For hydrogen gas,$C_P - C_V = a$,and for oxygen gas,$C_P - C_V = b$. The relationship between $a$ and $b$ is given by: (where $C_P$ and $C_V$ are molar specific heats at constant pressure and constant volume,respectively.)

Statement $A: C_P - C_V = R$
Statement $B: \frac{C_P}{C_V} = 1.67$

For an ideal gas,the molar specific heat at constant pressure is $(7/2) R$. Find the ratio of the molar specific heat at constant pressure to the molar specific heat at constant volume.

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 $\frac{\gamma_2}{\gamma_1}$ is

The specific heat of a gas at constant pressure $(C_p)$ is more than that of the same gas at constant volume $(C_v)$ because

$A$ polyatomic gas with $6$ degrees of freedom does $25 \ J$ of work when it is expanded at constant pressure. The heat given to the gas is ..... $J$.