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

$A$ mixture of one mole of monoatomic gas and one mole of a diatomic gas (rigid) is kept at room temperature $\left(27^{\circ} C\right)$. The ratio of the specific heat of these gases at constant volume is:

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

$A$ polyatomic gas with $6$ degrees of freedom does $25 \ J$ of work when it is expanded at constant pressure. The heat given to 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:

$C_v$ and $C_p$ denote the molar specific heat capacities of a gas at constant volume and constant pressure,respectively. Then