When an ideal monoatomic gas is heated at constant pressure,the fraction of heat energy supplied that increases the internal energy of the gas is:

For a diatomic gas,write the value of the ratio of $C_P$ and $C_V$.

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:

$306 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25^{\circ} C$ to $35^{\circ} C$. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is (in $J$)

The ratio of the specific heats $\frac{C_{p}}{C_{v}}=\gamma$,in terms of degrees of freedom $(n)$ is

The molar specific heat of an ideal gas at constant pressure and constant volume is $C_{p}$ and $C_{V}$ respectively. If $R$ is the universal gas constant and the ratio of $C_{p}$ to $C_{V}$ is $\gamma$,then $C_{p}$ is equal to: