Kinetic Theory of Gases HC Verma Solutions of Que for Short Ans Ch-24
Kinetic Theory of Gases HC Verma Solutions of Que for Short Ans Vol-2 Ch-24 Concept of Physics. Step by Step Solution of Questions for short answer of Ch-24 Kinetic Theory of Gases HC Verma Question for Short Answer . Visit official Website CISCE for detail information about ISC Board Class-12 Physics.
Kinetic Theory of Gases HC Verma Solutions Que for Short Ans Vol-2 Ch-24 Concept of Physics
|Board||ISC and other board|
|Publications||Bharti Bhawan Publishers|
|Ch-24||Kinetic Theory of Gases|
|writer||H C Verma|
|Book Name||Concept of Physics|
|Topics||Solutions of Question for short answer|
-: Select Topics :-
Ques for Short Ans
Kinetic Theory of Gases Que for short ans
HC Verma Solutions of Ch-24 Vol-2 Concept of Physics for Class-12
Question 1 :-
When we place a gas cylinder on a van and the van moves, does the kinetic energy of the molecules increase? Does the temperature increase?
Answer 1 :-
No, kinetic energy of the molecules does not increase. This is because velocity of the molecules does not increase with respect to the walls of the gas cylinder, when the cylinder is kept in a vehicle moving with a uniform motion. However, if the vehicle is accelerated or decelerated, then there will be a change in the gas’s kinetic energy and there will be a rise in the temperature.
Question 2 :-
While gas from a cooking gas cylinder is used, the pressure does not fall appreciably till the last few minutes. Why?
Answer 2 :-
When the gas oven is switched on, the vapour pressure inside the cylinder decreases. To compensate this fall in pressure, more liquid undergoes phase transition (vaporisation) to build up the earlier pressure. In this way, more and more gas evaporates from the liquified state at constant pressure.
Question 3 :-
Do you expect the gas in a cooking gas cylinder to obey the ideal gas equation?
Answer 3 :-
No, the gas won’t obey ideal gas equation due to the following reasons:
1. In a cooking gas cylinder, the gas is kept at high pressure and at room temperature. Real gases behave ideally only at low pressure and high temperature.
2. Cooking gas is kept in liquid state inside the cylinder because liquid state does not obey the ideal gas equation.
Question 4 :-
Can we define the temperature of (a) vacuum, (b) a single molecule?
Answer 4 :-
(a) Temperature is defined as the average kinetic energy of he particles. In a vacuum, devoid of any electromagnetic fields and molecules or entities, the temperature cannot be defined as there are no molecules or atoms or entities.
(b) No, we cannot define temperature of a single molecule. Since temperature is defined as the average kinetic energy of the particles, it is defined only statistically for a large collection of molecules.
Question 5 :-
Comment on the following statement: the temperature of all the molecules in a sample of a gas is the same.
Answer 5 :-
Yes, at equilibrium all the molecules in a sample of gas have the same temperature. This is because temperature is defined as the average kinetic energy for all the molecules in a system. Since all the molecules have the same average, temperature will be the same for all the molecules.
Question 6 :-
Consider a gas of neutrons. Do you expect it to behave much better as an ideal gas as compared to hydrogen gas at the same pressure and temperature?
Answer 6 :-
1. As per the Kinetic theory, neutrons do not interact with each other. Molecules of an ideal gas should also not interact with each other. On the other hand, hydrogen molecules interact with each other owing to the presence of charges in them.
2. Neutrons are smaller than hydrogen. This fulfils another kinetic theory postulate that gas molecules should be points and should have negligible size.
Question 7 :-
A gas is kept in a rigid cubical container. If a load of 10 kg is put on the top of the container, does the pressure increase?
Answer 7 :-
No, the pressure on gas won’t increase because of this. The pressure will not be transferred to the gas, but to the container and to the ground.
Question 8 :-
If it were possible for a gas in a container to reach the temperature 0 K, its pressure would be zero. Would the molecules not collide with the walls? Would they not transfer momentum to the walls?
Answer 8 :-
Since the pressure would be zero, the molecules would not collide with the walls and would not transfer momentum to the walls. This is because pressure of a gas is formed due to the molecule’s collision with the walls of the container.
It is said that the assumptions of kinetic theory are good for gases having low densities. Suppose a container is so evacuated that only one molecule is left in it. Which of the assumptions of kinetic theory will not be valid for such a situation? Can we assign a temperature to this gas?
Answer 9 :-
Two postulates of kinetic theory will not be valid in this case.
These are given below:
1. All gases are made up of molecules moving randomly in all directions
2. When a gas is left for a sufficient time, it comes to a steady state. The density and the distribution of molecules with different velocities are independent of position, direction and time.
Question 10 :-
A gas is kept in an enclosure. The pressure of the gas is reduced by pumping out some gas. Will the temperature of the gas decrease by Charles’s low?
Answer 10 :-
If the gas is ideal, there will be no temperature change. Moreover, Charles’s law relates volume with temperature not pressure with temperature, so the cause behind the phenomena cannot be explained by Charles’s law.
Question 11 :-
Explain why cooking is faster in a pressure cooker.
Answer 11 :-
In a pressure cooker, the vapour pressure over the water surface is more than the atmospheric pressure. This means boiling point of the water will be higher in the pressure cooker than in the open. This will let the cereals and food to be cooked in higher temperature than at 1000C,. Thus, cooking process gets faster.
Question 12 :-
If the molecules were not allowed to collide among themselves, would you expect more evaporation or less evaporation?
Answer 12 :-
If the molecules are not allowed to collide with each other, they will have long mean free paths and hence, evaporation will be faster. In vacuum, the external pressure will be very low. So, the liquid will boil and evaporate at very low temperature.
Question 13 :-
Is it possible to boil water at room temperature, say 30°C? If we touch a flask containing water boiling at this temperature, will it be hot?
Answer 13 :-
Yes, it is possible to boil water at 300C by reducing the external pressure. A liquid boils when its vapour pressure equals external pressure. By lowering the external pressure, it is possible to boil the liquid at low temperatures.
No, the flask containing water boiling at 300C will not be hot.
Question 14 :-
When you come out of a river after a dip, you feel cold. Explain.
Answer 14 :-
After a dip in the river, the water that sticks to our body gets evaporated. We know that evaporation takes place faster for higher temperatures. Thus, the molecules that have the highest kinetic energy leave faster and that is how heat is given away from our body.
As a result of it, temperature of our body falls down due to loss of heat and we feel cold.
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