Answer:
Ammonia
is prepared on commercial scale by Haber's Process from dinitrogen and
dihydrogen by the following chemical reaction
N2
(g) + 3H2(g) 
2NH3(g)
;
H = ?46.1
kJ mol?1
The
favourable conditions for the forward reactions are derived from Le-Chatelier's
principle. These are:
(a) Low
temperature. Low temperature should favour the formation of ammonia as the
forward reaction is exothermic. But an optimum temperature of nearly 700 K is
necessary to keep the reaction in progress.
(b)
High Pressure. High pressure (about 200 atm or 200 x 105 Pa) is needed
to favour the formation of ammonia because number of moles (gaseous) decrease
in the forward reaction.
(c)
Catalyst. The rate of reaction can be accelerated by using finely divided
iron oxide as catalyst with traces of K2O or Al2O3
or molybdenum acting as a promoter for the catalyst.
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