Extraction of Iron From Hematite (CIE IGCSE Chemistry: Co-ordinated Sciences (Double Award))

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Extraction of iron from hematite

  • Iron is extracted in a large container called a blast furnace from its ore, hematite 
  • Modern blast furnaces produce approximately 10,000 tonnes of iron per day 

The blast furnace

Carbon Extraction of Iron, downloadable AS & A Level Chemistry revision notes

Diagram showing the carbon extraction of iron

  • The raw materials: iron ore (hematite), coke (an impure form of carbon), and limestone are added into the top of the blast furnace
  • Hot air is blown into the bottom

Zone 1

  • Coke burns in the hot air forming carbon dioxide 
  • The reaction is exothermic so it gives off heat, heating the furnace

carbon + oxygen → carbon dioxide

Zone 2

  • At the high temperatures in the furnace, more coke reacts with carbon dioxide forming carbon monoxide
  • Carbon dioxide has been reduced to carbon monoxide

carbon + carbon dioxide → carbon monoxide

Zone 3

  • Carbon monoxide reduces the iron(III) oxide in the iron ore to form iron 
  • This will melt and collect at the bottom of the furnace, where it is tapped off

iron(III) oxide + carbon monoxide  →  iron + carbon dioxide

  • Limestone (calcium carbonate) is added to the furnace to remove impurities in the ore
    • The calcium carbonate in the limestone thermally decomposes to form calcium oxide

calcium carbonate → calcium oxide + carbon dioxide

  • The calcium oxide formed reacts with the silicon dioxide, which is an impurity in the iron ore, to form calcium silicate
  • This melts and collects as a molten slag floating on top of the molten iron, which is tapped off separately

calcium oxide + silicon dioxide →  calcium silicate

Examiner Tip

For Core students, the symbol equations are not needed for the different reactions involved in the extraction of iron from hematite.

Equations for extraction of iron from hematite

Extended tier only

Zone 1

  • The burning of carbon (coke) to provide heat and produce carbon dioxide:

C (s)  +  O2 (g)  →  CO2 (g)

Zone 2

  • The reduction of carbon dioxide to carbon monoxide:

CO2 (g)  +  C (s)  →  2CO (g)

Zone 3

  • The reduction of iron(III) oxide by carbon monoxide:

Fe2O3 (s)  +  3CO (g)  →  2Fe (I)  +  3CO2 (g)

  • The thermal decomposition of calcium carbonate (limestone) to produce calcium oxide:

CaCO3 (s)  →  CaO (s)  +  CO2 (g)

  • The formation of slag:

CaO (s)  +  SiO2 (s)  →  CaSiO3 (l)

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Caroline

Author: Caroline

Expertise: Physics Lead

Caroline graduated from the University of Nottingham with a degree in Chemistry and Molecular Physics. She spent several years working as an Industrial Chemist in the automotive industry before retraining to teach. Caroline has over 12 years of experience teaching GCSE and A-level chemistry and physics. She is passionate about creating high-quality resources to help students achieve their full potential.