On an industrial scale, ammonia is prepared by Haber’s process. The constituents of ammonia \\\\({N}_{2}\\\\) and \\\\({H}_{2}\\\\) combine in a ratio of \\\\(1 : 3\\\\).\\\\({N}_{2} + 3 {H}_{2} \\rightleftharpoons 2N{H}_{3}\\\\) The reaction proceeds in the forward direction with a remarkable decrease in volume and thus the reaction is exothermic. In accordance with Le Chatelier’s principle, high pressure would favour the formation of ammonia. The optimum conditions for the production of ammonia are a pressure of approx \\\\(200 \\; atm\\\\), a temperature of approx \\\\(700 \\; K\\\\) and the use of a catalyst such as iron oxide with small amounts of \\\\({K}_{2}O\\\\) and \\\\({Al}_{2}{O}_{3}\\\\) to increase the rate of attainment of equilibrium.