If the ratio of the universal gas constant $(R)$ and the specific heat capacity at constant volume $(C_v)$ of a gas is given by $0.67$,then the gas is

$40 \, \text{calories}$ of heat is needed to raise the temperature of $1 \, \text{mole}$ of an ideal monoatomic gas from $20^{\circ}C$ to $30^{\circ}C$ at a constant pressure. The amount of heat required to raise its temperature over the same interval at a constant volume $(R = 2 \, \text{cal} \, \text{mol}^{-1} \text{K}^{-1})$ is ..... $\text{calories}$.

If a gas has $f$ degrees of freedom,what is the ratio ${C_p}/{C_v}$?

$Assertion :$ The ratio of $\frac{C_p}{C_v}$ for an ideal diatomic gas is less than that for an ideal monoatomic gas (where $C_p$ and $C_v$ have usual meaning).
$Reason :$ The atoms of a monoatomic gas have less degrees of freedom as compared to molecules of the diatomic gas.

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

Molar specific heat at constant volume,for a non-linear triatomic gas is (vibration mode neglected).