The equation of a certain gas can be written as: $\left( \frac{T^7}{P^2} \right)^{1/5} = \text{constant}$. The specific heat at constant volume of this gas is (in $\text{J/mol K}$): (in $R$)

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 $b$?

If $C_{p}$ and $C_{v}$ are molar specific heats of an ideal gas at constant pressure and volume respectively and $\gamma$ is $C_{p} / C_{v}$,then $C_{p} =$ (where $R$ is the universal gas constant).

The graph of specific heat at constant volume $(C_v)$ for a monoatomic gas with respect to temperature $(T)$ is:

The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_{P}$ and $C_{V}$ respectively. If $\gamma = \frac{C_{P}}{C_{V}}$ and $R$ is the universal gas constant,then $C_{V}$ is equal to

$c_P$ and $c_V$ are specific heats at constant pressure and constant volume respectively. It is observed that
$c_P - c_V = a$ for hydrogen gas
$c_P - c_V = b$ for nitrogen gas
The correct relation between $a$ and $b$ is