Write the value of $\gamma$ for a polyatomic gas.

$A$ 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:

To increase the temperature of $2$ moles of an ideal gas by $30^{\circ}C$ to $35^{\circ}C$ at constant pressure,$70 \, cal$ of heat is required. How much heat energy in $cal$ is required to increase the temperature by the same amount at constant volume? $(R = 2 \, cal/mol \cdot K)$

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 = $ ........

When $5 \ mol$ of oxygen gas is heated at constant volume from $10^{\circ}C$ to $20^{\circ}C$,the change in internal energy is ........ $cal$. (Given: $C_P = 8 \ cal/mol \cdot K$,$R = 2 \ cal/mol \cdot K$)

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