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.

$2$ moles of $O_2$ and $4$ moles of $Ar$ are filled in a container at temperature $T$. What is the total internal energy (in $, RT$)?

The relation between internal energy $U$,pressure $P$,and volume $V$ for an ideal gas is given by $U = 2 + 2PV$. The gas is:

Two moles of an ideal gas with $\frac{C_{P}}{C_{V}}=\frac{5}{3}$ are mixed with $3$ moles of another ideal gas with $\frac{C_{P}}{C_{V}}=\frac{4}{3}$. The value of $\frac{C_{P}}{C_{V}}$ for the mixture is

$A$ gaseous mixture consists of $4 \ g$ oxygen and $4 \ g$ of helium. The ratio $\frac{C_p}{C_V}$ of the mixture is ($C_p$ and $C_V$ are molar specific heats of the mixture at constant pressure and at constant volume respectively).

$A$ mixture of two moles of hydrogen and one mole of argon gas is taken in a closed container at room temperature. Consider the following two statements:
$(i)$ The average kinetic energy of each molecule of $H_2$ and $Ar$ are the same.
$(ii)$ The partial pressure due to argon gas is more than that due to hydrogen gas.