$A$ flask contains argon and oxygen in the ratio of $3: 2$ in mass and the mixture is kept at $27^{\circ} C$. The ratio of their average kinetic energy per molecule respectively will be ...........

The energy (in $eV$) possessed by a neon atom at $77^{\circ} C$ is (Boltzmann constant,$K_{B} = 1.38 \times 10^{-23} \,J \,K^{-1}$)

At what temperature in $^\circ C$ will the kinetic energy of gas molecules be double the kinetic energy at $27^\circ C$?

The relation between the gas pressure $P$ and average kinetic energy per unit volume $E$ is

If the average kinetic energy of $O_2$ (molar mass $32$) is $0.048 \ eV$,what is the average kinetic energy of $N_2$ (molar mass $28$) at the same temperature (in $eV$)?

$A$ flask contains Hydrogen and Argon in the ratio $2:1$ by mass. The temperature of the mixture is $30^{\circ} C$. The ratio of average kinetic energy per molecule of the two gases $(K_{\text{argon}} / K_{\text{hydrogen}})$ is: (Given: Atomic weight of $Ar = 39.9$)