In the case of a diatomic gas,the fraction of heat supplied at constant pressure that is used for the expansion of the gas is:

The amount of heat that must be supplied to $35 \ g$ of oxygen at room temperature to raise its temperature by $80^{\circ} C$ at constant volume is (molecular mass of oxygen is $32$ and $R = 8.3 \ J \ mol^{-1} \ K^{-1}$) (in $kJ$)

For a gas,$\frac{R}{C_{v}} = 0.67$. This gas is made up of molecules which are

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 $R = 8.3 \, J/mol \cdot K$)

$A$ diatomic gas molecule has translational,rotational,and vibrational degrees of freedom. The ratio ${C_P}/{C_V}$ is

Which of the following formulae is wrong?