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 $.... \times 10^{11}$.

The kinetic energy of $1$ gram-mole of Argon at $127^{\circ}C$ is .... $J$.

Two gases $A$ and $B$ are contained in the same vessel which is at temperature $T$. The number of molecules of gas $A$ is $N$ and the mass of each molecule is $m$. The number of molecules of gas $B$ is $2N$ and the mass of each molecule is $2m$. If the mean square velocity of the $x$-component of velocity of gas $B$ is $v^2$ and the mean square velocity of the $x$-component of velocity of molecules of gas $A$ is $u_x^2$,then $\frac{u_x^2}{v^2}$ is:

What is the kinetic energy of $1$ mole of a monoatomic gas at $0 \, ^\circ C$? $(R = 8.31 \, J/mol \cdot K)$

The average kinetic energy of $H_2$ molecules at $300 \ K$ is $E$. At the same temperature,the average kinetic energy of an $O_2$ molecule is:

According to the kinetic theory of gases,the average kinetic energy of $1$ gram-mole of a gas is given by which of the following expressions?