Describe the extraction of iron from hematite in the blast furnace, limited to: (a) the burning of carbon (coke) to provide heat and produce carbon dioxide (b) the reduction of carbon dioxide to carbon monoxide (c) the reduction of iron(III) oxide by

Metals – Extraction of Iron from Hematite in the Blast Furnace

1️⃣ Burning of Carbon (Coke) to Provide Heat and Produce CO₂

The blast furnace is like a giant cooking pot where we heat things up until they change. First, we burn coke (a coal‑derived carbon) with oxygen from the air. This reaction releases a lot of heat (🔥) and produces carbon dioxide:

\$C + O2 \;\longrightarrow\; CO2\$

2️⃣ Reduction of CO₂ to CO

The hot furnace environment allows the CO₂ to react with more coke, turning it into carbon monoxide, which is a gas that loves to steal oxygen from iron oxides:

\$CO_2 + C \;\longrightarrow\; 2\,CO\$

3️⃣ Reduction of Iron(III) Oxide by CO

Now the CO gas comes into contact with the iron ore (hematite, \$Fe2O3\$). The CO donates oxygen, leaving behind molten iron:

\$Fe2O3 + 3\,CO \;\longrightarrow\; 2\,Fe + 3\,CO_2\$

4️⃣ Thermal Decomposition of Calcium Carbonate (Limestone) to CaO

Limestone (\$CaCO_3\$) is added to the furnace to help remove impurities. At high temperatures it breaks down into calcium oxide (lime) and CO₂:

\$CaCO3 \;\xrightarrow{heat}\; CaO + CO2\$

5️⃣ Formation of Slag

The lime reacts with silica and other impurities in the ore to form a molten slag that floats on top of the molten iron. Think of it as the “clean‑up crew” that carries away unwanted materials:

\$CaO + SiO2 \;\longrightarrow\; CaSiO3\$ (slag)

Summary Table of Key Reactions

Quick Quiz: Which gas is the real “oxygen thief” that helps turn iron ore into liquid iron? 🤔