The ratio of the specific heats $\frac{C_{p}}{C_{v}}=\gamma$,in terms of degrees of freedom $(n)$ is

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

When heat is supplied to a diatomic gas,it expands at constant pressure. What fraction of the heat supplied is converted into internal energy?

$A$ gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume $(C_v)$ to the specific heat of gas at constant pressure $(C_p)$ will be.

To increase the temperature of $1$ mole of an ideal monatomic gas by $10^{\circ}C$ at constant pressure,$40 \, cal$ of heat is required. How much heat (in $cal$) is required to increase the temperature by the same amount at constant volume?

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