# Ammonia is produced in the Haber process using the following reversible reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g). The forward reaction is exothermic. Explain what happens to the position of equilibrium when the temperature is increased, and what effect this has on the yield of ammonia.

> OCR GCSE Chemistry A: Gateway Science (J248) — C5.3 Equilibria · Explain · 4 marks

> Ammonia is produced industrially via the Haber process. The reaction is reversible and reaches dynamic equilibrium under certain conditions.

## Mark scheme (4 marks)

1. An increase in temperature causes the equilibrium position to shift in the direction of the endothermic reaction
2. The endothermic direction is the backward/reverse reaction (breaking down ammonia)
3. This is because Le Chatelier's principle states the equilibrium moves to counteract the change / to absorb the extra heat energy
4. The yield of ammonia decreases because more ammonia is converted back into nitrogen and hydrogen

## Key terms

- [reversible reaction](https://www.gradenine.co.uk/glossary/reversible-reaction)

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Source: [GradeNine](https://www.gradenine.co.uk/q/ammonia-is-produced-in-the-haber-7678d00d) · Published by Druglandscape Ltd.