Molar specific heat at constant pressure $C_p$ is related to internal energy $U$ and absolute temperature $T$ as $C_p$ is equal to

For a gas if $\gamma = 1.4$,then atomicity,${C_p}$ and ${C_v}$ of the gas are respectively

Obtain the relation between specific heat capacity at constant pressure $(C_P)$ and specific heat capacity at constant volume $(C_V)$ for an ideal gas.

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 $N_{2} = 28; R = 8.3 \; J \; mol^{-1} K^{-1}$.)

If $\frac{R}{C_v} = 0.67$,identify the gas.