During the industrial extraction of iron in a blast furnace, hematite (Fe_2O_3) is reduced… — JAMB UTME

During the industrial extraction of iron in a blast furnace, hematite ( $Fe_2O_3$ ) is reduced to iron in the upper region of the furnace. Which chemical species acts as the primary reducing agent in this upper zone?

Carbon(II) oxide ( $CO$ )Answer
B
Solid carbon ( $C$ )
C
Calcium oxide ( $CaO$ )
D
Carbon(IV) oxide ( $CO_2$ )

Answer

Carbon(II) oxide (

CO

)

In the blast furnace, carbon(II) oxide (

CO

) gas is produced when hot carbon dioxide reacts with excess coke. Rising

CO

gas encounters descending hematite (

Fe_2O_3

) in the upper, cooler zone of the furnace and reduces it to iron:

Fe_2O_3(s) + 3CO(g) \rightarrow 2Fe(s) + 3CO_2(g)

Step-by-Step Solution

Identify the chemical reactions occurring in the upper region of the blast furnace.

Near the top of the furnace (200°C–700°C), carbon(II) oxide gas reacts with descending hematite ore.

Gas-solid contact allows

CO

to easily reduce the porous iron ore.

Write the overall reduction equation.

Fe_2O_3(s) + 3CO(g) \rightarrow 2Fe(s) + 3CO_2(g)

This chemical equation confirms that

CO

gains oxygen (is oxidized) while reducing

Fe_2O_3

to metallic iron.

Key Concept

Role of gaseous carbon(II) oxide as the principal reducing agent in blast furnace iron extraction

Estimated Time:45s

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