According to the law of equipartition of energy, the molar specific heat of a diatomic gas at constant volume, where the molecule has one additional vibrational mode, is:

$40 \, \text{calories}$ of heat is needed to raise the temperature of $1 \, \text{mole}$ of an ideal monoatomic gas from $20^{\circ}C$ to $30^{\circ}C$ at a constant pressure. The amount of heat required to raise its temperature over the same interval at a constant volume $(R = 2 \, \text{cal} \, \text{mol}^{-1} \text{K}^{-1})$ is ..... $\text{calories}$.

For a monoatomic ideal gas,the universal gas constant $R$ is $n$ times the molar heat capacity at constant pressure $C_P$. Here,$n$ is ......

If $\gamma$ is the ratio of specific heats and $R$ is the universal gas constant,then the molar specific heat at constant volume $C_{V}$ is given by

Select the incorrect relation. (Where symbols have their usual meanings)

If a gas has $n$ degrees of freedom,the ratio of specific heats of the gas is: