# The Haber process is used to manufacture ammonia. The reaction reaches a dynamic equilibrium. Explain what is meant by the term 'dynamic equilibrium' and describe how changing the pressure affects the position of this equilibrium. The equation for the reaction is: N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

> Edexcel GCSE Chemistry (1CH0) — 9.3 Dynamic equilibria, calculations involving volumes of gases (Chem only) · Explain · 4 marks

> The Haber process operates at high temperature and high pressure. The reaction is reversible and reaches a state of dynamic equilibrium inside the reactor vessel.

## Mark scheme (4 marks)

1. The forward and reverse reactions are both still occurring (at equilibrium)
2. The rate of the forward reaction equals the rate of the reverse reaction
3. Increasing pressure shifts the equilibrium to the right / towards the products (ammonia)
4. Because there are fewer moles of gas on the right-hand side (2 moles) than the left-hand side (4 moles), so the system reduces pressure by favouring the side with fewer gas molecules

## Key terms

- [dynamic equilibrium](https://www.gradenine.co.uk/glossary/dynamic-equilibrium)
- [pressure](https://www.gradenine.co.uk/glossary/pressure)

## Related

- [Revision notes for Edexcel GCSE Chemistry (1CH0)](https://www.gradenine.co.uk/learn)
- [How to answer "Explain" questions](https://www.gradenine.co.uk/tools/command-word-cheatsheet)
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Source: [GradeNine](https://www.gradenine.co.uk/q/the-haber-process-is-used-to-47a2aec6) · Published by Druglandscape Ltd.