The average kinetic energy of a molecule of a gas is

The average translational kinetic energy of nitrogen (molar mass $28$) molecules at a particular temperature is $0.042 \ eV$. The translational kinetic energy of oxygen molecules (molar mass $32$) in $eV$ at double the temperature is:

The relation between the pressure $(P)$,volume $(V)$,and average kinetic energy $(E)$ of a gas is

The molecules of air in the room where you are sitting are all experiencing the force of gravity tending to bring them down. The molecules are also frequently and randomly undergoing collisions,which tend to oppose the effect of the fall under gravity. The density of air is nearly uniform throughout the room because:

The kinetic energy of one gm-mole of a gas at normal temperature and pressure is $(R = 8.31 \text{ J/mol-K})$.

The number of molecules in one litre of an ideal gas at $300 \, K$ and $2$ atmospheric pressure with mean kinetic energy $2 \times 10^{-9} \, J$ per molecule is $.... \times 10^{11}$.