According to the assumptions made in the kinetic theory of gases, when two molecules of a gas collide with each other then

Consider a sample of oxygen behaving like an ideal gas. At $300 \mathrm{K}$, the ratio of root-mean-square (RMS) velocity to the average velocity of the gas molecule would be :

(Molecular weight of oxygen is $32 \mathrm{g} {\mathrm{mol}}^{-1}; R=8.3 \mathrm{J}{ \mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$)

Assertion: An ideal gas is enclosed within a container fitted with a piston. When volume of this enclosed gas is increased at constant temperature, the pressure exerted by the gas on the piston decreases.

Reason: In the above situation, the rate of molecules striking the piston decreases. If the rate ạt which molecules of a gas having same average speed striking a given area of the wall decreases, the pressure exerted by gas on the wall decreases.

$n \mathrm{moles}$ of an ideal gas undergoes a process $A\to B$ as shown in the figure. The maximum temperature of the gas during the process will be