Helium and argon are placed in a flask at the same room temperature $(300 \ K)$. What is the ratio of the average kinetic energies (per molecule) of helium and argon?

Number of molecules in a volume of $4\, cm^{3}$ of a perfect monoatomic gas at some temperature $T$ and at a pressure of $2\, cm$ of mercury is close to $?$
(Given,mean kinetic energy of a molecule (at $T$) is $4 \times 10^{-14}\, erg$,$g=980\, cm/s^{2}$,density of mercury $=13.6\, g/cm^{3}$)

Consider a gas with density $\rho$ and $\bar{c}$ as the root mean square velocity of its molecules contained in a volume. If the system moves as a whole with velocity $v$,then the pressure exerted by the gas is

Explain the kinetic interpretation of temperature.

The average translational kinetic energy of $O_2$ molecules at a particular temperature is $0.048 \ eV$. The average translational kinetic energy of an equal number of $N_2$ molecules at the same temperature is (in $eV$):

The ratio of the mean kinetic energy of hydrogen and nitrogen at temperatures $300 \, K$ and $450 \, K$ respectively is: