$A$ gas is contained in a vessel at pressure $P_0$. If the mass of all molecules is halved and their speed is doubled,what will be the final pressure?

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?

According to the kinetic theory of gases,the total energy of an ideal gas is equal to:

Estimate the average thermal energy of a helium atom at:
$(i)$ room temperature $(27^{\circ} C)$,
$(ii)$ the temperature on the surface of the Sun $(6000\; K)$,
$(iii)$ the temperature of $10$ million kelvin (the typical core temperature in the case of a star).

The average translational kinetic energy of ${O_2}$ (molar mass $32$) molecules at a particular temperature is $0.048 \; eV$. The translational kinetic energy of ${N_2}$ (molar mass $28$) molecules in $eV$ at the same temperature is:

In a vessel,the gas is at pressure $P_0$. If the mass of all the molecules is halved and their speed is doubled,then the resultant pressure will be