In the kinetic theory of gases,a molecule of mass $m$ of an ideal gas collides with a wall of a vessel with velocity $V$. The change in the linear momentum of the molecule is

$A$ gas at pressure $P_0$ is contained in a vessel. If the masses of all the molecules are halved and their velocities are doubled,the resulting pressure would be equal to

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:

According to the kinetic theory of gases,

If the $r.m.s.$ velocity of a gas is $v_{rms} = 1840 \ m/s$ and its density is $\rho = 8.99 \times 10^{-2} \ kg/m^3$,what is the pressure of the gas?

What is the kinetic energy of one gram mole of a gas at standard temperature and pressure? $(R = 8.31 \ J/mol \cdot K)$