In the Haber process for the industrial manufacturing of ammonia involving the reaction $ N_{2}(g)+3 H_{2}(g) \rightleftharpoons 2 N H_{3}(g) $ at 200atm pressure in the presence of a catalyst, a temperature of about $ 500^{\circ} \mathrm{C} $ is used. This is considered as optimum tem

Question

In the Haber process for the industrial manufacturing of ammonia involving the reaction $ N_{2}(g)+3 H_{2}(g) \rightleftharpoons 2 N H_{3}(g) $ at 200atm pressure in the presence of a catalyst, a temperature of about $ 500^{\circ} \mathrm{C} $ is used. This is considered as optimum temperature for the process because:

Accepted Answer

rate of the catalytic reaction is fast enough while the yield is also appreciable for this exothermic reaction at this temperature. The Haber process uses a temperature that balances two competing effects: lower temperatures favor ammonia formation at equilibrium, but they make the reaction too slow. Around 500°C, the catalyst gives a fast enough rate while the equilibrium yield remains acceptable.

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