For a monoatomic gas,work done at constant pressure is $W$. The heat supplied at constant volume for the same rise in temperature of the gas is

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

What amount of heat (in $J$) must be supplied to $2.0 \times 10^{-2} \; kg$ of nitrogen (at room temperature) to raise its temperature by $45 \; ^{\circ}C$ at constant pressure? (Molecular mass of $N_{2} = 28; R = 8.3 \; J \; mol^{-1} K^{-1}$.)

If $c_p$ and $c_v$ denote the specific heats (per unit mass) of an ideal gas of molecular weight $M$,then which of the following relations holds true,where $R$ is the molar gas constant?

Derive the ratio of $\frac{C_{P}}{C_{V}}$ for a diatomic gas.

$c_P$ 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