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

For hydrogen gas $C_p - C_v = a$ and for oxygen gas $C_p - C_v = b$. The relation between $a$ and $b$ is given by:

The ratio of two specific heats $\frac{C_P}{C_V}$ of $CO$ is

$50 \, cal$ of heat is required to raise the temperature of $1 \, mol$ of an ideal gas from $20^{\circ} C$ to $25^{\circ} C$,while the pressure of the gas is kept constant. The amount of heat required to raise the temperature of the same gas through the same temperature range at constant volume is ........ $cal$ $(R = 2 \, cal / mol \cdot K)$.

The adiabatic Bulk modulus of a diatomic gas at atmospheric pressure is

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,$R=8.314 \ J \ mol^{-1} \ K^{-1}$)