The graph of specific heat at constant volume $(C_v)$ for a monoatomic gas with respect to temperature $(T)$ is:

If $C_{p}$ and $C_{v}$ are molar specific heats of an ideal gas at constant pressure and volume respectively and $\gamma$ is $C_{p} / C_{v}$,then $C_{p} =$ (where $R$ is the universal gas constant).

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

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

If a gas has $n$ degrees of freedom,the ratio of specific heats of the gas is:

$5 \ \text{moles}$ of an unknown gas is heated at constant volume from $10^\circ \text{C}$ to $20^\circ \text{C}$. The molar specific heat of this gas at constant pressure is $c_p = 8 \ \text{cal/mol} \cdot ^\circ \text{C}$ and the gas constant is $R = 8.36 \ \text{J/mol} \cdot ^\circ \text{C}$. The change in the internal energy of the gas is . . . . . . calorie.