$A$ gaseous mixture consists of $16\,g$ of helium and $16\,g$ of oxygen. The ratio $\frac{C_P}{C_V}$ of the mixture is

$A$ vessel contains hydrogen and nitrogen gases in the ratio $2: 3$ by mass. If the temperature of the mixture of the gases is $30^{\circ} C$, then the ratio of the average kinetic energies per molecule of hydrogen and nitrogen gases is $($Molecular mass of hydrogen gas $= 2$ and molecular mass of nitrogen gas $= 28)$.

Two ideal gases at temperatures $T_1$ and $T_2$ are mixed. There is no loss of energy. If the number of moles of the two gases are $n_1$ and $n_2$ respectively,then the temperature of the mixture will be:

$1 \, \text{mole}$ of a gas having $\gamma = \frac{7}{5}$ is mixed with $1 \, \text{mole}$ of a gas having $\gamma = \frac{4}{3}$. What will be the $\gamma$ for the mixture?

One gram mole of an ideal gas $A$ with the ratio of constant pressure and constant volume specific heats $\gamma_{A} = 5/3$ is mixed with $n$ gram moles of another ideal gas $B$ with $\gamma_{B} = 7/5$. If the $\gamma$ for the mixture is $19/13$,then what will be the value of $n$?

Two different gases have pressure $P$ and temperature $T$. Their volume is $V$. If these two gases are mixed while keeping the volume and temperature the same,the pressure of the mixture will be...........