States of Matter

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 = $\frac{\mathrm{RT}}{\mathrm{V} - \mathrm{b}}$ 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?

• Ne

• Xe

• Ar

• Kr

Consider the following table:

And b are vander walls contants . The correct statement a Bout the gases is :

• Gas A will occupy than gas D  Compressible than gas D Gas C will Occupy more volume than

• gas A gas B will be more compressible than gas D Gas C will Occupy Lesser volume than

• Gas A gas B will be more compressible than gas D Gas C will Occupy Lesser volume than

• Gas A: gas B will be lesser Compressble than gas D

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

• V_mp of N₂ (300K); V_mp of O₂(400K); V_mp of H₂ (300K)

• V_mp of N₂ (300K); V_mp of H₂(300K); V_mp of O₂ (400K)

• V_mp of H₂ (300K); V_mp of N₂(300K); V_mp of O₂ (400K)

• V_mp of O₂ (400K); V_mp of N₂(400K); V_mp of H₂ (300K)