In the Haber's process of the synthesis of ammonia, the use of catalyst helps

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increasing rate constant without changing the equilibrium amount of ${NH}_{3}$

increasing rate constant with increasing the equilibrium amount of ${NH}_{3}$

decreasing rate constant with increasing the equilibrium amount of ${NH}_{3}$

decreasing rate constant with decreasing the equilibrium amount of ${NH}_{3}$

answer is A.

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Detailed Solution

Nitrogen from the air is combined with hydrogen to create ammonia in the Haber process. Ammonia is produced exothermically and the reaction is reversible.
Iron is employed as a catalyst in this process.
The catalyst is used to speed up ammonia synthesis while keeping the amount produced constant.

$N_{2} + 3 H_{2} \to 2 {NH}_{3}$