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, QL
Packaging
25 Kg PP/PE Bags
Calcium oxide (CaO), also known as quicklime or burnt lime, is a highly corrosive and alkaline white crystalline solid at room temperature. Being an inexpensive compound to produce, along with calcium hydroxide, they are important chemicals for numerous industries. Calcium oxide has a melting point of 2570℃ (4658℉) and a boiling point of 2850℃ (5162℉). Calcium oxide dissolves in water to produce calcium hydroxide, an alkaline solution with a chemical formula of Ca(OH)2, also known as hydrated lime.
Calcium oxide is produced by thermal decomposition of calcium carbonate of calcium carbonate materials such as limestone in a lime kiln. The limestone is first mined and then crushed and washed, removing the impurities. The material is heated during calcination or lime burning, releasing carbon dioxide and leaving behind quicklime. This reaction is reversible and quicklime can react with carbon dioxide to convert back to calcium carbonate. Therefore, carbon dioxide is readily removed to prevent the conversion back to calcium carbonate.
Calcium oxide (CaO), also known as quicklime or burnt lime, is a highly corrosive and alkaline white crystalline solid at room temperature. Being an inexpensive compound to produce, along with calcium hydroxide, they are important chemicals for numerous industries. Calcium oxide has a melting point of 2570℃ (4658℉) and a boiling point of 2850℃ (5162℉). Calcium oxide dissolves in water to produce calcium hydroxide, an alkaline solution with a chemical formula of Ca(OH)2, also known as hydrated lime.
Calcium oxide is produced by thermal decomposition of calcium carbonate of calcium carbonate materials such as limestone in a lime kiln. The limestone is first mined and then crushed and washed, removing the impurities. The material is heated during calcination or lime burning, releasing carbon dioxide and leaving behind quicklime. This reaction is reversible and quicklime can react with carbon dioxide to convert back to calcium carbonate. Therefore, carbon dioxide is readily removed to prevent the conversion back to calcium carbonate.
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