When an ideal monoatomic gas is heated at constant pressure,the fraction of heat energy supplied that increases the internal energy of the gas is:

For a gas if $\gamma = 1.4$,then atomicity,${C_p}$ and ${C_v}$ of the gas are respectively

Obtain the molar specific heat of a solid by using the law of equipartition of energy.

$40 \, \text{calories}$ 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 ..... $\text{calories}$.

Column-$I$ represents the type of gas and Column-$II$ represents the ${C_P}$ value for that type of gas. Match them correctly:

Column-$I$	Column-$II$
$(a)$ Monoatomic gas	$(i)$ ${C_P} = \frac{3}{2}R$
$(b)$ Diatomic gas with vibration	$(ii)$ ${C_P} = \frac{5}{2}R$
	$(iii)$ ${C_P} = \frac{7}{2}R$
	$(iv)$ ${C_P} = \frac{9}{2}R$

The heat energy required to raise the temperature of $5 \, moles$ of an ideal gas by $5 \, K$ at constant pressure is $600 \, J$. How much heat (in $J$) is required to raise the same mass of the same gas by $5 \, K$ at constant volume? (Take $R = 8.3 \, J/mol \cdot K$)