MCQ Detailed View

Iron extraction in a blast furnace is a key process in metallurgy and inorganic chemistry. In the furnace, iron ore (Fe₂O₃) is converted into molten iron through a series of chemical reactions. At temperatures between 400°C and 600°C, the reduction of hematite (Fe₂O₃) by carbon monoxide (CO) takes place. The reaction is:

Fe₂O₃ + 3CO → 2Fe + 3CO₂

In this reaction, CO acts as a reducing agent, removing oxygen from the iron oxide to produce metallic iron. The carbon monoxide itself is generated in the furnace by partial combustion of coke (C):

2C + O₂ → 2CO

Other reactions occurring in the blast furnace include the formation of slag, such as:

CaO + SiO₂ → CaSiO₃,

which removes impurities like silica, but this is not the main reaction producing iron.

The reduction of Fe₂O₃ is critical because it directly produces molten iron, which collects at the bottom of the furnace. The reaction is temperature-dependent, occurring efficiently in the 400°C–600°C range, and demonstrates the principle of reduction in metallurgy, where a less reactive substance (CO) reduces a more stable compound (Fe₂O₃).

Understanding this reaction helps students connect concepts of oxidation-reduction, blast furnace operation, and extraction of metals. It also illustrates practical applications in steel production, chemical engineering, and industrial chemistry.

The correct reaction highlights the role of CO as a reducing agent and shows the conversion of iron ore into elemental iron, a fundamental concept in inorganic chemistry and metallurgy.