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?

An open vessel at 27^oC is heated until two fifth of the air (assumed as an ideal gas) it has escaped from the vessel assuming that the volume of the vessel remains constant, the temperature at which the vessel has been heated is -