An ideal diatomic gas is heated at constant pressure. What is the fraction of total energy applied,which increases the internal energy of the gas?

The molar specific heat of a gas as given from the kinetic theory is $\frac{5}{2} R$. If it is not specified whether it is $C_P$ or $C_V$,one could conclude that the molecules of the gas

Let $\gamma_1$ be the ratio of molar specific heat at constant pressure and molar specific heat at constant volume of a monoatomic gas and $\gamma_2$ be the similar ratio of a diatomic gas. Considering the diatomic gas molecule as a rigid rotator,the ratio $\frac{\gamma_1}{\gamma_2}$ is

According to the law of equipartition of energy, the molar specific heat of a diatomic gas at constant volume, where the molecule has one additional vibrational mode, is:

One mole of an ideal gas requires $207 \, J$ of heat to raise the temperature by $10 \, K$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10 \, K$,the heat required is ...... $J$ (Given the gas constant $R = 8.3 \, J/mol \cdot K$)

If the ratio of the universal gas constant $(R)$ and the specific heat capacity at constant volume $(C_v)$ of a gas is given by $0.67$,then the gas is