Assertion $(A)$: The temperature of a gas is a result of the kinetic energy of its molecules.
Reason $(R)$: Due to kinetic energy,the molecules collide with each other to produce thermal energy.

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

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?

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:

At what temperature does the average translational kinetic energy of a molecule in a gas become equal to the kinetic energy of an electron accelerated from rest through a potential difference of $V$ volt? ($N=$ Avogadro number,$R=$ gas constant,$e=$ electronic charge)

The average kinetic energy of a gas at $-23^{\circ}C$ and $75 \, cm$ pressure is $5 \times 10^{-14} \, erg$ for $H_2$. The mean kinetic energy of $O_2$ at $227^{\circ}C$ and $150 \, cm$ pressure will be: