IUPAC Name
Oxocalcium
Cas Number
1305-78-8
HS Code
2522.10.00
Formula
CaO
Appearance
White or Grayish-White Lumps or Powder
Common Names
Lime, Hi-Cal Quicklime, Calcium Oxide, Burnt Lime,
Packaging
25 Kg PP/PE Bags
Calcium oxide, commonly referred to as quicklime or burnt lime, is a highly caustic and alkaline white crystalline solid when at room temperature. It holds significance across various industries alongside calcium hydroxide due to its cost-effective production. With a melting point at 2570°C (4658°F) and a boiling point at 2850°C (5162°F), calcium oxide readily dissolves in water, forming calcium hydroxide—an alkaline solution recognized as hydrated lime, with the chemical formula Ca(OH)2.
Calcium oxide is generated through the thermal breakdown of calcium carbonate materials, like limestone, within a lime kiln. Initially, limestone undergoes mining, followed by crushing and washing to eliminate impurities. Through calcination or lime burning, the material is heated, causing the release of carbon dioxide and the formation of quicklime. This process is reversible, as quicklime can react with carbon dioxide, reverting to calcium carbonate. To prevent this reversal, carbon dioxide is efficiently extracted, ensuring the prevention of reconversion to calcium carbonate.
Calcium oxide, commonly referred to as quicklime or burnt lime, is a highly caustic and alkaline white crystalline solid when at room temperature. It holds significance across various industries alongside calcium hydroxide due to its cost-effective production. With a melting point at 2570°C (4658°F) and a boiling point at 2850°C (5162°F), calcium oxide readily dissolves in water, forming calcium hydroxide—an alkaline solution recognized as hydrated lime, with the chemical formula Ca(OH)2.
Calcium oxide is generated through the thermal breakdown of calcium carbonate materials, like limestone, within a lime kiln. Initially, limestone undergoes mining, followed by crushing and washing to eliminate impurities. Through calcination or lime burning, the material is heated, causing the release of carbon dioxide and the formation of quicklime. This process is reversible, as quicklime can react with carbon dioxide, reverting to calcium carbonate. To prevent this reversal, carbon dioxide is efficiently extracted, ensuring the prevention of reconversion to calcium carbonate.
