If $C_P$ and $C_V$ are the specific heats of unit mass of nitrogen at constant pressure and constant volume respectively,then:

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?

If $\gamma$ is the ratio of specific heats and $R$ is the universal gas constant,then the molar specific heat at constant volume $C_{V}$ is given by

To increase the temperature of $1$ $mol$ of an ideal gas by $10$ $K$ at constant pressure,$207$ $J$ of heat is required. If the temperature of this gas is increased by $10$ $K$ at constant volume,the heat required is ....... $J$ $(R = 8.3$ $J/mol$ $K)$.

$5 \ \text{moles}$ of an unknown gas is heated at constant volume from $10^\circ \text{C}$ to $20^\circ \text{C}$. The molar specific heat of this gas at constant pressure is $c_p = 8 \ \text{cal/mol} \cdot ^\circ \text{C}$ and the gas constant is $R = 8.36 \ \text{J/mol} \cdot ^\circ \text{C}$. The change in the internal energy of the gas is . . . . . . calorie.

The specific heat of helium at constant volume is $12.6 \ J \ mol^{-1} \ K^{-1}$. The specific heat of helium at constant pressure in $J \ mol^{-1} \ K^{-1}$ is about (Assume the temperature of the gas is moderate,universal gas constant,$R=8.314 \ J \ mol^{-1} \ K^{-1}$)