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

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

$310 \ J$ 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 gas through the same range at constant volume is (in $J$)

$A$ diatomic gas molecule has translational,rotational,and vibrational degrees of freedom. The ratio ${C_P}/{C_V}$ 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 ratio of specific heats $(\gamma)$ of an ideal gas is given by