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 gas,$R/C_V = 0.67$. What kind of molecules is this gas made of?

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

For a gas,the value of $\frac{R}{C_v} = 0.4$. What is the nature of the gas? ($R$ is the universal gas constant)

On giving an equal amount of heat at constant volume to $1 \, mol$ of a monoatomic and a diatomic gas,the rise in temperature $(\Delta T)$ is more for:

$5 \ \text{moles}$ 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.