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

The molar specific heat of a monoatomic gas at constant pressure is (Universal gas constant $R = 8.3 \,J \,mol^{-1} \,K^{-1}$)

$A$ 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.

For a gas,$\frac{R}{C_{V}} = 0.4$,where $R$ is the universal gas constant and $C_{V}$ is the molar specific heat at constant volume. The gas is made up of molecules which are

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? $(R = 2 \, cal/mol \cdot K)$

Molar specific heat at constant pressure $C_p$ is related to internal energy $U$ and absolute temperature $T$ as $C_p$ is equal to