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 energy of a gas per litre is $600 \text{ J}$. What will be its pressure?

At $300 \ K$,the number of $H_2$ molecules is twice the number of $O_2$ molecules. What is the ratio of the total kinetic energy of $H_2$ to that of $O_2$?

The $rms$ speed of an ideal hydrogen gas molecule in a gas chamber at $0^{\circ}C$ is $3180 \ m/s$. What is the pressure of the hydrogen gas in atmospheres? (Given: Density of hydrogen gas $\rho = 8.99 \times 10^{-2} \ kg/m^3$,$1 \ atm = 1.01 \times 10^5 \ N/m^2$)

The translational kinetic energy of the molecules of a gas at absolute temperature $T$ can be doubled by

$A$ gas is filled in a container at pressure ${P_0}$. If the mass of all molecules is halved and their $rms$ speed is doubled,what will be the new pressure?