pressure, presence of catalyst

Question 7.
Ammonia water makes a good cleaning agent because it: ……………
(A) is weakly basic
(B) emulsifies grease
(C) leaves no residue when wiped out
(D) all are true
Answer:
(D) all are true

Question 8.
A mixture of ammonia and air at about 800°C in the presence of Pt gauze forms : ……………
(A) N₂O
(B) NO
(C) NH₂OH
(D) NO
Answer:
(B) N₂O₃

Question 9.
Ammonium ion in solution is detected by ……………
(A) Brown-ring test
(B) Molish’s test
(C) Nessler’s solution
(D) Fehling’s solution
Answer:
(C) Nessler’s solution

Question 10.
The substance used for drying ammonia gas in the laboratory ……………
(A) cone. H₂SO₄
(B) P₂O₂
(C) quick lime
(D) silica gel
Answer:
(C) quick lime

Question 11.
Non-combustible hydride is : ……………
(A) NH₃
(B) PH₃
(C) ASH₃
(D) SbH₃
Answer:
(A) NH₃

Question 12.
Which is most explosive ?
(A) NCl₃
(B) PCl₃
(C) ASCl₃
(D) All
Answer:
(A) NCl₃

Question 13.
Ammonia gas is prepared in the laboratory by the action of slaked lime on ……………
(A) NH₄Cl
(B) (NH₄)₂SO₄
(C) NH₄Cl + NaNO₃
(D) NH₄NO₃
Answer:
(A) NH₄Cl

Question 14.
With excess of Cl₂ ammonia gives
(A) NCl₃
(B) HCl
(C) NH₄Cl
(D) N₂O
Answer:
(A) NCl₃

Question 15.
How NH₃ is generally manufactured for fertilizers ?
(A) by reducing the by product HNO₃
(B) passing a mixture of N₂ and H₂ under high pressure and moderate temperature over a catalyst
(C) by passing an electric discharge in the mixture of H₂ and N₂
(D) 2NH₄Cl + Ca(OH)₂ → CaCl₂ + 2NH₃ + 2H₂O
Answer:
(B) passing a mixture of N₂ and H₂ under high pressure and moderate temperature over a catalyst

Question 16.
Liquid NH₃ bottles are opened only after cooling for some time. This is because :
(A) NH₃ is corrosive liquid
(B) it is a mild explosive
(C) it brings tears in eyes
(D) it generates high vapour pressure.
Answer:
(D) it generates high vapour pressure

Question 17.
Aqueous solution of ammonia consists of :
(A) H⁺
(B) OH^–
(C) NH
(D) NH₄⁺+ OH^–
Answer:
(D) NH₄⁺+ OH^–

Question 18.
The vapour density of ammonia is:
(A) 7
(B) 7.5
(C) 8.5
(D) 17
Answer:
(C) 8.5

Question 19.
Nessler’s reagent is :
(A) K₂Hgl₄
(B) K₂Hgl₄ + KOH
(C) K₂Hgl₄
(D) K₂Hgl₄ + KOH
Answer:
(B) K₂Hgl₄ + KOH

Question 20.
Cupric hydroxide dissolves in aqueous ammonia due to
(A) reduction to cuprous hydroxide
(B) complex formation
(C) increase in pH
(D) the amphoteric nature of Cu(OH)₂
Answer:
(B) complex formation

Question 21.
The blue complex formed on addition of cone. NH₄OH solution to a Cu2+ salt solution has the structure :
(A) \(\left[\mathrm{Cu}\left(\mathrm{NH}_4\right)_4\right]^{2+}\)
(B) \(\left[\mathrm{Cu}\left(\mathrm{NH}_3\right)_2\right]^{2+}\)
(C) \(\left[\mathrm{Cu}\left(\mathrm{NH}_3\right)_4\right]^{2+}\)
(D) \(\left[\mathrm{Cu}\left(\mathrm{NH}_4\right)_2\right]^{2+}\)
Answer:
(C) \(\left[\mathrm{Cu}\left(\mathrm{NH}_3\right)_4\right]^{2+}\)

Question 22.
On addition of NH₄OH to a copper sulphate solution :
(A) blue precipitate of copper hydroxide is obtained
(B) black precipitate of copper oxide is obtained
(C) a deep blue solution is obtained
(D) no change is observed
Answer:
(C) a deep blue solution is obtained

Question 23.
In which the ammonia is not used ?
(A) Cold storage
(B) Anaesthetic
(C) Manufacture of rayon and plastic
(D) None of these.
Answer:
(B) Anaesthetic

Question 24.
In the reaction : \(\mathbf{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3,\) the catalyst used is :
(A) Pt and Cu
(B) Fe and Mo
(C) NO + Pt
(D) Ni + Ti
Answer:
(B) Fe and Mo

Question 25.
Ammonia can be obtained by heating ammonium sulphate with :
(A) KOH
(B) NaCl
(C) CaCl₂
(D) ZnSO₄
Answer:
(A) KOH

Question 26.
Ammonia is collected by :
(A) downward displacement of water
(B) downward displacement of air
(C) upward displacement of air
(D) by downward displacement of hot water
Answer:
(B) downward displacement of air

Question 27.
Ammonia is :
(A) basic
(B) acidic
(C) neutral
(D) insoluble in water
Answer:
(A) basic

Question 28.
Ammonium chloride and Ca(OH)₂ on heating produce :
(A) N₂
(B) NO₂
(C) NH₃
(D) NO
Answer:
(C) NH₃

Question 29.
Liquid ammonia contains :
(A) 35% NH₃
(B) 60% NH₃
(C) 80% NH₃
(D) 0.0% NH₃
Answer:
(A) 35%NH₃

Fill in the blanks

1. Ammonia gas is prepared by heating on ammonium salt mixed with a strong ……………………..
Answer:
base

2. Ammonia produces a white cloud with ……………………. acid.
Answer:
hydrochloric

3. Ammonia turns red litmus solution ……………………..
Answer:
blue

4. Ammonia has a typical ……………………. smell.
Answer:
pungent

5. Aqueous solution of ammonia is …………………….
Answer:
alkaline

6. A ……………. aqueous solution of ammonia is called liquor ammonia.
Answer:
Concentrated

7. Ammonia gas when passed over heated sodium, amide salt and ……………. gas produce.
Answer:
hydrogen

8. Since ammonia gas is …………….than air, it is collected by downward displacement of air.
Answer:
lighter

9. Ammonia is dried by passing through …………….
Answer:
quick lime

10. Ammonia is ………………. soluble in water.
Answer:
highly

11. In ammonia we have nitrogen and ……………..
Answer:
hydrogen

12. Ammonia gas is passed over heated black cupric oxide which is reduced to red metallic …………….
Answer:
copper

13. 2NH₃Cl + Ca(OH)₂ = _________ + CaCl₂ + 2H₂O
Answer:
2NH₃

14. When excess chlorine reacts ammonia forming nascent nitrogen which again combines with chlorine producing, ………… an oily yellow explosive compound.
Answer:
nitrogen trichloride.

15. ………… gas is obtained by heating ammonium sulphate with sodium hydroxide.
Answer:
Ammonia

16. ………… reagent is used for the identification of ammonia.
Answer:
Nessler’s

17. Ammonia is ………… for eyes.
Answer:
harmful

18. Ammonia gas is collected by the ………… displacement of air.
Answer:
downward.

19. Ammonia is dried with …………
Answer:
calcium oxide.

20. When ammonia leaks from factory we should wash our eyes with …………….
Answer:
water.

21. is an inorganic fertilizer which is produced from ammonia.
Answer:
Ammonium sulphate [(NH₄)₂SO₄]

22. is an organic fertilizer which is produced from ammonia.
Answer:
Urea [CO(NH₂)₂]

23. HNO₃ ………… is manufactured from ammonia by process.
Answer:
Ostwald.

(b) Sulphuretted Hydrogen (H₂S)

Multiple Choice Questions :

Question 1.
Which of the following oxidation states is applicable to sulphur in H₂S?
(A) -2
(B) +5
(C) +6
(D) +3
Answer:
(A) -2

Question 2.
An example of non-linear molecule is :
(A) H₂S
(B) CO₂
(C) C₂H₂
(D) N₂O
Answer:
(A) H₂S

Question 3.
H₂S on Incomplete combustion forms mainly
(A) HO and S
(B) H and SO₂
(C) H₂S and S
(D) H₂O and SO₂
Answer:
(C) H₂S and S

Question 4.
H₂S is a: ……….
(A) weak dibasic acid
(B) strong dibasic acid
(C) weak monobasic acid
(D) monobasic
Answer:
(C) Weak dibasic acid

Question 5.
When QuestionH₂S is passed through acidified KMnO₄
(A) KHSO₂
(B) K₂SO₄
(C) MnO₂
(D) S
Answer:
(D) S

Question 6.
Which of the following turns lead acetate paper black?
(A) SO₂
(B) SO₃
(C) H₂S
(D) H₂SO₄
Answer:
(C) H₂S

Question 7.
Sulphuretted hydrogen was discovered by:
(A) Shele
(B) Dalton
(C) Lavoisier
(D) Richter
Answer:
(A) Shele

Question 8.
H₂S is :
(A) alkaline
(B) neutral
(C) acidic
(D) amphoteric gas
Answer:
(C) acidic

Question 9.
When a strip of filter paper, soaked in colourless lead acetate solution, is held in the H₂S gas the filter paper becomes
(A) black
(B) blue
(C) pink
(D) red
Answer:
(A) black

Question 10.
Molecular weight of H₂S is:
(A) 32
(B) 34
(C) 36
(D) 38
Answer:
(A) 34

Question 11.
FeS reacts with
(A) dil. H₂SO₄
(B) Conc. H₂SO₄
(C) Conc.HNO₃ to form H₂S
(D) None of these
Answer:
(A) dil. H₂SO₄

Question 12.
H₂S is passed through a added to it. The solution
(A) violet
(B) black
(C) green
(D) red
Answer:
(A) violet

Question 13.
H₂S gas has a smell:
(A) like roften eggs
(B) pungent
G smell like fish none of these
Answer:
(C) smell like fish

Question 14.
H₂S is: ……………
(A) heavier
(B) lighter
(C) slightly heavier than air
(D) none of these
Answer:
(C) smell like fish

Question 15.
Aqueous soution of the gas turns blue litmus to red:
(A) H₂S
(B) NH₃
(C) O₂
(D) H₂
Answer:
(A) H₂S

Question 16.
H₂S can be collected in downward displacement of
(A) hot water
(B) cold water
(C) Hg
(D) none of these
Answer:
(A) hot water

Question 17.
mejas which is identified by its smell:
(A) Nitrogen
(B) Hydrogen
(C) Hydrogen sulphide
(D) None of these
Answer:
(C) Hydrogen sulphide

Question 18.
The gas which has reducing property:
(A) H₂S
(B) CO₂
(C) NO₂
(D) none of these
Answer:
(A) H₂S

Question 19.
H₂S gas is passed through :
(A) P₂O₅
(B) Anhydrous CaCl₂
(C) CaO
(D) none of these
Answer:
(A) P₂O₅

Question 20.
The gas which is absorbed by NaOH :
(A) NH₃
(B) H₂S
(C) O₂
(D) None of these
Answer:
(B) H₂S

Fill in the Blanks:

1. H₂S is a gas having the smell of ……………………
Answer:
rotten egg

2. H₂S is a good ………….. agent.
Answer:
reducing

3. Hydrogen sulphide is a combustible gas but not a supporter of ……………..
Answer:
combustion

4. H₂S reduces acidified yellow solution of ferric chloride to colourless chloride.
Answer:
ferrous

5. Aqueous solution of H₂S is a mild acid, it turns blue ……………. red.
Answer:
litmus

6. H₂S gas has the characteristic unpleasant smell of rotten
Answer:
egg

7. H₂S + H₂SO₄ (cone.) = S + ……………. + 2H₂O
Answer:
SO₂

8. Pb(CH₂COO)₂ + H₂S = ……………….. +2 CH₂COOH
Answer:
PbS

9. H₂S gas turns lead acetate ……………..
Answer:
black

10. H₂S gas is 1.5 times heavier than ……………..
Answer:
air

11. Dilute H₂SO₄ is preferred to dilute HCl acid, for the latter is very ……………..
Answer:
volatile

12. Presence of ………………… gas in the atmosphere in traces tarnishes silver to black silver sulphide.
Answer:
H₂S

13. On passing H₂S gas through zinc salt solution in ………………… medium sulphide of zinc gets precipitated.
Answer:
basic

14. Hydrogen sulphide reduces concentrated sulphuric acid to …………………
Answer:
SO₂

15. Hydrogen sulphide reduces concentrated nitric acid to …………………
Answer:
NO₂

16. Molecular formula of sulphuretted hydrogen is …………………
Answer:
H₂S

17. ………………… is used in order to dry H₂S.
Answer:
P₂O₅

18. H₂S is appreciable soluble in ………………… water, but practically insoluble in not water.
Answer:
cold                                                                                                                     .

19. H₂S is a weak ………………… acid.
Answer:
dibasic

(c) Nitrogen

Multiple choice questions (MCQ) :

Question 1.
The boiling point of liquid nitrogen is
(A) 0°C
(B) – 195.7°C
(C) – 180°C
(D) – 273°C
Answer:
(B) – 195.7°C

Question 2.
Chlorine present as impurity in nitrogen gas is removed by :
(A) Conc. NaOH
(b) Conc. H₂SO₄
(C) P₂O₅
(D) KNO₃
Answer:
(A) Conc. NaOH

Question 3.
The formula of an Inorganic fertilizer containing nitrogen is :
(A) NH₄Cl
(B) (NH₄)₂SO₄
(C) HCN
(D) Pb(NO₃)₂
Answer:
(B) (NH₄)₂SO₄

Question 4.
How is nitrogen gas dried :
(A) Passing through conc.H₂SO₄
(B) By heating the gas in a vessel
(C) P₂O₅
(D) CaCl₄
Answer:
(A) Passing through conc.H₂SO₄

Question 5.
What is the product of combination of nitrogen with calcium carbidc?
(A) calcium nitride
(B) calcium nitrate
(C) calcium nitrite
(D) calcium cyanamide
Answer:
(D) calcium cyanamide

Question 6.
How does nitrogen combine with oxygen :
(A) The two gases combine at a very high temperature under electric spark
(B) The two gases directly combine in presence of sunlight
(C) In absence of sunlight
(D) In presence of iron catalyst.
Answer:
(A) The two gases combine at a very high temperature under electric spark

Question 6.
How does nitrogen combine with oxygen :
(A) The two gases combine at a very high temperature under electric spark
(B) The two gases directly combine in presence of sunlight
(C) In absence of sunlight
(D) In presence of iron catalyst.
Answer:
(A) The two gases combine at a very high temperature under electric spark

Question 7.
What is the necessity of presence of ñttrogen in air:
(A) Nitrogen helps respiration of plants
(B) Nitrogen helps respiration of animals
(C) Nitrogen helps to burn
(D) Nitrogen helps to control burning in air.
Answer:
(D) Nitrogen helps to control burning in air

Question 8.
Why is not nitrogen gas prepared by heating NH₄NO₂ directly :
(A) Rapid explosive dissociation takes place
(B) Nitrogen gas is not obtained
(c) Nitrogen gas combines with oxygen in air
(D) None of these.
Answer:
(A) Rapid explosive dissociation takes place

Question 9.
At ordinary temperature nitrogen is ________
(A) reactive
(B) inert
(C) very-active
(D) None of these.
Answer:
(B) inert

Question 10.
The solubility of nitrogen in water is :_______
(A) low
(B) very low
(C) high
(D) very high
Answer:
(B) very low

Question 11.
Nitrogen is ______
(A) heavier
(B) lighter
(C) slightly heavier
(D) slightly lighter than air
Answer:
(D) slightly lighter

Question 12.
The conversion of Nitrogen gas to liquid nitrogen is :_____________
(A) possible
(B) impossible
(C) easily possible
(D) possible but difficult
Answer:
(D) possible but difficult

Question 13.
Which of the following compounds is used as fertilizer ?
(A) calcium carbide
(B) calcium chloride
(C) magnesium nitride
(D) nitrolim
Answer:
(D) nitrolim

Question 14.
Who discovered nitrogen_______
(A) Daniel Rutherford
(B) Bohr
(C) Dalton
(D) Lavoisier
Answer:
(A) Daniel Rutherford

Question 15.
Nitrogen containing organic fertilizer is :________
(A) nitrolim
(B) ammonium sulphate
(C) ammonium nitrate
(D) urea
Answer:
(D) urea

Question 16.
The requisite chemicals for the preparation of nitrogen :___________
(A) NH₄Cl and Ca(OH)₂
(B) NaNO₂ and NH₄Cl
(C) (NH₄)₂SO₄ and NaOH
(D) NH₄CL and NaOH
Answer:
(B) NaNO₂ and NH₄Cl

Question 17.
Nitrogen gas is collected by :___________
(A) downward displacement of water
(B) downward displacement of air
(C) upward displacement of air
(D) None of these
Answer:
(A) downward displacement of water

Question 18.
Percentage of nitrogen in air by volume is :_______
(A) 20
(B) 30
(C) 78
(D) 88
Answer:
(C) 78

Fill in the blanks

1. Solubility of nitrogen in water is very___________
Answer:
low

2. Nitrogen is a_________ gas._____________
Answer:
colourless

3. Liquid nitrogen is used as ________
Answer:
Condenser

4. 3Mg + N₂ =…………………
Answer:
Mg₃N₂

5. N₂ + ________  = 2NH₃
Answer:
3H₂

6. CaC₂ + N₂ = ________  + C
Answer:
CaCN₂

7. _______ has main role in protein synthesis.
Answer:
Nitrogen

8. The density of nitrogen gas is _____ g/L at NTP.
Answer:
1-25

9. Nitrogen is slightly _______  than air.
Answer:
lighter

10. Solubility of nitrogen in water is about ________  ml/L at NTP.
Answer:
23.5

11. With the help of electric spark nitrogen combines with oxygen at about 3000°C to produce ………..
Answer:
nitric oxide.

12. Nitrolim reacts with steam to form calcium carbonate and__________
Answer:
ammonia.

13. Ammonium nitrite decomposes into nitrogen and __________  due to heating.
Answer:
water

14. Nitrogen gas is passed over concentrated_______ acid where by dry nitrogen is obtained.
Answer:
sulphuric

15. Nitrogen gas is collected by the _________  displacement of water.
Answer:
downward.

16. Nitrogen is relatively_________ element
Answer:
non-reactive

17. Natural source of nitrogen is  _______
Answer:
air

18. The requisite chemicals used for the preparation of nitrogen are sodium nitrite and ______
Answer:
ammonium chloride.

19. Nitrogen was discovered by ________  in 1772.
Answer:
Daniel Rutherford

20. Nitrogen combines with oxygen forming nitric oxide under the influence of electric arc at a temperature of _________
Answer:
3000°C…….

21. Nitrogen combines with hydrogen in presence of electric sparks to produce ________
Answer:
Ammonia

22. When calcium carbide is heated in a current of nitrogen at temperature of ………….. calcium cyanamide and carbon are formed.
Answer:
1100°C

(d) Hydrogen Chloride (Hydrochloric acid), Nitric acid and Sulphuric acid

Multiple choice questions (MCQ) :

Question 1.
How does copper react with sulphuric acid ?
(A) Copper reacts with sulphuric acid in all forms
(B) Copper reacts with hot and concentrated sulphuric acid
(C) Copper reacts with dilute sulphuric acid
(D) None of these
Answer:
(B) copper reacts with hot and concentrated sulphuric acid.

Question 2.
What is passive iron and how it produces ?
(A) Chemically inactive iron is passive iron. It produces as insoluble coating of Fe₃O₄ forms on iron in contact with nitric acid
(B) Iron is inactive with all acids, so iron is passive
(C) It forms Fe₂O₃
(D) None of these
Answer:
(A) Chemically inactive iron is passive iron. It produces as insoluble coating of Fe₃O₄ forms on iron in contact with nitric acid.

Question 3.
In contact process for the production of H₂SO₄ on an industrial scale, the impurities of arsenic are removed by :
(A) Fe₂O₃
(B) Al(OH)₃
(C) Fe(OH))₃
(D) Cr(OH)₃
Answer:
(C) Fe(OH)₃

Question 4.
The conversion of SO₂ by O₂ into SO₃ is :_____
(A) an irreversible reaction
(B) an endothermic reaction
(C) an exothermic reaction
(D) none of these
Answer:
(C) An exothermic reaction

Question 5.
The most favourable condition for the conversion of
\(2 \mathrm{SO}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{SO}_3+98\) KJ/mole is:_____
(A) low temperature and high presure
(B) high temperature and low pressure
(C) high temperature and high pressure
(D) low temperature and low pressure
Answer:
(A) Low temperature and high pressure

Question 6.
In the contact process, sulphur trioxide is dissolved in :
(A) water
(B) dilute sulphuric acid
(C) cone sulphuric acid
(D) none of these
Answer:
(C) Cone., sulphuric acid

Question 7.
Which of the following statements concerning the manufacture of sulphuric acid is false ?
(A) Sulphur is burnt in air to produce SO₂
(B) SO₂ is catalytically oxidised to SO₃
(C) SO₃ is dissolved in water to get 100% sulphuric acid
(D) The lead chamber process for its manufacture is not much in use these days.
Answer:
(C) SO₃ is dissolved in water to get 100% sulphuric acid

Question 8.
Contact process is superior to chamber process for the manufacture of sulphuric acid as it:
(A) provides acid of any concentration
(B) gives acid of low concentration
(C) provides impure acid
(D) Occupies large space
Answer:
(A) provides acid of any concentration

Question 9.
Oleum is :
(A) H₂SO₅
(B) H₂S₂O₇
(C) H₂S₂O₈
(D) H₂SO₃
Answer:
(B) H₂S₂O₇

Question 10.
Oil of vitriol is :
(A) H₂SO₃
(B) H₂SO₄
(C) H₂S₂O₇
(D) H₂S₂O₈
Answer:
(B) H₂SO₄

Question 11.
Which is not correct in case of H₂SO₄ ?
(A) Oxidising agent
(B) Reducing agent
(C) Sulphonating agent
(D) Dehydrating agent
Answer:
(B) Reducing agent

Question 12.
Cone. H₂SO₄ is not :
(A) hygroscopic
(B) dehydrating agent
(C) sulphonating agent
(D) efflorescent
Answer:
(D) efflorescent

Question 13.
Catalyst used In the manufacture of H₂SO₄ by lead chamber process is: _________
(A) V₂O₅
(B) Pt
(C) Ni
(D) oxides of nitrogen
Answer:
(D) oxides of nitrogen

Question 14.
When sugar is treated with cone. H₂SO₄ the sugar becomes black due to;
(A) dehydration
(B) hydration
(C) hydrolysis
(D) decolourisation
Answer:
(D) decolourisation

Question 15.
Electrolysis of…. pure H₂SO₄ produces at anode :
(A) H₂S₂O₅
(B) H₂S₄O₆
(C) H₂S₂O₈
(D) H₂
Answer:
(C) H₂S₂O_s

Question 16.
When charcoal is heated with cone H₂SO₄ 
(A) there is no reaction
(B) CO₂ and SO₂ are evolved
(C) water gas is formed
(D) CO₂ and SO₂ are not evolved
Answer:
(B) CO₂ and SO₂ are evolved

Question 17.
Fuming sulphuric acid is commercially known as: ______
(A) Carro’s acid
(B) Marshall’s acid
(C) Oleum
(D) Sulphurous acid.
Answer:
(C) Oleu

Question 18.
Which of the following gives carbon with cone. H₂SO₄?
(A) Ethyl alcohol
(B) Starch
(C) Formic acid
(D) Oxalic acid
Answer:
(C) Formic acid

Question 19.
King of chemicals is
(A) H₂SO₄
(B) Oxalic acid
(C) HNO₃
(D) NaOH
Answer:
(A) H₂SO₄

Question 20.
Sulphuric acid is a dibasic in nature, hence it forms :
(A) acidic salt
(B) acidic and basic salt
(C) acidic and normal salt
(D) double salt.
Answer:
(C) acidic and normal salt

Question 21.
The main difference between nitric acid and hydrochloric acid lies in their reaction of
(A) nitrates
(B) chlorides
(C) metals
(D) bicarbonates
Answer:
(C) metals

Question 22.
The most volatile compound among the following is :
(A) HF
(B) HCl
(c) HBr
(d) Hl
Answer:
(B) HCl

Question 23.
Cone. HNO₃ oxidises phosphorus to: …………..
(A) H₃PO₄
(B) P₂O₅
(C) H₂PO₃
(D) H₄P₂O₇
Answer:
(A) H₃PO₄

Question 24.
When concentrated HNO₃ is heated, it decomposes to give :
(A) O₂ and N₂
(B) NO
(C) O
(D) NO₂ and O₂
Answer:
(D) NO₂ and O₂

Question 25.
Aqua fortis is :
(A) HNO₃
(B) HNO₂
(C) H₂NO₃
(D) H₂N₂O₂
Answer:
(A) HNO₃

Question 26.
The process used to manufacture nitric acid is :
(A) Solvay process
(B) Ostwald process
(C) Hall process
(D) Haber process
Answer:
(B) Ostwald process

Question 27.
‘Sulphan’ is …………..
(A) 20% oleum
(B) 80% oleum
(C) 100% oleum
(D) 88% oleum
Answer:
(C) 100% oleum

Question 28.
Specific gravity of liquor ammonia is :________
(A) 0.80
(B) 0.44
(C) 0.88
(D) 0.66
Answer:
(C) 0.88

Question 29.
In Haber’s process, the product is :_____
(A) CO(NH₂)₂
(B) NH₃
(C) HNO₃
(D) H₂SO₄
Answer:
(B) NH₃

Question 30.
Which of the following responds in nitroprusside test?
(A) HCl
(B) NH₃
(C) N₂
(D) H₂S
Answer:
(D) H₂S

Question 31.
The optimum temperature for industrial preparation of H₂SO₄ is :___
(A) 650°c
(B) 850°c
(C) 450°c
(D) 250°c
Answer:
(C) 450°c

Question 32.
Raw material for manufacture of HCl by Le Blanck process is :_____
(A) NaCl
(B) Na₂SO₄
(C) NH₄Cl
(D) CaCl₂
Answer:
(A) NaCl

Question 33.
Which of the following gases can be prepared by kipp’s apparatus?
(A) N₂
(B) H₂S
(C) HCl
(D) NH₃
Answer:
(B) H₂S

Question 34.
Choose the wrong statement :
(A) H₂S is a yellow cofoured gas
(B) H₂S is heavier than air
(C) H₂S has rotten egg like smell
(D) The aqueous solution of H₂S is acidic
Answer:
(A) H₂S is a yellow coloured gas

Question 35.
Choose the wrong statement :
(A) Ammonia is a colourless gas
(B) Ammonia is heavier than air
(C) Ammonia is highly soluble in water
(D) Ammonia can be easily liquefied by applying pressure.
Answer:
(B) Ammonia is heavier than air

Question 36.
Which one of the following is not a fertilizer?
(A) ammonia
(B) ammonium phosphate
(C) ammonium nitrate
(D) ammonium sulphate
Answer:
(A) ammonia

Fill in the blanks

1. In contact process, during the preparation of SO₃ from SO₂__________ is used as catalyst.
Answer:
V₂O₅

2. H₂S gas is __________ than air.
Answer:
heavier

3. An aqueous solution of H₂S litmus red.
Answer:
blue

4. In ostwald’s process, for the preparation of nitric acid _______ is used as catalyst.
Answer:
platinum

5. Red hot magnesium reacts with nitrogen to form
Answer:
Mg₃N₂

6. Ammonia gas prepared in the laboratory is dried by__________
Answer:
CaO

7. Ammonia has a strong …………..smell.
Answer:
pungent

8. In the laboratory, H₂S is prepared by the action of dilute H₂SO₄ acid on________
Answer:
FeS

9. Calcium Cyanamide is prepared by reaction between cac₂ and______at elevated temperature.
Answer:
N₂

10. Urea is prepared by reaction between NO₃ and________ at elevated temperature and high pressure.
Answer:
CO₂

State whether the following statement is True or False :

1. Nitrogen is slightly heavier than air.
Answer:
False

2. HCl is produced as a by-product during the manufacture of sodium sulphate by ostwald’s process.
Answer:
False

3. H₂S is a poisonous gas.
Answer:
True

4. In presence of air, H₂S burns with blue flame.
Answer:
True

5. Ammonia is used for production of fertilizers like urea.
Answer:
True

6. Ammonia is prepared by heating a dry ammonium salt with a dry alkali.
Answer:
True

7. P₂O₅ is acidic so it reacts with ammonia.
Answer:
True

8. Ammonia is highly soluble in water.
Answer:
True

9. H₂S is a strong oxidizing agent.
Answer:
False

10. In presence of air, H₂S burns with blue flame.
Answer:
True