$310 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25 \ ^oC$ to $35 \ ^oC$. The amount of heat required to raise the temperature of the gas through the same range at constant volume is $.... \ J$.

If a gas has $n$ degrees of freedom, then the ratio of $\frac{C_p}{C_V}$ is

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:

What amount of heat (in $J$) must be supplied to $2.0 \times 10^{-2} \; kg$ of nitrogen (at room temperature) to raise its temperature by $45 \; ^{\circ}C$ at constant pressure? (Molecular mass of $N_{2} = 28; R = 8.3 \; J \; mol^{-1} K^{-1}$.)

The quantity of heat required to raise the temperature of one mole of a monoatomic gas by one degree Kelvin at constant volume is

Let $\gamma_1$ be the ratio of molar specific heat at constant pressure and molar specific heat at constant volume of a monoatomic gas and $\gamma_2$ be the similar ratio of a diatomic gas. Considering the diatomic gas molecule as a rigid rotator,the ratio $\frac{\gamma_2}{\gamma_1}$ is