The molar specific heat at constant pressure of an ideal gas is $(7/2)R$. The ratio of specific heat at constant pressure to that at constant volume is

If the difference between the specific heats of a gas is $4150 \, J/kg \cdot K$ and the ratio of specific heats is $1.4$,then the specific heat at constant volume is ...... $J/kg \cdot K$.

The molar specific heat at constant volume,${C_V}$,for a monoatomic gas is:

$40 \, \text{calories}$ 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 ..... $\text{calories}$.

Write definitions of molar specific heat at constant pressure and constant volume.

$C_{v}$ and $C_{p}$ denote the molar specific heat capacities of a gas at constant volume and constant pressure,respectively. Then
$(A)$ $C_{p}-C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas
$(B)$ $C_{p}+C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas
$(C)$ $C_{p} / C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas
$(D)$ $C_{p} \cdot C_v$ is larger for a diatomic ideal gas than for a monoatomic ideal gas