For an ideal gas,$R = \frac{2}{3} C_v$. This suggests that the gas consists of molecules which are: $[R = \text{universal gas constant}]$

The total number of degrees of freedom in $1 \ cm^3$ of $H_2$ gas at $NTP$ is ....

$A$ diatomic gas consisting of rigid molecules is at a temperature of $87^{\circ} C$. If the moment of inertia of the rotating diatomic rigid molecule is $2.76 \times 10^{-46} kg \cdot m^2$,then the rms angular speed of the molecule is (Boltzmann constant $= 1.38 \times 10^{-23} J \cdot K^{-1}$)

$A$ polyatomic gas with $n$ degrees of freedom has a mean energy per molecule given by (where $k$ is Boltzmann's constant and $T$ is temperature).

The kinetic energy per gram mole for a diatomic gas at room temperature is:

The ratio of the kinetic energy of a diatomic gas molecule at a high temperature to that at $NTP$ is: