Find the average kinetic energy for $1$ gram-mole of a monatomic gas.

The number of gas molecules striking per second per square metre of the top surface of a table placed in a room at $20^{\circ} C$ and $1$ atmospheric pressure is of the order of (given $k_{B} = 1.4 \times 10^{-23} \, J K^{-1}$ and the average mass of an air molecule is $m = 5 \times 10^{-27} \, kg$).

$Assertion$: 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 kinetic energy of translation of $20 \, g$ of oxygen at $47^{\circ}C$ is (molecular weight of oxygen is $32 \, g/mol$ and $R = 8.3 \, J/mol \cdot K$).

Two gases are at absolute temperatures $300 \ K$ and $350 \ K$ respectively. The ratio of the average kinetic energy of their molecules is:

Molecular motion shows itself as