Blast-furnace equations and oxygen accounting
Balance the five required equations and distinguish redox, decomposition and slag formation.
Cross-referenced from the related Cambridge IGCSE Chemistry 0620 or Physics 0625 teaching to the 0652 syllabus. Exact 0652 Core/Supplement objective coverage and this final-series course’s examiner fit still need specialist review. Written practice is self-checked and does not predict a Cambridge grade or demonstrate supervised laboratory competence.
Before you begin
- Explain all five furnace stages in words.
- Balance equations and apply Extended reacting-mass ratios.
Work on paper. Try each question before revealing help, and explain why your method works.
Quick readiness check
How many iron atoms occur in Fe₂O₃?
What you will learn
- State and balance the five required extraction equations.
- Use them to check oxygen transfer and a supplied theoretical iron calculation.
Match each equation with its purpose
Coke combustion is C+O₂→CO₂. Carbon-monoxide formation is C+CO₂→2CO. Hematite reduction is Fe₂O₃+3CO→2Fe+3CO₂. The third equation shows iron oxide losing oxygen while carbon monoxide gains oxygen; matching oxygen atoms does not require molecular oxygen as a product.
Limestone decomposition is CaCO₃→CaO+CO₂. Slag formation is CaO+SiO₂→CaSiO₃. In the last reaction the basic calcium oxide reacts with acidic silicon dioxide; it is not the equation that produces metallic iron. Balance by coefficients while preserving the correct formulas and distinguish the chemical role of each equation.
Use the reduction ratio with explicit assumptions
One mole of Fe₂O₃ forms two moles of Fe in the balanced reduction. With supplied relative atomic masses Fe=56 and O=16, Fe₂O₃ has formula mass 160 and its iron contribution is 112. Thus a theoretical pure-hematite calculation uses an iron mass factor 112/160=0.70, assuming complete reduction and adequate carbon monoxide.
Ore impurities, incomplete conversion and product losses reduce actual recovery relative to the stated pure theoretical case. Do not use the same mass factor directly on an impure ore without first finding its hematite amount. The equation's three CO molecules per Fe₂O₃ formula unit explain oxygen acceptance; the three is not the number of iron atoms produced.
Sources for this lesson
Pause and explain
Which required equation forms slag?
Worked example
Using Fe=56 and O=16, find the theoretical iron from 160 g pure Fe₂O₃ with sufficient CO and complete reduction.
Show the worked solution
- Fe₂O₃ has molar mass 2×56+3×16=160 g/mol.
- 160 g is 1 mol and gives 2 mol Fe.
- Iron mass is 2×56=112 g under the stated complete-reduction assumptions.
Answer 112 g theoretical iron.
Try a topic test
Choose Easy, Normal or Difficult. Save your answers and open worked review after finishing.
Test this topic →From guided practice to a new situation
Write your answer and reasoning first. Use a hint only if you are stuck. The model solution is for self-checking; your written work is not automatically marked.
Write coke combustion and carbon-monoxide formation equations and state their roles.
Give me a hint
The carbon dioxide formed first is used with further hot carbon.
Compare my reasoning
- C+O₂→CO₂ describes combustion and heat release.
- C+CO₂→2CO describes carbon-monoxide formation.
- CO then serves as the reducing gas for hematite in the separate ore reaction.
C+O₂→CO₂; C+CO₂→2CO; heat first, reducing-gas formation next.
Look for these in your work
- Both equations balance.
- Their separate purposes are stated.
Write the limestone decomposition and slag equations, then explain why neither gives iron metal directly.
Give me a hint
Track calcium-containing substances rather than adding iron from nowhere.
Compare my reasoning
- CaCO₃→CaO+CO₂ is decomposition.
- CaO+SiO₂→CaSiO₃ is slag formation.
- Neither equation contains iron; iron is produced in Fe₂O₃ reduction.
CaCO₃→CaO+CO₂; CaO+SiO₂→CaSiO₃; iron comes from the separate oxide-reduction equation.
Look for these in your work
- All formulas and atoms are correct.
- The roles stay distinct from iron production.
A hypothetical 400 g ore contains 80% Fe₂O₃ by mass. Using Fe=56 and O=16, find theoretical iron assuming complete reduction and sufficient CO, and explain why actual recovery may be smaller.
Give me a hint
Apply purity before the oxide-to-metal mass ratio.
Compare my reasoning
- Pure Fe₂O₃ amount is 400×0.80=320 g.
- Theoretical iron is 320×112/160=224 g.
- Incomplete conversion or product losses can make actual recovered mass smaller than this ideal result.
224 g theoretical iron; actual recovery can be lower through incomplete conversion or losses.
Look for these in your work
- Ore purity is applied first.
- Theoretical and actual recovery are distinguished.
Common mistakes
- Writing CO₂ as the reducing reactant instead of CO in hematite reduction.
- Changing Fe₂O₃ to FeO to balance the required equation.
- Using an impure ore's whole mass as pure hematite.
- Calling every furnace step the same redox equation.
What can you explain now?
Balance the required hematite reduction equation using carbon monoxide.
Compare with the explanation
Fe₂O₃+3CO→2Fe+3CO₂.
Two iron atoms and six total oxygen atoms are conserved on each side; CO receives the oxide's oxygen.
After trying it yourself, choose your next review. This is your self-assessment.
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Make it stick
Write all five equations, balance each and label its purpose. Calculate a new pure-oxide or impure-ore theoretical yield with the assumptions stated.
If you needed the solution, close it and solve the problem again from a blank page. A correct answer is stronger when you can explain the reason for each step.