The molar specific heat at constant volume,${C_V}$,for a monoatomic gas 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? $(R = 2 \, cal/mol \cdot K)$

$A$ 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:

If $C_p$ and $C_v$ denote the specific heat of nitrogen at constant pressure and constant volume respectively,then

The specific heat of an ideal gas is

If a gas has $n$ degrees of freedom, then the ratio of $\frac{C_p}{C_V}$ is