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)

When a monoatomic gas is heated at constant pressure,what fraction of the heat energy supplied is used to increase the internal energy?

What will be the molar specific heat at constant volume of an ideal gas consisting of rigid diatomic molecules?

$A$ polyatomic gas has $f$ vibrational degrees of freedom, then the ratio of the specific heat at constant pressure to that at constant volume will be

The amount of heat that must be supplied to $35 \ g$ of oxygen at room temperature to raise its temperature by $80^{\circ} C$ at constant volume is (molecular mass of oxygen is $32$ and $R = 8.3 \ J \ mol^{-1} \ K^{-1}$) (in $kJ$)

What is the value of $\frac{R}{C_P}$ for a diatomic gas?