When $5 \ mol$ of oxygen gas is heated at constant volume from $10^{\circ}C$ to $20^{\circ}C$,the change in internal energy is ........ $cal$. (Given: $C_P = 8 \ cal/mol \cdot K$,$R = 2 \ cal/mol \cdot K$)

$306 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25^{\circ} C$ to $35^{\circ} C$. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is (in $J$)

Let $\gamma_1$ be the ratio of molar specific heat at constant pressure and molar specific heat at constant volume of a monoatomic gas and $\gamma_2$ be the similar ratio of a diatomic gas. Considering the diatomic gas molecule as a rigid rotator,the ratio $\frac{\gamma_1}{\gamma_2}$ is

$176 \text{ grams}$ of $CO_2$ can change its temperature from $0^{\circ} C$ to $30^{\circ} C$ by absorbing $3600 \text{ joules}$ of thermal energy. The molar specific heat of $CO_2$ in $J \ mol^{-1} K^{-1}$ is:

The value of $C_V$ for one mole of neon gas is

One mole of an ideal monoatomic gas is heated at a constant pressure from $0^{\circ} C$ to $100^{\circ} C$. The change in the internal energy of the gas is (Given,$R = 8.32 \text{ J mol}^{-1} \text{ K}^{-1}$):