Calcium oxide

Source: Wikipedia, the free encyclopedia.
Calcium oxide
Calcium oxide
Ionic crystal structure of calcium oxide
  Ca2+   O2-

Powder sample of white calcium oxide
Names
IUPAC name
Calcium oxide
Other names
  • Lime
  • Quicklime
  • Burnt lime
  • Unslaked lime
  • Free lime (building)
  • Caustic lime
  • Pebble lime
  • Calcia
  • Oxide of calcium
Identifiers
3D model (
JSmol
)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard
 100.013.763 Edit this at Wikidata
EC Number
  • 215-138-9
E number E529 (acidity regulators, ...)
485425
KEGG
RTECS number
  • EW3100000
UNII
UN number 1910
  • InChI=1S/Ca.O
    Key: ODINCKMPIJJUCX-UHFFFAOYSA-N
  • InChI=1/Ca.O/rCaO/c1-2
    Key: ODINCKMPIJJUCX-BFMVISLHAU
  • O=[Ca]
Properties
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 2,850 °C (5,160 °F; 3,120 K) (100 
hPa)[2]
Reacts to form calcium hydroxide
Solubility in Methanol Insoluble (also in diethyl ether, octanol)
Acidity (pKa) 12.8
−15.0×10−6 cm3/mol
Structure
Cubic, cF8
Thermochemistry
40 J·mol−1·K−1[3]
Std enthalpy of
formation
(ΔfH⦵298)
 −635 kJ·mol−1[3]
Pharmacology
QP53AX18 (WHO
)
Hazards
GHS labelling:
GHS05: CorrosiveGHS07: Exclamation mark
Danger
H302, H314, H315, H335
P260, P261, P264, P270, P271, P280, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P340, P305+P351+P338, P310, P312, P321, P330, P332+P313, P362, P363, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
3
0
2
W
Flash point Non-flammable[4]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 5 mg/m3[4]
REL (Recommended)
 TWA 2 mg/m3[4]
IDLH
(Immediate danger)
 25 mg/m3[4]
Safety data sheet (SDS) ICSC 0409
Related compounds
Other anions
 Calcium sulfide
Calcium hydroxide
Calcium selenide
Calcium telluride
Other cations
 Beryllium oxide
Magnesium oxide
Strontium oxide
Barium oxide
Radium oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
See also: Lime (material)

Calcium oxide (

caustic, alkaline, crystalline solid at room temperature. The broadly used term lime connotes calcium-containing inorganic compounds, in which carbonates, oxides, and hydroxides of calcium, silicon, magnesium, aluminium, and iron predominate. By contrast, quicklime specifically applies to the single compound calcium oxide. Calcium oxide that survives processing without reacting in building products, such as cement, is called free lime.[5]

Quicklime is relatively inexpensive. Both it and the chemical derivative calcium hydroxide (of which quicklime is the base anhydride) are important commodity chemicals.

Preparation

Calcium oxide is usually made by the

prehistoric times.[8]

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 tonnes. 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.[9]

Approximately 1.8 t of limestone is required per 1.0 t of quicklime. Quicklime has a high affinity for water and is a more efficient desiccant than silica gel. The reaction of quicklime with water is associated with an increase in volume by a factor of at least 2.5.[10]

Uses

A demonstration of slaking of quicklime as a strongly exothermic reaction. Drops of water are added to pieces of quicklime. After a while, a pronounced
exothermic
reaction occurs ('slaking of lime'). The temperature can reach up to some 300 °C (572 °F).
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 
self-heating can, cooking, and heating water without open flames. Several companies sell cooking kits using this heating method.[12]
  • It is known as a
    FAO as an acidity regulator, a flour treatment agent and as a leavener.[13] It has E number
    E529.
  • 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 before the invention of electric lighting.[14]
  • Cement: Calcium oxide is a key ingredient for the process of making cement.
  • As a cheap and widely available alkali. About 50% of the total quicklime production is converted to
    hydrated lime are used in the treatment of drinking water.[10]
  • 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.[15][16][17] 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.
  • Carbon capture and storage: Calcium oxide can be used to capture carbon dioxide from flue gases in a process called calcium looping.
  • Mining: Compressed lime cartridges exploit the exothermic properties of quicklime to break rock. A shot hole is drilled into the rock in the usual way and a sealed cartridge of quicklime is placed within and tamped. A quantity of water is then injected into the cartridge and the resulting release of steam, together with the greater volume of the residual hydrated solid, breaks the rock apart. The method does not work if the rock is particularly hard.[18][19][20]
  • Disposal of corpses: Historically, it was mistakenly believed that quicklime was efficacious in accelerating the decomposition of corpses. The application of quicklime can, in fact, promote preservation. Quicklime can aid in eradicating the stench of decomposition, which may have led people to the erroneous conclusion.[21]
  • It has been determined that the durability of ancient Roman concrete is attributed in part to the use of quicklime as an ingredient. Combined with hot mixing, the quicklime creates macrosized lime clasts with a characteristically brittle nano-particle architecture. As cracks form in the concrete they preferentially pass through the structurally weaker lime clasts, fracturing them. When water enters these cracks it creates a calcium-saturated solution which can recrystallize as calcium carbonate, quickly filling the crack. [22]

Weapon

In 80 BC, the Roman general

Sertorius deployed choking clouds of caustic lime powder to defeat the Characitani of Hispania, who had taken refuge in inaccessible caves.[23] A similar dust was used in China to quell an armed peasant revolt in 178 AD, when lime chariots equipped with bellows blew limestone powder into the crowds.[24]

Quicklime is also thought to have been a component of Greek fire. Upon contact with water, quicklime would increase its temperature above 150 °C (302 °F) and ignite the fuel.[25]

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.[26] Quicklime may have been used in medieval naval warfare – up to the use of "lime-mortars" to throw it at the enemy ships.[27]

Substitutes

Limestone is a substitute for lime in many applications, which include agriculture, fluxing, and sulfur removal. Limestone, which contains less reactive material, is slower to react and may have other disadvantages compared with lime, depending on the application; however, limestone is considerably less expensive than lime. Calcined gypsum is an alternative material in industrial plasters and mortars. Cement, cement kiln dust, fly ash, and lime kiln dust are potential substitutes for some construction uses of lime. Magnesium hydroxide is a substitute for lime in pH control, and magnesium oxide is a substitute for dolomitic lime as a flux in steelmaking.[28]

Safety

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, and 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.

better source needed
]

Mineral

Calcium oxide is also a separate mineral species (with the unit formula CaO), named 'Lime'.[30][31] It has an isometric crystal system, and can form a solid solution series with monteponite. The crystal is brittle, pyrometamorphic, and is unstable in moist air, quickly turning into portlandite (Ca(OH)2).[32]

References

  1. ^
    ISBN 1-4398-5511-0
    .
  2. ^ Calciumoxid Archived 2013-12-30 at the Wayback Machine. GESTIS database
  3. ^
    ISBN 978-0-618-94690-7
    .
  4. ^ a b c d NIOSH Pocket Guide to Chemical Hazards. "#0093". National Institute for Occupational Safety and Health (NIOSH).
  5. ^ "free lime". DictionaryOfConstruction.com. Archived from the original on 2017-12-09.
  6. ^ Merck Index of Chemicals and Drugs, 9th edition monograph 1650
  7. ISBN 978-1-58829-860-7
    , retrieved 2022-07-26
  8. ^ "Lime throughout history | Lhoist - Minerals and lime producer". Lhoist.com. Retrieved 10 March 2022.
  9. U.S. Geological Survey
    . p. 43.13.
  10. ^
    ISBN 978-3527306732
  11. ^ Collie, Robert L. "Solar heating system" U.S. patent 3,955,554 issued May 11, 1976
  12. ^ Gretton, Lel. "Lime power for cooking - medieval pots to 21st century cans". Old & Interesting. Retrieved 13 February 2018.
  13. ^ "Compound Summary for CID 14778 - Calcium Oxide". PubChem.
  14. ^ Gray, Theodore (September 2007). "Limelight in the Limelight". Popular Science: 84. Archived from the original on 2008-10-13. Retrieved 2009-03-31.
  15. ^ Tel Aviv University (August 9, 2012). "Neolithic man: The first lumberjack?". phys.org. Retrieved 2023-02-02.
  16. S2CID 129562287
    .
  17. ^ Connelly, Ashley Nicole (May 2012) Analysis and Interpretation of Neolithic Near Eastern Mortuary Rituals from a Community-Based Perspective Archived 2015-03-09 at the Wayback Machine. Baylor University Thesis, Texas
  18. ^ Walker, Thomas A (1888). The Severn Tunnel Its Construction and Difficulties. London: Richard Bentley and Son. p. 92.
  19. ^ "Scientific and Industrial Notes". Manchester Times. Manchester, England: 8. 13 May 1882.
  20. ^ US Patent 255042, 14 March 1882
  21. PMID 22030481
    .
  22. ^ "Riddle solved: Why was Roman concrete so durable?", MIT News, January 6, 2023
  23. ^ Plutarch, "Sertorius 17.1–7", Parallel Lives
  24. ISBN 0-12-745354-7
  25. ISBN 0-387-95076-1
    .
  26. ^ David Hume (1756). History of England. Vol. I.
  27. ^ Sayers, W. (2006). "The Use of Quicklime in Medieval Naval Warfare". The Mariner's Mirror. Volume 92. Issue 3. pp. 262–269.
  28. ^ "Lime" (PDF). Prd-wret.s3-us-west-2.amazonaws.com. p. 96. Archived from the original (PDF) on 2021-12-19. Retrieved 2022-03-10.
  29. ^ Mallinckrodt Baker Inc. - Strategic Services Division (December 8, 1996). "Hazards". ww25.hazard.com. Archived from the original on May 1, 2012. Retrieved 2023-02-02.{{cite web}}: CS1 maint: unfit URL (link)
  30. ^ "List of Minerals". Ima-mineralogy.org. 21 March 2011.
  31. S2CID 93706828
    . Retrieved 9 February 2023.
  32. ^ "Lime". Mindat.org. Retrieved 10 March 2022.

External links

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