An ideal mono-atomic gas of given mass is heated at constant pressure. In this process, the fraction of supplied heat energy used for the increase of the internal energy 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 $kJ$)

The specific heat at constant pressure $(C_P)$ is greater than the specific heat at constant volume $(C_V)$ for the same gas because:

Specific heats of an ideal gas at constant pressure and volume are denoted by $C_p$ and $C_v$ respectively. If $\gamma = \frac{C_p}{C_v}$ and $R$ is the universal gas constant,then $C_v$ is equal to:

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 ......

For an ideal gas,the molar specific heat at constant pressure is $(7/2) R$. Find the ratio of the molar specific heat at constant pressure to the molar specific heat at constant volume.