The Habar's process of production of ammonia involves the equilibrium:
`N_(2)(g)+3H_(2)(g)hArr2NH_(2)(g)`
Assuming `DeltaH^(@)` and `DeltaS^(@)` for the reaction do not change with temperature, which of the statements is true?
`(DeltaH^(@)=-95kJ and DeltaS^(@)=-198JK^(-1))`

Options

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

Answer

A

Explanation

`DeltaG^(@)=DeltaH^(@)-TDeltaS^(@)`
`=-95xx1000-500xx(-190)`
`=-95000+95000=0`
thus, ammonia will dissociate below 500 K because `DeltaG^(@)` will be negative.