The molar specific heat of an ideal gas at constant pressure and constant volume is '$C_p$' and $C_v$' respectively. If 'R' is the universal gas constant and the ratio of $C_p$ to $C_v$ is ${}^{\prime }{\gamma }^{\prime }$ then $C_v$ =

Q. The molar specific heats of an ideal gas at constant pressure and volume are denoted by $C_p$ and $C_v$, respectively. If $\gamma =$ $\frac{C_p}{C_v}$ and R is the universal gas constant, then $C_v$ is equal to -

Q. The molar specific heat capacity of an ideal gas, at constant pressure and at constant volume, are denoted by $C_p\text{and}{C}_v$, respectively. If $\gamma =\frac{C_p}{C_v}\text{and R}$ is the universal gas constant, then $C_v$ is equal to,

Q. For an ideal gas $\frac{C_p}{C_v}=\gamma$. then its specific heat capacity at constant volume $\left(C_v\right)$ is :

Q.

For an ideal gas $(\frac{C_P}{C_v}=\gamma )$; of molar mass M, its specific heat capacity at constant volume is:

Q. During an adiabatic process, if the pressure of the ideal gas is proportional to the cube of its temperature, the ratio $\gamma =\frac{C_p}{C_v}$ is
($C_p=$ Specific heat at constant pressure ; $C_v=$Specific heat at constant volume)