Five moles of helium are mixed with two moles of hydrogen to form a mixture. Take molar mass of helium $M_1 = 4 \ g/mol$ and that of hydrogen $M_2 = 2 \ g/mol$. The equivalent molar mass of the mixture is:

If $7 \, g$ of $N_{2}$ is mixed with $20 \, g$ of $Ar$,the $C_{p} / C_{v}$ ratio of the mixture will be:

If $2 \text{ mole}$ of an ideal monoatomic gas at temperature $T$ is mixed with $6 \text{ mole}$ of another ideal monoatomic gas at temperature $2T$, then the temperature of the mixture is:

The volume $V$ of an enclosure contains a mixture of three gases: $16 \, g$ of oxygen,$28 \, g$ of nitrogen,and $44 \, g$ of carbon dioxide at absolute temperature $T$. Consider $R$ as the universal gas constant. The pressure of the mixture of gases is:

The ratio of specific heat of a mixture of one mole of helium and one mole of hydrogen gas will be

Two ideal polyatomic gases at temperatures $T_{1}$ and $T_{2}$ are mixed such that there is no loss of energy. If $F_{1}$ and $F_{2}$,$m_{1}$ and $m_{2}$,$n_{1}$ and $n_{2}$ are the degrees of freedom,masses,and number of molecules of the first and second gas respectively,then the temperature of the mixture of these two gases is: