Out of `N_(2)` and `NH_(3)`, which one will have greater value for van der Waals constant 'a' and which one will have greater value for der Waals constant 'b' ?

Explanation

(i) As `NH_(3)` is more easily liquefiable (due to hydrogen bonding), intermolecular forces of attraction are stronger than in `N_(2)`. Hence, `NH_(3)` will have greater value for 'a'.
(ii) As `NH_(3)` molecule is larger in size than `N_(2)`, hence `NH_(3)` will have greater value for 'b'.
(For `NH_(3),a=4.17 L^(2) atm mol^(-2), b=0.0371 L mol^(-1) For N_(2), a=1.39 L^(2) atm mol^(-2), b=0.0319 L mol^(-1)`)