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| Calcium oxide | |
|---|---|
| General | |
| Systematic name | Calcium oxide |
| Molecular formula | CaO |
| Molar mass | 56.1 g/mol |
| Appearance | White solid |
| Properties | |
| Density and phase | 3350 kg/m3, solid |
| Solubility in water | reacts |
| Melting point | 2572 °C (2845 K) |
| Boiling point | 2850 °C (3123 K) |
| Structure | |
| Crystal structure | Face-Centered Cubic |
| Thermochemistry | |
| ΔfH0gas | 43.93 kJ/mol |
| ΔfH0liquid | −557.33 kJ/mol |
| ΔfH0solid | −635.09 kJ/mol |
| S0gas, 1 bar | 219.71 J/mol·K |
| S0liquid, 1 bar | 62.31 J/mol·K |
| S0solid | 38.19 J/mol·K |
| Hazards | |
| MSDS | External MSDS |
| NFPA 704 | |
| Supplementary data page | |
| Structure and properties | n, εr, etc. |
| Thermodynamic data | Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Chemical infobox | |
Calcium oxide (CaO), commonly known as lime, quicklime or burnt lime, is a widely used chemical compound. It is a white, caustic and alkaline crystalline solid. As a commercial product lime often also contains magnesium oxide, silicon oxide and smaller amounts of aluminium oxide and iron oxide.
Calcium oxide is usually made by the thermal decomposition of materials, such as limestone, that contain calcium carbonate (CaCO3; mineral name: calcite). This is accomplished by heating the material to around 900°C (American Scientist), a process called calcination or lime-burning, so as to remove the carbon dioxide in a non-reversible chemical reaction. Lower temperatures would result in a reversible reaction, allowing the calcium carbonate to reabsorb the surrounding carbon dioxide. This is one of the first chemical reactions discovered by man and was known in prehistory: see limekiln.
As hydrated or slaked lime, Ca(OH)2 (mineral name: portlandite), it was used in mortar and plaster to increase the rate of hardening. Hydrated lime is very simple to make as lime is a basic anhydride and reacts vigorously with water. Lime was also used in glass production and its ability to work with silicates is also used in modern metal production (steel, magnesium, aluminium and other non-ferrous metals) industries to remove impurities as slag.
It is also used in water and sewage treatment to reduce acidity, to soften, as a flocculant and to remove phosphates and other impurities; in paper making to dissolve lignin, as a coagulant and in bleaching; in agriculture to improve acidic soils; and in pollution control - in gas scrubbers to desulfurize waste gases and to treat many liquid effluents. It is a refactory and a dehydrating agent and is used to purify citric acid, glucose, dyes and as a CO2 absorber. It is also used in pottery, concrete, paints and the food industry, where it is sometimes used (in conjunction with water) to heat items like MREs (Meals Ready To Eat) and coffee.
See also
External link
Oxides | Calcium compounds | Bases | Limestone
Kalciumoxid | Kalziumoxid | Kaltsiumoksiid | Óxido de calcio | Kalko | Chaux (chimie) | סיד | Kalcio oksidas | Calciumoxide | 酸化カルシウム | Tlenek wapnia | Óxido de cálcio | Оксид кальция | Kalciumoxid | Ôxít canxi | Оксид кальцію | 氧化鈣
"Calcium oxide"