# Iron is produced in a blast furnace by the reduction of iron(III) oxide with carbon monoxide. The equation for this reaction is: Fe₂O₃ + 3CO → 2Fe + 3CO₂. A student states that 160 g of iron(III) oxide would produce 112 g of iron. Show whether the student is correct by using mole calculations. (Relative atomic masses: Fe = 56, O = 16, C = 12.) (5 marks)

> Edexcel A-Level Chemistry (9CH0) — 5.1 Calculations using moles · Justify · 5 marks

> Iron is produced industrially in a blast furnace. The theoretical yield of iron can be calculated from the balanced equation for the reaction.

## Mark scheme (5 marks)

1. Correct molar mass of Fe₂O₃ calculated as 160 g/mol
2. Correct calculation of moles of Fe₂O₃ as 1 mol
3. Correct use of molar ratio to determine moles of Fe produced
4. Correct molar mass of Fe used as 56 g/mol
5. Correct mass of Fe calculated as 112 g AND conclusion that the student is correct

## Related

- [Revision notes for Edexcel A-Level Chemistry (9CH0)](https://www.gradenine.co.uk/learn)
- [How to answer "Justify" questions](https://www.gradenine.co.uk/tools/command-word-cheatsheet)
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