An ideal diatomic gas is heated at constant pressure. What is the fraction of total energy applied,which increases the internal energy of the gas?

If the degree of freedom of a gas is $f,$ then the ratio of two specific heats ${C_P}/{C_V}$ is given by

$A$ cylinder of fixed capacity $67.2 \text{ litres}$ contains helium gas at $STP$. The amount of heat needed to raise the temperature of the gas in the cylinder by $20^{\circ} C$ is: (in $\text{ J}$)

The average degree of freedom per molecule of a gas is $6$. The gas performs $25 \ J$ work,while expanding at constant pressure. The heat absorbed by the gas is .... $J$

One mole of an ideal monoatomic gas is heated at a constant pressure from $0^{\circ} C$ to $100^{\circ} C$. The change in the internal energy of the gas is (Given,$R = 8.32 \text{ J mol}^{-1} \text{ K}^{-1}$):

For a certain gas,the ratio of specific heats is given to be $\gamma = 1.5$. For this gas,