📖 Metallurgy & Reduction▼

Reduction Process

Reduction is the removal of oxygen from a compound. In metallurgy, metal oxides (ores) are reduced to obtain the pure metal using reducing agents like Carbon (C), Hydrogen (H₂), or Carbon Monoxide (CO).

  • Less Reactive Metals (Cu, Pb, Fe) can be reduced by Carbon/CO.
  • Highly Reactive Metals (Na, K, Al) require electrolytic reduction.
EquationObservation
2CuO + C → 2Cu + CO₂Black CuO turns to Reddish-brown Cu
2PbO + C → 2Pb + CO₂Yellow PbO yields Silvery-grey Pb globule
Fe₂O₃ + 3CO → 2Fe + 3CO₂Red-brown ore turns to Grey Iron

Select Metal Oxide

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Action

⚠️ Safety

  • Strongly heated crucible, burner flame and residue are extremely hot — use tongs and let apparatus cool before handling.
  • Lead(II) oxide and lead are toxic; avoid skin contact and inhaling dust or fumes.
  • Reduction of Fe₂O₃ uses carbon monoxide (CO), a colourless, odourless, poisonous gas — work in a fume cupboard.
  • CO₂ and CO evolved should be vented; keep the area well ventilated.
  • Tie back hair, wear goggles, and keep flammables away from the open flame.
2CuO + C → 2Cu + CO₂↑
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