The temperature of a gas is $-68^\circ C$. At what temperature in $^\circ C$ will the average kinetic energy of its molecules be twice that of at $-68^\circ C$?

The initial average kinetic energy of the molecules was $E$,when a gas sample is at $27^{\circ} C$. When the gas is heated to $327^{\circ} C$,then the final average kinetic energy will be

$A$ vessel of volume $10 \text{ liters}$ is filled with $H_2$ gas. The total average translational kinetic energy of its molecules is $4.5 \times 10^5 \text{ J}$. The pressure of hydrogen in the vessel is

Assuming the expression for the pressure exerted by the gas, it can be shown that pressure is

$A$ container of volume $10^{-3} \ m^3$ contains $3.0 \times 10^{22}$ gas molecules,each having a mass of $5.3 \times 10^{-26} \ kg$. If the $rms$ speed of the molecules is $400 \ m/s$,calculate the pressure exerted by the gas.

If the momentum transferred by gas molecules to the walls of a container is $p_1 = nmAv_x^2 \Delta t$,then derive the equation for the pressure of the gas.