The molar specific heat at constant pressure of an ideal gas is $\frac{7}{2} R$. The gas is made up of molecules which are ( $R$ is the universal gas constant)

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 $N_{2} = 28; R = 8.3 \; J \; mol^{-1} K^{-1}$.)

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

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?

The ratio of the adiabatic to isothermal elasticities of a triatomic (non-linear) gas is

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).