(i) Any real gas behaves ideally at very low pressure and high temperature explain.
(ii) The value of van der waals constant 'a' for `N_(2)` and `NH_(3)` are 1.37 and 4.30 `L^(2)*atm*mol^(-2)` respectively explain the difference in values.

Explanation

(ii) Van der waals constant 'a' denotes magnitude of attractive forces between the molecules of real gases. Value of 'a' is higher in case of `NH_(3)` than `N_(2)`. That means attractive forces (Londong force, dipole-dipole attraction force) present among the molecules of `NH_(3)` is stronger than that of `N_(2)` (Londong force). consequently `NH_(3)` can be liquefied more easily than `N_(2)`.