Kinetic TheoryNEET Physics · Class 11 · NCERT Chapter 12

The RMS speed of gas molecules of mass $m$ at temperature $T$ is given by:

The average translational kinetic energy of a gas molecule at temperature $T$ is:

The ratio of RMS speeds of $H_2$ and $O_2$ at the same temperature is:

The pressure of an ideal gas in terms of density $\rho$ and v_rms is:

If the temperature of an ideal gas is doubled, the RMS speed becomes:

The total internal energy of one mole of a diatomic gas (f = 5) at temperature $T$ is:

The value of $\gamma =C_P/C_V$ for a polyatomic gas (f = 6) is:

The ratio $v_p:v_{\text{avg}}:v_{\text{rms}}$ for a Maxwell distribution is:

At what temperature is the average translational kinetic energy of an ideal gas molecule $1.0\times 10^{-20}\text{J}$? (Use $k_B=1.38\times 10^{-23}\text{J/K}$.)

At STP, the volume occupied by one mole of any ideal gas is approximately:

A gas in a closed container is heated. Its pressure depends on:

According to the law of equipartition of energy, the energy associated with each quadratic degree of freedom of a molecule at temperature $T$ is:

For a monoatomic gas, $C_V$ in terms of $R$ is:

At the same temperature, the RMS speed of helium ($M=4$) is what factor times the RMS speed of oxygen ($M=32$)?

Two ideal gases are at the same temperature. The molecules of the two gases will have:

The mean free path of a gas molecule depends on:

A gas at $300\text{K}$ and $1\text{atm}$ is heated to $600\text{K}$ at constant volume. The new pressure is:

If the volume of a gas is reduced to half at constant temperature, the pressure becomes:

In a Maxwell-Boltzmann distribution at fixed T, the most probable speed:

The molar specific heat at constant volume of a diatomic gas is:

The temperature at which the average translational kinetic energy of a gas molecule is twice its value at 300 K is:

The internal energy of two moles of a monoatomic ideal gas at $300\text{K}$ is:

If pressure is halved at constant T, the mean free path:

A gas in a container is heated such that its v_rms doubles. The pressure (at constant volume and same number of molecules):

For a gas with degrees of freedom $f$, the value of $\gamma$ is:

Two gases at the same T have molar masses $M_1$ and $M_2$. The ratio of their RMS speeds is:

The Boltzmann constant $k_B$ is related to the universal gas constant $R$ by:

Increasing the temperature of a gas does what to the Maxwell-Boltzmann curve?

A gas obeying the ideal gas law has $PV=N{k}_{B}T$. The number of molecules in 22.4 L at STP is:

If the rms speed of an ideal gas is increased by a factor of 3, then its pressure (at constant volume and density) increases by a factor of:

The energy associated with vibrational mode of a diatomic molecule (one vibrational mode = 2 quadratic dof) at temperature T is:

At STP, the mean free path of an air molecule (d ≈ 0.4 nm) is roughly: