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

$A$ diatomic gas is heated at constant pressure. What fraction of the heat energy is used to increase the internal energy?

The ratio of the specific heats $\frac{C_p}{C_v} = \gamma$ in terms of degrees of freedom $(n)$ is given by

$40 \, \text{calories}$ of heat is needed to raise the temperature of $1 \, \text{mole}$ of an ideal monoatomic gas from $20^{\circ}C$ to $30^{\circ}C$ at a constant pressure. The amount of heat required to raise its temperature over the same interval at a constant volume $(R = 2 \, \text{cal} \, \text{mol}^{-1} \text{K}^{-1})$ is ..... $\text{calories}$.

The ratio of specific heats $(\gamma)$ of an ideal gas is given by

If the molar specific heat at constant volume is $\frac{3R}{2}$,then the adiabatic index $\gamma$ is: