# A chemical engineer is studying the following reversible reaction used in the production of methanol, which is carried out in a closed system at high pressure: CO(g) + 2H₂(g) ⇌ CH₃OH(g). The forward reaction is exothermic. Explain what happens to the position of equilibrium when the temperature of the closed system is increased.

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

> Methanol (CH₃OH) is an important industrial chemical used as a fuel and as a solvent. It is manufactured from carbon monoxide and hydrogen gases in a reversible reaction carried out in a closed system.

## Mark scheme (4 marks)

1. The equilibrium position shifts in the direction of the endothermic reaction / shifts in the reverse direction / shifts to the left
2. This is because the system acts to counteract the increase in temperature / opposes the change (Le Chatelier's principle)
3. More reactants / CO and H₂ are formed (at the expense of products)
4. The concentration of methanol / CH₃OH decreases (and the concentration of CO and H₂ increases) until a new equilibrium is reached

## Key terms

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

## Related

- [Revision notes for OCR GCSE Chemistry A: Gateway Science (J248)](https://www.gradenine.co.uk/learn)
- [How to answer "Explain" questions](https://www.gradenine.co.uk/tools/command-word-cheatsheet)
- [Practice this with AI marking (free)](https://www.gradenine.co.uk/start)

---
Source: [GradeNine](https://www.gradenine.co.uk/q/a-chemical-engineer-is-studying-the-d776df94) · Published by Druglandscape Ltd.