The molar specific heat of an ideal gas at constant pressure and constant volume is $C_{p}$ and $C_{v}$ respectively. If $R$ is the universal gas constant and $\gamma = \frac{C_p}{C_v}$,then $C_v =$

The molar specific heat at constant volume,${C_V}$,for a monoatomic gas is:

For a gas molecule with $6$ degrees of freedom,which one of the following relations between gas constant '$R$' and molar specific heat '$C_{V}$' is correct?

When $300 \ J$ of heat is given to an ideal gas with $C_{p} = \frac{7}{2} R$,its temperature rises from $20^{\circ}C$ to $50^{\circ}C$ while keeping its volume constant. The mass of the gas is (approximately) . . . . . . g. (Assume the molar mass of the gas is $28 \ g/mol$ and $R = 8.314 \ J/mol \cdot K$).

If a gas has $n$ degrees of freedom,then the ratio of $\frac{C_p}{C_V}$ is

$310 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25 \ ^oC$ to $35 \ ^oC$. The amount of heat required to raise the temperature of the gas through the same range at constant volume is $.... \ J$.