Which of the following statements is correct?

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?

In gases of diatomic molecules,the ratio of the two specific heats of gases ${C_P}/{C_V}$ is

One mole of an ideal gas requires $207 \, J$ of heat to raise the temperature by $10 \, K$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10 \, K$,the heat required is ...... $J$ (Given the gas constant $R = 8.3 \, J/mol \cdot K$)

What amount of heat (in $J$) must be supplied to $2.0 \times 10^{-2} \; kg$ of nitrogen (at room temperature) to raise its temperature by $45 \; ^{\circ}C$ at constant pressure? (Molecular mass of $N_{2} = 28; R = 8.3 \; J \; mol^{-1} K^{-1}$.)

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