The temperature of a gas is $-73^{\circ}C$. To what temperature in $^{\circ}C$ should the gas be heated so that the average kinetic energy of its molecules becomes doubled?

Pressure of an ideal gas at constant volume is proportional to

If the mass of each molecule of a gas kept at a constant pressure $P$ in a container is halved and their speed is doubled,what will be the resulting pressure of the gas?

If the kinetic energy of a helium atom at temperature $T$ is $E$,then the Avogadro constant $N_A$ is given by:

If $r.m.s.$ velocity of a gas is $V_{rms} = 1840 \ m/s$ and its density $\rho = 8.99 \times 10^{-2} \ kg/m^3$,the pressure of the gas will be

$A$ cylinder of capacity $200 \ L$ is filled with $H_2$ gas. The total average translational kinetic energy of the molecules is $1.52 \times 10^5 \ J$. Calculate the pressure of $H_2$ in the cylinder in $N \ m^{-2}$.