# Ethanol is manufactured industrially by the hydration of ethene. The reaction takes place in a closed container and reaches a dynamic equilibrium. Explain what is meant by the term 'dynamic equilibrium' and describe how increasing the concentration of ethene in the closed container would affect the position of this equilibrium.

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

> Ethene reacts with steam to produce ethanol: C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g). The reaction is carried out in a closed container and reaches a dynamic equilibrium.

## 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 the concentration of ethene causes the equilibrium position to shift to the right / towards the products
4. This is because the system acts to reduce the increased concentration of ethene / opposes the change

## Key terms

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

## 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/ethanol-is-manufactured-industrially-by-the-7ad18f7e) · Published by Druglandscape Ltd.