$A$ mixture of one mole of monoatomic gas and one mole of a diatomic gas (rigid) is kept at room temperature $\left(27^{\circ} C\right)$. The ratio of the specific heat of these gases at constant volume is:

If $C_p$ and $C_v$ denote the specific heats of nitrogen per unit mass at constant pressure and constant volume respectively,then

For an ideal gas,the molar specific heat at constant pressure is $(7/2) R$. Find the ratio of the molar specific heat at constant pressure to the molar specific heat at constant volume.

$1 \, mole$ of a gas requires $40 \, calories$ of heat to raise its temperature from $20^{\circ}C$ to $30^{\circ}C$ at constant pressure. How many calories of heat are required to raise the temperature of the same gas by the same amount at constant volume? $(R = 2 \, cal \, mol^{-1} K^{-1})$

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 ....... $J$.

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