Here we will provide you the 50+ MCQ Questions of Kinetic Theory for NEET-UG. Kinetic Theory is the chapter 13 in Class XI or Class 11 Physics NCERT Unit Kinetic Theory NEET (conducted by NTA) is based on the NCERT book.
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Kinetic Theory NEET MCQ
Which of the following gases will have the highest average velocity at the same temperature and pressure?
A) O2
B) N2
C) CO2
D) He
The pressure exerted by a gas is proportional to its
A) mass
B) temperature
C) volume
D) number of molecules
The root mean square speed of gas molecules is proportional to the
A) temperature
B) pressure
C) density
D) none of the above
The ratio of the root mean square speed of two gases at the same temperature is given by
A) √(M1/M2)
B) √(M2/M1)
C) (M1/M2)
D) (M2/M1)
The temperature of a gas is doubled at constant pressure. What will be the change in the average kinetic energy of its molecules?
A) It will become four times
B) It will become two times
C) It will remain the same
D) It cannot be determined
The ratio of specific heats of a diatomic gas is
A) 1.4
B) 1.67
C) 1.33
D) 2.5
Which of the following is not a postulate of Kinetic Theory of Gases?
A) The volume occupied by the gas molecules is negligible compared to the volume of the container.
B) The gas molecules are in constant random motion and collide with each other and the walls of the container.
C) The collision between gas molecules is perfectly elastic.
D) The gas molecules interact with each other through intermolecular forces.
In an adiabatic process, the temperature of an ideal gas
A) remains constant
B) increases
C) decreases
D) first increases and then decreases
In an isothermal process, the change in internal energy of an ideal gas is
A) positive
B) negative
C) zero
D) unpredictable
What is the mean free path of gas molecules?
A) the average distance a molecule travels between two successive collisions
B) the average time between two successive collisions of a molecule
C) the average energy of a molecule
D) the average force experienced by a molecule
Which of the following statements is true about the internal energy of an ideal gas?
a) It depends on the temperature and pressure of the gas
b) It is solely a function of the temperature of the gas
c) It is solely a function of the pressure of the gas
d) It is a function of the temperature, pressure, and volume of the gas
Which of the following statements is false about an ideal gas?
a) The molecules of an ideal gas have no volume
b) The molecules of an ideal gas do not exert any forces on each other
c) The pressure of an ideal gas is solely a function of the temperature of the gas
d) The volume of an ideal gas is solely a function of the pressure of the gas
At a constant temperature, the root-mean-square speed of the molecules of a gas is proportional to:
a) The pressure of the gas
b) The density of the gas
c) The square root of the mass of the gas molecules
d) The volume of the gas
The pressure of an ideal gas is related to the kinetic energy of its molecules as:
a) Pressure = (2/3) x (kinetic energy per unit volume)
b) Pressure = (1/3) x (kinetic energy per unit volume)
c) Pressure = (3/2) x (kinetic energy per unit volume)
d) Pressure = (1/2) x (kinetic energy per unit volume)
The average kinetic energy of the molecules of an ideal gas is directly proportional to:
a) The temperature of the gas
b) The pressure of the gas
c) The volume of the gas
d) The number of molecules of the gas
Which of the following statements is true about the specific heat capacity of an ideal gas at constant volume?
a) It is equal to zero
b) It is equal to infinity
c) It is directly proportional to the number of molecules of the gas
d) It is solely a function of the temperature of the gas
The mean free path of the molecules of a gas is:
a) The average distance traveled by a molecule between two collisions
b) The average time elapsed between two collisions of a molecule
c) The average distance between two molecules in the gas
d) The average time elapsed between two consecutive collisions of a molecule with the walls of the container
At a given temperature, the rms speed of the molecules of hydrogen gas is v1, and that of the molecules of nitrogen gas is v2. Which of the following is true?
a) v1 = v2
b) v1 > v2
c) v1 < v2
d) It is impossible to compare the two rms speeds without additional information.
Which of the following statements is false about an ideal gas?
a) The molecules of an ideal gas have zero volume
b) The molecules of an ideal gas have elastic collisions
c) The molecules of an ideal gas obey the laws of Newtonian mechanics
d) The molecules of an ideal gas experience intermolecular forces.
The mean free path of the molecules of an ideal gas is inversely proportional to:
a) Pressure of the gas
b) Temperature of the gas
c) Density of the gas
d) All of the above
An ideal gas undergoes an isothermal process. Which of the following statements is false?
a) The internal energy of the gas remains constant
b) The pressure of the gas decreases if the volume is increased
c) The volume of the gas increases if the pressure is decreased
d) The work done by the gas is zero.
The root mean square velocity of the molecules of an ideal gas is given by:
a) (3RT/M)^1/2
b) (2RT/M)^1/2
c) (RT/M)^1/2
d) (4RT/M)^1/2
The velocity distribution of the molecules of an ideal gas is given by:
a) Gaussian distribution
b) Poisson distribution
c) Binomial distribution
d) Uniform distribution
The collision frequency of the molecules of an ideal gas is proportional to:
a) The number of molecules in the gas
b) The average speed of the molecules
c) The mean free path of the molecules
d) All of the above
Which of the following statements is true about the specific heat of an ideal gas at constant pressure and constant volume?
a) The specific heat at constant pressure is greater than the specific heat at constant volume
b) The specific heat at constant pressure is equal to the specific heat at constant volume
c) The specific heat at constant pressure is less than the specific heat at constant volume
d) The specific heat at constant pressure and constant volume is zero.
Which of the following is NOT a postulate of the kinetic theory of gases?
a) Gases are made up of small particles
b) The particles in a gas are in constant random motion
c) The particles in a gas are attracted to each other
d) The collisions between gas particles are perfectly elastic
Which of the following is true about the average kinetic energy of gas molecules?
a) It is directly proportional to the temperature of the gas
b) It is inversely proportional to the pressure of the gas
c) It is independent of the mass of the gas molecules
d) It is directly proportional to the volume of the gas
Which of the following statements about the root-mean-square speed of gas molecules is true?
a) It is proportional to the pressure of the gas
b) It is inversely proportional to the temperature of the gas
c) It is proportional to the square root of the mass of the gas molecules
d) It is independent of the number of gas molecules present
A container is filled with an ideal gas at a pressure of 2 atm and a temperature of 300 K. If the pressure is increased to 4 atm while the temperature is held constant, what is the new root-mean-square speed of the gas molecules?
a) Remains unchanged
b) Doubles
c) Increases by a factor of √2
d) Increases by a factor of 2
Which of the following statements is true about the distribution of molecular speeds in a gas at a given temperature?
a) All molecules have the same speed
b) Most molecules have the same speed, with a few having much higher speeds
c) The distribution is uniform across all speeds
d) The distribution is logarithmic, with most molecules having low speeds and a few having high speeds
The pressure of a gas is doubled at constant temperature. By what factor does the root-mean-square speed of the gas molecules change?
a) Remains unchanged
b) Doubles
c) Increases by a factor of √2
d) Increases by a factor of 2
We hope there NEET MCQ of Class 11 Kinetic Theory will help you to score an excellent rank in NEET-UG. If you have any queries feel free to write in the comments section. We at Study Rate are always ready to serve our students
