Points I, II and III in the following plot respectively correspond to
(V_mp : most probable velocity)

Consider the following table :

Gas	a/(k Pa dm6 mol-1)	b/(dm3 mol-1)
A	642.32	0.05196
B	155.21	0.04136
C	431.91	0.05196
D	155.21	0.4382

a and b are vander Waals constants. The correct statement about the gases is :

At a given temperature T, gases Ne, Ar, Xe and Kr are found to deviate from ideal gas behaviour. Their equation of state is given as

$$p = {{RT} \over {V - b}}$$ at T.

Here, b is the van der Waals constant. Which gas will exhibit steepest increase in the plot of Z (compression factor) vs p?

Consider the van der Waals constants, a and b, for the following gases.

Gas	Ar	Ne	Kr	Xe
a/ (atm dm6 mol–2)	1.3	0.2	5.1	4.1
b/ (10–2 dm3 mol–1)	3.2	1.7	1.0	5.0

Which gas is expected to have the highest critical temperature?