For a diatomic gas,write the value of the ratio of $C_P$ and $C_V$.

$306 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25^{\circ} C$ to $35^{\circ} C$. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is (in $J$)

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 $kJ$)

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

The energy required to raise the temperature of $5 \, \text{moles}$ of $H_2$ gas from $30^{\circ}C$ to $60^{\circ}C$ at constant pressure is ......... $\text{calories}$ $(R = 2 \, \text{cal/mol} \cdot \text{K})$.

The molar specific heat of an ideal gas at constant pressure and constant volume is $C_{p}$ and $C_{V}$ respectively. If $R$ is the universal gas constant and the ratio of $C_{p}$ to $C_{V}$ is $\gamma$,then $C_{p}$ is equal to: