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

For a gas,$\frac{R}{C_{v}} = 0.67$. This gas is made up of molecules which are

If $C_{p}$ and $C_{v}$ are molar specific heats of an ideal gas at constant pressure and volume respectively and $\gamma$ is $C_{p} / C_{v}$,then $C_{p} =$ (where $R$ is the universal gas constant).

To raise the temperature of a certain mass of gas by $50^{\circ} C$ at a constant pressure,$160$ calories of heat is required. When the same mass of gas is cooled by $100^{\circ} C$ at constant volume,$240$ calories of heat is released. How many degrees of freedom does each molecule of this gas have (assume gas to be ideal)?

When some amount of heat energy is supplied to a monatomic gas, the percentage of heat energy used for increasing the internal energy of the gas $(\gamma = 5/3)$ is

The value of the gas constant $(R)$ calculated from the perfect gas equation is $8.32 \ J/mol \cdot K$,whereas its value calculated from the knowledge of $C_P$ and $C_V$ of the gas is $1.98 \ cal/mol \cdot K$. From this data,the value of $J$ is ......... $J/cal$.