The degrees of freedom of a triatomic gas is

Molecules of an ideal gas are known to have three translational degrees of freedom and two rotational degrees of freedom. The gas is maintained at a temperature of $T$. The total internal energy,$U$ of a mole of this gas,and the value of $\gamma \left( = \frac{C_P}{C_V} \right)$ are given,respectively,by:

$A$ container holds $1 \, \text{mole}$ of oxygen and $2 \, \text{moles}$ of nitrogen at a temperature of $300 \, K$. What is the ratio of the average rotational kinetic energy of $O_2$ to that of $N_2$?

For a diatomic gas,let $\gamma_1 = \frac{C_p}{C_v}$ for rigid molecules and $\gamma_2 = \frac{C_p}{C_v}$ for diatomic molecules that also have a vibrational mode. Which of the following options is correct? ($C_p$ and $C_v$ are the specific heats of the gas at constant pressure and volume,respectively.)

If the degrees of freedom of a gas molecule is $6$,then the total internal energy of the gas molecule at a temperature of $47^{\circ} C$ (in $eV$) is (Boltzmann constant $= 1.38 \times 10^{-23} \ J \ K^{-1}$)

Degree of freedom of a gas depends on which factors?