## NEET Important Questions for Kinetic Theory of Gases

The Kinetic Theory of Gases was developed by James Clark Maxwell, Rudolph and Claussius to explain the behaviour of gases. It helps in understanding the physical properties of the gases at the molecular level. The Kinetic Theory of Gases is based on the following assumptions.

## Assumptions of Kinetic Theory of Gases

• Gas is a collection of numerous atoms or molecules.
• The space occupied by the molecules of gas in a container is very negligible. Particles are generally far apart such that their inter-particle distance is much larger than the particle size and there is large free unoccupied space in the container.
• Particles are independent. They do not have any (attractive or repulsive) interactions among them.
• The particles are always in constant motion. Because of lack of interactions and the free space available, the particles randomly move in all directions but in a straight line. These molecules always have linear motion.
• Owing to motion, gas particles occupy the total volume of the container whether it is small or big and hence the volume of the container to be treated as the volume of the gases.
• Mean free path is the average distance a particle travels to meet another particle.
• Since the particles are always in motion, they have average kinetic energy proportional to the temperature of the gas
• The free movement of molecules results in collision which is perfectly elastic. Collisions do not change the energy or momentum of the particle.
• Collision of the particles on the walls of the container exerts a force on the walls of the container. Force per unit area is the pressure. The pressure of the gas is thus proportional to the number of particles colliding (frequency of collisions) in unit time per unit area on the wall of the container. Sure! Here are some important questions on the topic of “Kinetic Theory of Gases” for NEET preparation:

1. The pressure exerted by an ideal gas in a container is due to:
a) The attractive forces between gas molecules.
b) The repulsive forces between gas molecules.
c) The random motion of gas molecules colliding with the walls of the container.
d) The gravitational force acting on gas molecules.

2. The average kinetic energy of gas molecules is directly proportional to:
a) The square of the temperature in Kelvin.
b) The square of the volume of the container.
c) The square root of the molar mass of the gas.
d) The square of the pressure of the gas.

3. The root-mean-square speed of gas molecules is related to the average speed (u) as:
a) u = (3/2) times the root-mean-square speed.
b) u = (2/3) times the root-mean-square speed.
c) u = 2 times the root-mean-square speed.
d) u = (1/2) times the root-mean-square speed.

4. The ratio of specific heats (γ) for a diatomic ideal gas is:
a) γ = 5/3
b) γ = 7/5
c) γ = 3/2
d) γ = 4/3

5. A gas undergoes an adiabatic expansion. What happens to the temperature and pressure of the gas?
a) Temperature increases, pressure decreases.
b) Temperature decreases, pressure increases.
c) Temperature remains constant, pressure decreases.
d) Temperature decreases, pressure remains constant.

6. The average kinetic energy of a gas is directly proportional to:
a) The pressure of the gas.
b) The volume of the gas.
c) The square root of the absolute temperature of the gas.
d) The number of gas molecules.

7. Which of the following statements about the ideal gas is true?
a) An ideal gas obeys the van der Waals equation.
b) The molecules of an ideal gas have no volume.
c) The molecules of an ideal gas experience attractive forces.
d) An ideal gas can liquefy at any temperature.

8. The pressure exerted by an ideal gas is increased by:
a) Increasing the temperature while keeping the volume constant.
b) Decreasing the number of gas molecules while keeping the temperature constant.
c) Decreasing the volume while keeping the temperature constant.
d) Increasing the volume while keeping the temperature constant.

9. Avogadro’s law states that equal volumes of different gases at the same temperature and pressure contain:
a) The same number of molecules.
b) The same number of atoms.
c) The same mass.
d) The same density.

10. According to the kinetic theory of gases, the absolute temperature of a gas is a measure of:
a) The average kinetic energy of the gas molecules.
b) The mass of the gas molecules.
c) The volume of the gas.
d) The pressure of the gas.

1. c) The random motion of gas molecules colliding with the walls of the container.
2. a) The square of the temperature in Kelvin.
3. d) u = (1/2) times the root-mean-square speed.
4. a) γ = 5/3
5. b) Temperature decreases, pressure increases.
6. c) The square root of the absolute temperature of the gas.
7. b) The molecules of an ideal gas have no volume.
8. d) Increasing the volume while keeping the temperature constant.
9. a) The same number of molecules.
10. a) The average kinetic energy of the gas molecules.

Note: These questions cover essential concepts in the Kinetic Theory of Gases. Please ensure you understand the underlying principles and theories while preparing for the NEET exam. Good luck with your preparation!

## JEE Important Questions for Kinetic Theory of Gases

Certainly! Here are some important questions on the topic of “Kinetic Theory of Gases” for JEE (Joint Entrance Examination) preparation:

1. The root-mean-square speed of gas molecules is given by the expression:
a) √(3RT/M)
b) √(2RT/M)
c) √(RT/2M)
d) √(3RT/2M)

2. An ideal gas is contained in a closed container. If the container’s volume is doubled while keeping the temperature constant, how does the pressure change?
a) Pressure doubles.
b) Pressure is halved.
c) Pressure becomes four times.
d) Pressure remains constant.

3. The average kinetic energy of an ideal gas is directly proportional to:
a) The temperature of the gas.
b) The square of the temperature of the gas.
c) The square root of the temperature of the gas.
d) The volume of the gas.

4. A gas undergoes an adiabatic compression. What happens to its temperature and pressure?
a) Temperature increases, pressure decreases.
b) Temperature decreases, pressure increases.
c) Temperature increases, pressure increases.
d) Temperature decreases, pressure decreases.

5. The ratio of specific heats (γ) for a monatomic ideal gas is:
a) γ = 1.66
b) γ = 1.33
c) γ = 1.25
d) γ = 1.50

6. The pressure of an ideal gas is increased by:
a) Increasing the temperature while keeping the volume constant.
b) Decreasing the number of gas molecules while keeping the temperature constant.
c) Increasing the volume while keeping the temperature constant.
d) Increasing the temperature while decreasing the volume to half.

7. According to the kinetic theory of gases, which of the following statements is true about the pressure exerted by a gas?
a) Pressure is due to the gravitational force acting on gas molecules.
b) Pressure is due to the attractive forces between gas molecules.
c) Pressure is due to the elastic collisions of gas molecules with the walls of the container.
d) Pressure is due to the expansion of gas molecules in the container.

8. An ideal gas is initially at a temperature T1 and volume V1. If the volume is reduced to V2, what will be the final temperature if the process is adiabatic?
a) T1
b) 2T1
c) T1/2
d) T1^2

9. Avogadro’s law states that equal volumes of different gases at the same temperature and pressure contain:
a) The same number of molecules.
b) The same number of atoms.
c) The same mass.
d) The same density.

10. The average kinetic energy of gas molecules in an ideal gas is directly proportional to:
a) The square of the mass of gas molecules.
b) The square of the root-mean-square speed of gas molecules.
c) The absolute temperature of the gas.
d) The pressure of the gas.

1. a) √(3RT/M)
2. b) Pressure is halved.
3. b) The square of the temperature of the gas.
4. b) Temperature decreases, pressure increases.
5. d) γ = 1.50
6. c) Increasing the volume while keeping the temperature constant.
7. c) Pressure is due to the elastic collisions of gas molecules with the walls of the container.
8. c) T1/2
9. a) The same number of molecules.
10. c) The absolute temperature of the gas.

Note: These questions cover important concepts in the Kinetic Theory of Gases. Please ensure you understand the underlying principles and theories while preparing for the JEE exam. Good luck with your preparation!

NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases NEET Important Questions for Kinetic Theory of Gases

JEE Important Questions for Kinetic Theory of Gases

JEE Important Questions for Kinetic Theory of Gases

JEE Important Questions for Kinetic Theory of Gases

JEE Important Questions for Kinetic Theory of Gases

JEE Important Questions for Kinetic Theory of Gases

JEE Important Questions for Kinetic Theory of Gases

JEE Important Questions for Kinetic Theory of Gases