One mole of an ideal monatomic gas requires $210 \, J$ 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 $10 \, K$,then the heat required is ....... $J$.

The figure shows the variation in heat supplied $(Q)$ with the change in temperature $(\Delta T)$ in an isobaric process for a monoatomic $(M)$,diatomic $(D)$,and a polyatomic $(P)$ gas. The initial state of all the gases is the same,and the scales for the two axes coincide. Ignoring vibrational degrees of freedom,the lines $a, b,$ and $c$ respectively correspond to

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

When an ideal diatomic gas is heated at constant pressure,the fraction of the heat utilized to increase the internal energy of the gas is

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

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