Calcium carbide
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| Calcium carbide | |
|---|---|
| Image:Cac2.jpg | |
| General | |
| Systematic name | Calcium Carbide |
| Other names | |
| Molecular formula | CaC2 |
| Molar mass | 64.1 g/mol |
| Appearance | gray-black Crystals |
| Crystal Structure | orthorhombic |
| CAS number | 75-20-7 |
| Properties | |
| Density and phase | 2.22 g/cm3 |
| Melting point | 2300 °C |
| Boiling point | |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references | |
Calcium carbide (is a chemical compound with the chemical formula Ca{{#if:{{{1|}}}|{{{1}}}|}}C{{#if:{{{1|}}}|{{{1}}}|}}2. It has the appearance of grayish white lumps.
Calcium carbide is produced by electric discharge through a mixture of lime and carbon at high temperature. The compound reacts vigorously with water to form acetylene. This reaction is the basis of the industrial manufacture of dissolved acetylene (DA), and the only modern industrial use for calcium carbide.
Calcium carbide is used in carbide lamps, in which water drips on carbide and the formed acetylene is ignited. The lamps found extensive use in coal mines, but most have now been replaced by electric lamps. Carbide lamps are still used by many spelunkers exploring caves and other underground areas.
It is still used in the Netherlands and Belgium for a traditional custom called Carbidschieten (Shooting Carbid).
The equation for calcium carbide's reaction with water is:
- CaC2 + 2 H2O → C2H2 + Ca(OH)2
Therefore, 1 gram of CaC2 gives 349ml of acetylene.
Together with calcium phosphide, calcium carbide is used in floating, self-igniting naval signal flares.de:Kalziumcarbid es:Carburo de calcio hu:Kalcium-karbid id:Karbit nl:Calciumcarbide ru:Карбид кальция