The Haber's process for production of ammonia involves the equilibrium: `N _(2) (g) + 3 H _(2) (g) hArr 2NH _(3) (g)` Assuming `Delta H^(@) and Delta S ^(@)` for the reaction do not change with temperature, which of the statements is true? `(Delta H ^(@) =- 95kJ and Delts S ^(@) =- 190 JK ^(-1))`

Options

A. Ammonia dissociates spontaneously below 500 K.
B. Ammonia dissociates spontaneously above 500K.
C. Ammonia dissociates at all temperatures.
D. Ammonia does not dissociate at any temperature.

Explanation

`Delta G ^(@) = Delta H ^(@) - T Delta S ^(@) =- 95 xx 100 - 500 xx ( - 190) =- 95000 + 95000 =0`
Thus, ammonium will dissociate below 500 K because `Delta G ^(@)` will be negative.