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

What is the relationship between the internal energy $U$ of an ideal gas and its pressure $P$ and volume $V$?

For a gas,the value of $\frac{R}{C_v} = 0.4$. What is the nature of the gas? ($R$ is the universal gas constant)

The specific heat of helium at constant volume is $12.6 \ J \ mol^{-1} \ K^{-1}$. The specific heat of helium at constant pressure in $J \ mol^{-1} \ K^{-1}$ is about (Assume the temperature of the gas is moderate,universal gas constant,$R=8.314 \ J \ mol^{-1} \ K^{-1}$)

Let $\gamma_1$ be the ratio of molar specific heat at constant pressure and molar specific heat at constant volume of a monoatomic gas and $\gamma_2$ be the similar ratio of a diatomic gas. Considering the diatomic gas molecule as a rigid rotator,the ratio $\frac{\gamma_2}{\gamma_1}$ is

Identify the correct relationship between the molar heat capacities of an ideal gas.