If the mean free path of atoms is doubled,then the pressure of the gas will become:

The value of critical temperature in terms of Vander Waals constants $a$ and $b$ is

For the given concentration,if the ratio of the diameters of the molecules of two gases is $1: 2$,then the ratio of their mean free paths is

Given below are two statements:
Statement $(I)$: The mean free path of gas molecules is inversely proportional to the square of the molecular diameter.
Statement $(II)$: The average kinetic energy of gas molecules is directly proportional to the absolute temperature of the gas.
In the light of the above statements,choose the correct answer from the options given below:

The mean free path of molecules of a certain gas at $STP$ is $1500\,d$,where $d$ is the diameter of the gas molecules. While maintaining the standard pressure,the mean free path of the molecules at $373\,K$ is approximately $..........\,d$

$A$ gas deviates maximum from the ideal gas law at