Iron is extracted from its ore using reduction with carbon in a blast furnace. Explain why this method can be used to extract iron, and describe what happens chemically during the extraction process.
Written & reviewed by James Millett — Biology (Imperial College London), PGCE Science (University of Cambridge).
Model answer (4 marks)
Iron is less reactive than carbon, so carbon can displace it. In a blast furnace the iron ore (Fe₂O₃) is heated with carbon (C). The carbon reduces the iron oxide – the iron oxide loses oxygen. Iron metal is produced while the carbon is oxidised, forming CO₂ or CO.
Examiner tips
- Use the term ‘reduction’ and ‘oxidation’ explicitly
- Show the iron ore formula and the carbon source
- Mention that carbon is more reactive than iron
- State the products – Fe and CO/CO₂
Common mistakes
- Saying iron is more reactive than carbon
- Omitting the role of carbon as the reducing agent
- Not naming the products (CO or CO₂)
Mark scheme (4 marks)
- Iron is less reactive than carbon (so carbon can displace/reduce it)
- The iron ore (iron oxide) is heated with carbon
- Carbon reduces the iron oxide / the iron oxide loses oxygen
- Iron (metal) is produced / carbon is oxidised (gains oxygen to form carbon dioxide or carbon monoxide)
Key terms in this question
reduction with carbon · reduction
Related
- All Edexcel GCSE Chemistry (1CH0) revision notes →
- How to answer a "Explain" question →
- Decode the mark scheme abbreviations →
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