# The Haber process is a reversible reaction used to produce ammonia. The reaction can reach dynamic equilibrium. Describe what is meant by a reversible reaction and explain what would happen to the concentrations of nitrogen, hydrogen and ammonia once dynamic equilibrium is reached if the temperature is then increased.

> Edexcel GCSE Chemistry (1CH0) — 4.2 Reversible reactions and equilibria · Describe and Explain · 4 marks

> In the Haber process, nitrogen and hydrogen react to produce ammonia. The forward reaction is exothermic.

## Mark scheme (4 marks)

1. A reversible reaction is one in which the products can react together to reform the reactants
2. Increasing temperature favours the endothermic (backward/reverse) reaction
3. The concentration of ammonia decreases
4. The concentrations of nitrogen and hydrogen increase

## Key terms

- [reversible reaction](https://www.gradenine.co.uk/glossary/reversible-reaction)
- [dynamic equilibrium](https://www.gradenine.co.uk/glossary/dynamic-equilibrium)
- [Haber process](https://www.gradenine.co.uk/glossary/haber-process)

## Related

- [Revision notes for Edexcel GCSE Chemistry (1CH0)](https://www.gradenine.co.uk/learn)
- [How to answer "Describe and Explain" questions](https://www.gradenine.co.uk/tools/command-word-cheatsheet)
- [Practice this with AI marking (free)](https://www.gradenine.co.uk/start)

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Source: [GradeNine](https://www.gradenine.co.uk/q/the-haber-process-is-a-reversible-13cdd9f8) · Published by Druglandscape Ltd.