One mole of a gas mixture is heated under constant pressure,and the heat supplied $Q$ is plotted against the temperature difference $\Delta T$ acquired. Find the approximate value of $\gamma$ for the mixture.

$3\, \text{moles}$ of an ideal gas at a temperature of $27^{\circ}\, \text{C}$ are mixed with $2\, \text{moles}$ of an ideal gas at a temperature of $227^{\circ}\, \text{C}$. Determine the equilibrium temperature $(^{\circ}\, \text{C})$ of the mixture, assuming no loss of energy.

One mole of monoatomic gas and three moles of diatomic gas are put together in a container. The molar specific heat (in $J\,K^{-1}\,mol^{-1}$) at constant volume is $(R = 8.3\,J\,K^{-1}\,mol^{-1})$.

$A$ gas mixture consists of $8$ moles of argon and $6$ moles of oxygen at temperature $T$. Neglecting all vibrational modes,the total internal energy of the system is (in $RT$)

The pressure of a mixture of $64 \ g$ of oxygen,$28 \ g$ of nitrogen,and $132 \ g$ of carbon dioxide gases in a closed vessel is $P$. Under isothermal conditions,if the entire oxygen is removed from the vessel,the pressure of the mixture of the remaining two gases is:

If two moles of diatomic gas and one mole of monoatomic gas are mixed,then the ratio of specific heats is: