Using the law of equipartition of energy, the specific heat (in $J\, kg^{-1}\, K^{-1}$) of aluminium at room temperature can be estimated to be (atomic weight of aluminium $= 27$).

One mole of an ideal gas requires $207 \, J$ of heat to raise the temperature by $10 \, K$ when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by the same $10 \, K$,the heat required is ...... $J$ (Given the gas constant $R = 8.3 \, J/mol \cdot K$)

$310 \ J$ 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 $.... \ J$.

The ratio of the molar specific heat capacities of monatomic and diatomic gases at constant pressure is (in $: 7$)

If the degree of freedom of a gas is $f,$ then the ratio of two specific heats ${C_P}/{C_V}$ is given by

The ratio of the specific heats $\frac{C_{p}}{C_{v}}=\gamma$,in terms of degrees of freedom $(n)$ is