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

$A$ vessel contains $3$ moles of $He$,$1$ mole of $Ar$,$5$ moles of $N_2$,and $3$ moles of $H_2$. If the vibrational modes are ignored,the total internal energy of the system of gases is (in $RT$)

Four moles of hydrogen,two moles of helium and one mole of water vapour form an ideal gas mixture. $[C_v$ for hydrogen $= \frac{5}{2} R, C_v$ for helium $= \frac{3}{2} R, C_v$ for water vapour $= 3 R]$. What is the molar specific heat at constant pressure of the mixture?

One mole of an ideal monoatomic gas $(\gamma = 5/3)$ is mixed with one mole of a diatomic gas $(\gamma = 7/5).$ What is $\gamma$ for the mixture? $\gamma$ denotes the ratio of specific heat at constant pressure to that at constant volume.

In a container,there is a mixture of two different gases. Will both gases have the same kinetic energy?

$A$ mixture of two non-reactive ideal gases is enclosed in a vessel consisting of one mole of a monatomic gas '$A$' and 'n' moles of a diatomic gas '$B$' at a temperature '$T$'. If the adiabatic constant of the gaseous mixture is $\frac{13}{9}$,then the value of 'n' is: