Equilibrium in Industrial Processes Flashcards

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In an industrial chemical plant, what does it mean when a reaction is at equilibrium?

The forward and reverse reactions happen at the same rate, so the amounts of each substance stay constant.

The Haber process makes ammonia, which is mainly used to make fertilisers.

N2(g) + 3H2(g) ⇌ 2NH3(g)

High pressure increases the equilibrium yield of ammonia because the reaction makes fewer gas molecules.

Very high pressure needs expensive, very strong equipment and is less safe, so a lower, compromise pressure is used.

The forward reaction in the Haber process is exothermic; it gives out heat.

Lowering the temperature increases the equilibrium yield of ammonia, but makes the reaction slower.

It is a temperature chosen to give a good yield in a reasonable time, while keeping costs manageable.

The iron catalyst speeds up the reaction so equilibrium is reached faster, but it does not change the equilibrium yield of ammonia.

Removing ammonia makes the equilibrium move to make more ammonia, increasing the overall yield.

Unreacted nitrogen and hydrogen are recycled back into the reactor to reduce waste and improve yield.

Industry must balance a fast enough reaction rate with a high enough equilibrium yield, while keeping costs and safety under control.