The mean kinetic energy per degree of freedom of gas molecules is:

The internal energy $(U)$,pressure $(P)$,and volume $(V)$ of an ideal gas are related as $U = 3PV + 4$. The gas is:

Internal energy of $n_1$ moles of hydrogen at temperature $T$ is equal to the internal energy of $n_2$ moles of helium at temperature $2T$. Then the ratio $n_1:n_2$ is: [Degree of freedom of $He = 3$,Degree of freedom of $H_2 = 5$]

Consider a gas of triatomic molecules. The molecules are assumed to be triangular and made of massless rigid rods whose vertices are occupied by atoms. The internal energy of a mole of the gas at temperature $T$ is $......RT$.

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

The internal energy of one mole of a rigid diatomic gas at absolute temperature $T$ is