List of top Physics Questions on kinetic theory asked in KEAM

The product of the pressure P and volume V of an ideal gas in a container is related to the translational part of the internal energy, E as
The mean free path of a molecule is inversely proportional to
The temperature at which the r.m.s. velocity of oxygen molecule is equal to that of hydrogen molecule at 20 K is
Mean free path is inversely proportional to (n = number density, d = diameter of particle)
The ratio between the root mean square velocities of \( O_2 \) and \( O_3 \) molecules at the same temperature is:
Two gases under the same thermal conditions have the same number of molecules per unit volume. If the respective molecular diameters of the gases are in the ratio 1 : 3, then their respective mean free paths are in the ratio:
The rms speed of a gas having diatomic molecules at temperature T (in Kelvin) is 200 m/s. If the temperature is increased to 4T and the molecules dissociate into monoatomic atoms,the rms speed will become:
The average kinetic energy of a monoatomic gas molecule kept at temperature \(27^\circ\)C is \((\text{Boltzmann constant}=1.3\times 10^{-23}\ \text{J K}^{-1})\)
If a monoatomic gas is compressed adiabatically to \((1/27)^{\text{th\) of its initial volume, then its pressure becomes}
The values of \(C_V\) and \(C_P\) for a diatomic gas are respectively \((R=\) gas constant\()\)
Some smoke is trapped in a small glass container and is viewed through a microscope. A number of very small smoke particles are seen in continuous random motion as a result of bombardment by air molecules. If the mass of the smoke particle is about \(10^{12}\) times higher than that of an air molecule, the average speed of a smoke particle is:
Consider a system of gas of a diatomic molecule in which the speed of sound at $0^\circ\text{C}$ is 1260 $\text{ms}^{-1}$. Then, the molecular weight of the gas is (Given the gas constant $R=8.314\,\text{J mol}^{-1}\text{K}^{-1}$)
Five moles of an ideal monatomic gas with an initial temperature of $150^\circ\text{C}$ expand and in the process absorb 1500 J of heat and does 2500 J of work. The final temperature of the gas in $^\circ\text{C}$ is (Ideal gas constant $R=8.314\,\text{J K}^{-1}\text{mol}^{-1}$)
The temperature of an ideal gas is increased from 100 K to 400 K. If the rms speed of the gas molecule is $v$ at 100 K then at 400 K it becomes
For an ideal gas, the specific heat at constant pressure $C_p$ is greater than the specific heat at constant volume $C_v$. This is because
Match the following: I) Isothermal process
II) Isobaric process
III) Isochoric process
IV) Adiabatic process
If the average kinetic energy of a molecule of a hydrogen gas at 300 K is $E$, the average kinetic energy of a molecule of a nitrogen gas at the same temperature is
The difference between the specific heats of a gas is \( 4150 \, \text{J kg}^{-1}\text{K}^{-1} \). If the ratio of specific heats is \( 1.4 \), then the specific heat at constant volume of the gas (in \( \text{J kg}^{-1}\text{K}^{-1} \)) is
The Zeroth law of thermodynamics leads to the concept of
For a monatomic gas, the molar specific heat at constant pressure divided by the molar gas constant \(R\) is equal to
Total number of degrees of freedom of a rigid diatomic molecule is
A molecule of a gas has six degrees of freedom. Then the molar specific heat of the gas at constant volume is
If \(m\) represents the mass of each molecule of a gas and \(T\), its absolute temperature, then the root mean square velocity of the gaseous molecule is proportional to
A molecule of a gas has six degrees of freedom. Then the molar specific heat of the gas at constant volume is
Total number of degrees of freedom of a rigid diatomic molecule is