In the manufacture of iron, a mixture of limestone, coke, and iron ore is added to the blast furnace. In this context give the equation for the reduction of the iron ore.

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Solution

The reduction of Haematite or Iron oxide $(F e_{2} O_{3})$ in blast furnace is done with coke and limestone or Calcium carbonate $({CaCO}_{3})$ .
Coke is burned to red hot coke where reduction of Carbon dioxide $(C O_{2})$ takes place.
The actual reducing agent is Carbon monoxide $(C O)$ formed from Carbon dioxide $(C O_{2})$ .
The reactions involved are:
$C (s) + O_{2} \overset{∆}{(g) \to} C O_{2} (g) C a r b o n O x y g e n C a r b o n d i o x i d e C O_{2} (g) + C (s) \to 2 C O (g) C a r b o n d i o x i d e C a r b o n C a r b o n m o n o x i d e F e_{2} O_{3} (s) + 3 C O (g) \to 2 F e (s) + 3 C O_{2} (g) I r o n o x i d e C a r b o n m o n o x i d e I r o n C a r b o n d i o x i d e$

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In the manufacture of iron, a mixture of limestone, coke, and iron ore is added to the blast furnace.

In this context,

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(iv) Write the chemical equation for the formation of the substance named in (iii) above.

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