Favourable conditions for the manufacture of ammonia by the...

Favourable conditions for the manufacture of ammonia by the reaction $\mathrm{N}_{2}(\mathrm{~g})$ ? $3 \mathrm{II}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NII}_{3}(\mathrm{~g}), \Delta \mathrm{II}=21.9 \mathrm{kcal}$ arc (1) Low temperature, low pressure and catalyst. (2) Low temperature, high pressure and catalyst. (3) High temperature, low pressure and catalyst. (4) High temperature, high pressure and catalyst.

Favourable conditions for the manufacture of ammonia by the reaction $\mathrm{N}_{2}(\mathrm{~g})$ ? $3 \mathrm{II}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NII}_{3}(\mathrm{~g}), \Delta \mathrm{II}=21.9 \mathrm{kcal}$ arc
(1) Low temperature, low pressure and catalyst.
(2) Low temperature, high pressure and catalyst.
(3) High temperature, low pressure and catalyst.
(4) High temperature, high pressure and catalyst.

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Key Concepts

Le Chatelier’s Principle

This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system adjusts to counteract the change and restore a new equilibrium. In the context of ammonia synthesis, increasing or decreasing temperature and pressure influences the direction of the shift to favor either the products or the reactants.

Effect of Temperature on Equilibrium

For exothermic reactions like ammonia synthesis, lower temperatures favor the formation of products because the reaction releases heat. However, operating at too low a temperature can slow down the reaction kinetics, so a balance must be reached in industrial practice.

Effect of Pressure on Equilibrium

Increasing pressure favors the formation of the side of the reaction with fewer moles of gas. Since the production of ammonia results in a decrease in the total number of gas moles compared to the reactants, high pressure shifts the equilibrium toward the ammonia formation.

Role of Catalysts

Catalysts accelerate the rate of reaction without being consumed, enabling the system to reach equilibrium faster. They lower the activation energy for the process, which is particularly important in industrial chemical processes where reaction rates at low temperatures may otherwise be prohibitively slow.

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