If $C_{p}$ and $C_{v}$ are molar specific heats of an ideal gas at constant pressure and volume respectively and $\gamma$ is $C_{p} / C_{v}$,then $C_{p} =$ (where $R$ is the universal gas constant).

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

$70 \, cal$ of heat are required to raise the temperature of $2 \, moles$ of an ideal gas at constant pressure from $30^{\circ}C$ to $35^{\circ}C$. The amount of heat required to raise the temperature of the same gas through the same range ($30^{\circ}C$ to $35^{\circ}C$) at constant volume is ..... $cal$ $(R = 2 \, cal/mol \cdot K)$.

$1 \, mole$ of a gas requires $40 \, calories$ of heat to raise its temperature from $20^{\circ}C$ to $30^{\circ}C$ at constant pressure. How many calories of heat are required to raise the temperature of the same gas by the same amount at constant volume? $(R = 2 \, cal \, mol^{-1} K^{-1})$

The heat energy that must be supplied to $14 \ g$ of nitrogen at room temperature to raise its temperature by $48^{\circ} C$ at constant pressure is (Molecular weight of nitrogen $= 28, R =$ gas constant,$C_p = \frac{7}{2} R$ for diatomic gas). (in $R$)

For a monoatomic ideal gas,the universal gas constant $R$ is $n$ times the molar heat capacity at constant pressure $C_P$. Here,$n$ is ......