CALCIUM OXIDE


Calcium oxide
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)

'Calcium oxide' ('CaO'), commonly known as 'burnt lime', 'caustic lime', 'lime' or 'quicklime', 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) in a lime kiln. This is accomplished by heating the material to above 825°C,[1] a process called calcination or ''lime-burning'', to liberate a molecule of carbon dioxide(CO2); leaving CaO. This process is reversible, since once the quicklime product has cooled, it immediately begins to absorb carbon dioxide from the air, until, after enough time, it is completely converted back to calcium carbonate. Calcination of limestone is one of the first chemical reactions discovered by man and was known in prehistory.

Contents
Usage
See also
External links
References

Usage


As hydrated or slaked lime, Ca(OH)2 (mineral name: portlandite), it is 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 is also used in glass production and its ability to react 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 has traditionally been used in the burial of bodies in open graves, to hide the smell of decomposition, as well as in forensic science, to reveal fingerprints. It is a refractory and a dehydrating agent and is used to purify citric acid, glucose, dyes and as a CO2 absorber. It is also used in pottery, paints and the food industry. Furthermore, quicklime is used in epidemics, plagues, and disasters to disintegrate bodies in order to help fight the spread of disease. CaO is a key ingredient in the ''nixtamalization'' process used to create corn hominy and masa or tortilla dough.
A relatively inexpensive substance, CaO produces heat energy by the formation of the hydrate, as in the following equation:[2]
::CaO + H2O ↔ Ca(OH)2 + 488 BTU/lb of CaO
The hydrate can be reconverted to calcium oxide by removing the water in the reversible equation. If the hydrated lime is heated to redness, the CaO will be regenerated to reverse the reaction. As it hydrates, an exothermic reaction results. One pound of water combines with approximately 3 1/9 pounds of calcium oxide to give calcium hydroxide plus 1618 BTU's of energy. This process can be used to provide a convenient portable source of heat, as for on-the-spot food warming in a self-heating can.
World lime annual production is around 130 million tonnes, with the USA and China the largest producers, each producing around 20 million tonnes.[1]

See also



★ Calcium hydroxide

★ Common chemicals

★ Limelight

★ Magnesium oxide

External links



★ An authoritative discussion of lime and its uses (US context) by the US Geological Survey

★ Factors Affecting the Quality of Quicklime

★ ''American Scientist'' (discussion of 14C dating of mortar)

References


1. Merck Index of chemicals and Drugs , 9th ed. monograph 1650
2. US Patent 3,955,554, '' Solar heating system.''


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