The energy of all molecules of a monoatomic gas having a volume $V$ and pressure $P$ is $\frac{3}{2}PV$. The total translational kinetic energy of all molecules of a diatomic gas at the same volume and pressure is:

$A$ gas has volume $V$ and pressure $P$. The total translational kinetic energy of all the molecules of the gas is

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 $-68^\circ C$?

$Assertion$: The total translational kinetic energy of all the molecules of a given mass of an ideal gas is $1.5$ times the product of its pressure and its volume.
$Reason$: The molecules of a gas collide with each other and the velocities of the molecules change due to the collision.

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?

If the average kinetic energy of a gas molecule at $27^{\circ} C$ is $3.3 \times 10^{-20} \,J$, then the average kinetic energy of the gas molecules at $127^{\circ} C$ is