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?

Let $\gamma_1$ be the ratio of molar specific heat at constant pressure and molar specific heat at constant volume of a mono-atomic gas and $\gamma_2$ be the similar ratio of a diatomic gas. Considering the diatomic gas molecule as a rigid rotator, the ratio $\gamma_1/\gamma_2$ is

The ratio of specific heats $\left(\frac{C_{P}}{C_{V}}\right)$ in terms of degree of freedom $(f)$ is given by

For hydrogen gas $(H_2)$,$C_P - C_V = a$,and for oxygen gas $(O_2)$,$C_P - C_V = b$. What is the relationship between $a$ and $b$?

An ideal mono-atomic gas is taken through a process such that $dQ = 3dU$. The molar heat capacity for this process is: (in $R$)

The ratio of the molar specific heat capacities of monatomic and diatomic gases at constant pressure is (in $: 7$)