$A$ mixture of one mole of monoatomic gas and one mole of a diatomic gas (rigid) is kept at room temperature $\left(27^{\circ} C\right)$. The ratio of the specific heat of these gases at constant volume is:

For a diatomic gas,write the value of the ratio of $C_P$ and $C_V$.

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

When an ideal diatomic gas is heated at constant pressure,the fraction of the heat utilized to increase the internal energy of the gas is

$Assertion:$ At a given temperature,the specific heat of a gas at constant pressure $(C_p)$ is always greater than its specific heat at constant volume $(C_v)$.
$Reason:$ When a gas is heated at constant volume,some extra heat is needed compared to that at constant pressure for doing work in expansion.

The correct relation between $\gamma = \frac{C_p}{C_v}$ and temperature $T$ is: