Calcium oxide
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| Names |
| IUPAC name
Calcium oxide
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| Other names
Quicklime, burnt lime, unslaked lime, pebble lime
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| Identifiers |
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CAS Number
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1305-78-8 N |
| ChemSpider |
14095 |
| Jmol interactive 3D |
Image |
| PubChem |
14778 |
| RTECS number |
EW3100000 |
| UNII |
C7X2M0VVNH |
| UN number |
1910 |
InChI
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InChI=1/Ca.O/rCaO/c1-2
Key: ODINCKMPIJJUCX-BFMVISLHAU
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| Properties |
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Chemical formula
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CaO |
| Molar mass |
56.0774 g/mol |
| Appearance |
White to pale yellow/brown powder |
| Odor |
Odorless |
| Density |
3.34 g/cm3[1] |
| Melting point |
2,613 °C (4,735 °F; 2,886 K)[1] |
| Boiling point |
3,850 °C (6,960 °F; 4,120 K) (100 hPa)[2] |
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Solubility in water
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Reacts to form calcium hydroxide |
| Solubility in Methanol |
Insoluble (also in diethyl ether, n-octanol) |
| Acidity (pKa) |
12.8 |
| Structure |
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Crystal structure
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NaCl |
| Thermochemistry |
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Std molar
entropy (So298)
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40 J·mol−1·K−1[3] |
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Std enthalpy of
formation (ΔfHo298)
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−635 kJ·mol−1[3] |
| Pharmacology |
| ATCvet code |
QP53AX18 |
| Hazards |
| Safety data sheet |
Hazard.com |
| NFPA 704 |
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| Flash point |
Non-flammable [4] |
| US health exposure limits (NIOSH): |
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PEL (Permissible)
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TWA 5 mg/m3[4] |
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REL (Recommended)
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TWA 2 mg/m3[4] |
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IDLH (Immediate danger
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25 mg/m3[4] |
| Related compounds |
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Other anions
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Calcium sulfide
Calcium hydroxide |
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Other cations
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Beryllium oxide
Magnesium oxide
Strontium oxide
Barium oxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references |
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Calcium oxide (CaO), commonly known as quicklime or burnt lime, is a widely used chemical compound. It is a white, caustic, alkaline, crystalline solid at room temperature. The broadly used term "lime" connotes calcium-containing inorganic materials, in which carbonates, oxides and hydroxides of calcium, silicon, magnesium, aluminium, and iron predominate. By contrast, "quicklime" specifically applies to the single chemical compound calcium oxide. Calcium oxide which survives processing without reacting in building products such as cement is called free lime.[5]
Quicklime is relatively inexpensive. Both it and a chemical derivative (calcium hydroxide, of which quicklime is the base anhydride) are important commodity chemicals.
Contents
- 1 Preparation
- 2 Usage
- 3 Health issues
- 4 References
- 5 External links
PreparationEdit
Calcium oxide is usually made by the thermal decomposition of materials such as limestone, or seashells, that contain calcium carbonate (CaCO3; mineral calcite) in a lime kiln. This is accomplished by heating the material to above 825 °C (1,517 °F),[6] a process called calcination or lime-burning, to liberate a molecule of carbon dioxide (CO2); leaving quicklime.
- CaCO3(s) → CaO(s) + CO2(g)
The quicklime is not stable and, when cooled, will spontaneously react with CO2 from the air until, after enough time, it will be completely converted back to calcium carbonate unless slaked with water to set as lime plaster or lime mortar.
Annual worldwide production of quicklime is around 283 million metric tons. China is by far the world's largest producer, with a total of around 170 million tonnes per year. The United States is the next largest, with around 20 million tonnes per year.[7]
UsageEdit
- Heat: Quicklime releases Thermal energy by the formation of the hydrate, calcium hydroxide, by the following equation:[8]
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- CaO (s) + H2O (l) Ca(OH)2 (aq) (ΔHr = −63.7 kJ/mol of CaO)
- As it hydrates, an exothermic reaction results and the solid puffs up. The hydrate can be reconverted to quicklime by removing the water by heating it to redness to reverse the hydration reaction. One litre of water combines with approximately 3.1 kilograms (6.8 lb) of quicklime to give calcium hydroxide plus 3.54 MJ 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.
- Light: When quicklime is heated to 2,400 °C (4,350 °F), it emits an intense glow. This form of illumination is known as a limelight, and was used broadly in theatrical productions prior to the invention of electric lighting.[9]
- Cement: Calcium oxide is a key ingredient for the process of making cement.
- As an alkali in biodiesel production[10][11]
- Petroleum industry: Water detection pastes contain a mix of calcium oxide and phenolphthalein. Should this paste come into contact with water in a fuel storage tank, the CaO reacts with the water to form calcium hydroxide. Calcium hydroxide has a high enough pH to turn the phenolphthalein a vivid purplish-pink color, thus indicating the presence of water.
- Paper: Calcium oxide is used to regenerate sodium hydroxide from sodium carbonate in the chemical recovery at Kraft pulp mills.
- Plaster: There is archeological evidence that Pre-Pottery Neolithic B humans used limestone-based plaster for flooring and other uses.[12][13][14] Such Lime-ash floor remained in use until the late nineteenth century.
- Chemical or power production: Solid sprays or slurries of calcium oxide can be used to remove sulfur dioxide from exhaust streams in a process called flue-gas desulfurization.
Use as a weaponEdit
Historian and philosopher David Hume, in his history of England, recounts that early in the reign of Henry III, the English Navy destroyed an invading French fleet by blinding the enemy fleet with quicklime:
D’Albiney employed a stratagem against them, which is said to have contributed to the victory: Having gained the wind of the French, he came down upon them with violence; and throwing in their faces a great quantity of quicklime, which he purposely carried on board, he so blinded them, that they were disabled from defending themselves.[15]
Quicklime is also thought to have been a component of Greek fire. Upon contact with water, quicklime would increase its temperature above 150 °C and ignite the fuel.[16]
Health issuesEdit
Because of vigorous reaction of quicklime with water, quicklime causes severe irritation when inhaled or placed in contact with moist skin or eyes. Inhalation may cause coughing, sneezing, labored breathing. It may then evolve into burns with perforation of the nasal septum, abdominal pain, nausea and vomiting. Although quicklime is not considered a fire hazard, its reaction with water can release enough heat to ignite combustible materials.[17]
ReferencesEdit
- ^ a b Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.55. ISBN 1439855110.
- ^ Calciumoxid. GESTIS database
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A21. ISBN 0-618-94690-X.
- ^ a b c d "NIOSH Pocket Guide to Chemical Hazards #0093". National Institute for Occupational Safety and Health (NIOSH).
- ^ "free lime". DictionaryOfConstruction.com.
- ^ Merck Index of chemicals and Drugs , 9th edition monograph 1650
- ^ Miller, M. Michael (2007). "Lime". Minerals Yearbook (PDF). U.S. Geological Survey. p. 43.13.
- ^ Collie, Robert L. "Solar heating system" U.S. Patent 3,955,554 issued May 11, 1976
- ^ Gray, Theodore (September 2007). "Limelight in the Limelight". Popular Science: 84.
- ^ Kouzu, M.; Kasuno, T.; Tajika, M.; Sugimoto, Y.; Yamanaka, S.; Hidaka, J. (2008). "Calcium oxide as a solid base catalyst for transesterification of soybean oil and its application to biodiesel production". Fuel 87 (12): 2798. doi:10.1016/j.fuel.2007.10.019.
- ^ Zhu, H.; Wu, Z.; Chen, Y.; Zhang, P.; Duan, S.; Liu, X.; Mao, Z. (2006). "Preparation of Biodiesel Catalyzed by Solid Super Base of Calcium Oxide and Its Refining Process". Chinese Journal of Catalysis 27 (5): 391. doi:10.1016/S1872-2067(06)60024-7.
- ^ Neolithic man: The first lumberjack?. Phys.org (August 9, 2012). Retrieved on 2013-01-22.
- ^ Karkanas, P.; Stratouli, G. (2011). "Neolithic Lime Plastered Floors in Drakaina Cave, Kephalonia Island, Western Greece: Evidence of the Significance of the Site". The Annual of the British School at Athens 103: 27. doi:10.1017/S006824540000006X.
- ^ Connelly, Ashley Nicole (May 2012) Analysis and Interpretation of Neolithic Near Eastern Mortuary Rituals from a Community-Based Perspective. Baylor University Thesis, Texas
- ^ David Hume (1756). History of England I.
- ^ Croddy, Eric (2002). Chemical and biological warfare: a comprehensive survey for the concerned citizen. Springer. p. 128. ISBN 0-387-95076-1.
- ^ CaO MSDS. hazard.com
External linksEdit
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Wikimedia Commons has media related to Calcium oxide. |
- Lime Statistics & Information from the United States Geological Survey
- Factors Affecting the Quality of Quicklime
- American Scientist (discussion of 14C dating of mortar)
- Chemical of the Week – Lime
- Material Safety Data Sheet
- CDC - NIOSH Pocket Guide to Chemical Hazards
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Calcium compounds
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- CaAl2O4
- CaB6
- CaBr2
- Ca(BrO3)2
- CaC2
- CaCN2
- Ca(CN)2
- CaCO3
- CaC2O4
- CaCl2
- Ca(ClO)2
- Ca(ClO3)2
- CaCrO4
- CaF2
- CaH2
- Ca(HCO3)2
- CaH2S2O6
- CaI2
- Ca(IO3)2
- Ca(MnO4)2
- CaN6
- Ca(NO3)2
- CaO
- CaO2
- Ca(OH)2
- CaP
- CaS
- CaSO3
- CaSO4
- CaSi2
- CaTiO3
- Ca2P2O7
- Ca2SiO4
- Ca3Al2O6
- Ca3(AsO4)2
- Ca3(BO3)2
- Ca3(C6H5O7)2
- Ca3N2
- Ca3P2
- Ca4(PO4)2O
- Ca3(PO4)2
- Ca(H2PO4)2
- CaHPO4
- C36H70CaO4
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