The average degree of freedom per molecule of a gas is $6$. The gas performs $25 \ J$ work,while expanding at constant pressure. The heat absorbed by the gas is .... $J$

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:

If $C_p$ and $C_v$ are molar specific heats of an ideal gas at constant pressure and volume respectively,if $\gamma$ is the ratio of the two specific heats and $R$ is the universal gas constant,then $C_p$ is equal to

To raise the temperature of a certain mass of gas by $50^{\circ} C$ at a constant pressure,$160$ calories of heat is required. When the same mass of gas is cooled by $100^{\circ} C$ at constant volume,$240$ calories of heat is released. How many degrees of freedom does each molecule of this gas have (assume gas to be ideal)?

When an ideal triatomic non-linear gas is heated at constant pressure,the fraction of the heat energy supplied which increases the internal energy of the gas is

If $C_p$ and $C_v$ denote the specific heat of nitrogen at constant pressure and constant volume respectively,then