The specific heat of a gas:

Explain the difference between the expressions $C_P - C_V = R$,$C_P - C_V = \frac{R}{J}$,and $C_P - C_V = \frac{r}{J}$.

The specific heat of helium at constant volume is $12.6 \,J \,mol^{-1} \,K^{-1}$. The specific heat of helium at constant pressure in $J \,mol^{-1} \,K^{-1}$ is approximately (assume, the universal gas constant, $R=8.314 \,J \,mol^{-1} \,K^{-1}$)

One mole of an ideal monatomic gas requires $210 \, J$ of heat to raise the temperature by $10 \, K$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by $10 \, K$,then the heat required is ....... $J$.

The molar specific heats of an ideal gas at constant pressure and constant volume are denoted by $C_P$ and $C_V$ respectively. If $\gamma = C_P/C_V$ and $R$ is the universal gas constant,then $C_V = $ ........

The amount of heat needed to raise the temperature of $4 \, \text{moles}$ of a rigid diatomic gas from $0^{\circ} \text{C}$ to $50^{\circ} \text{C}$ when no work is done is ......$R$ ($R$ is the universal gas constant).