On giving an equal amount of heat at constant volume to $1 \, mol$ of a monoatomic and a diatomic gas,the rise in temperature $(\Delta T)$ is more for:

The molar specific heats of an ideal gas at constant pressure and constant 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:

If the ratio of specific heat of a gas at constant pressure to that at constant volume is $\gamma$,the change in internal energy of a mass of gas,when the volume changes from $V$ to $2V$ at constant pressure $p$,is

The amount of heat required to raise the temperature of $2$ moles of helium gas from $0^{\circ}C$ to $100^{\circ}C$ at constant volume and constant pressure,respectively,is:

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)

The specific heat of helium at constant volume is $12.6 \,J \,mol^{-1} \,K^{-1}$. The specific heat of helium at constant pressure in $J \,mol^{-1} \,K^{-1}$ is approximately (assume, the universal gas constant, $R=8.314 \,J \,mol^{-1} \,K^{-1}$)