If $E$ is the kinetic energy per mole of an ideal gas and $T$ is the absolute temperature,then the universal gas constant is given as

The average translational kinetic energy of a hydrogen gas molecule at $NTP$ will be. [Boltzmann's constant $k_B = 1.38 \times 10^{-23} \text{ J/K}$]

According to the Kinetic Theory of Gases,at a given temperature:

An ideal gas in a container of volume $500 \text{ c.c.}$ is at a pressure of $2 \times 10^5 \text{ N/m}^2$. The average kinetic energy of each molecule is $6 \times 10^{-21} \text{ J}$. The number of gas molecules in the container is:

At what temperature in $^\circ C$ is the average molecular kinetic energy of any gas double that of its value at $20^\circ C$?

Absolute temperature can be calculated by