WordNet

cover with lime so as to induce growth; "lime the lawn"
any of various related trees bearing limes (同)lime tree, Citrus aurantifolia
the green acidic fruit of any of various lime trees
a white metallic element that burns with a brilliant light; the fifth most abundant element in the earths crust; an important component of most plants and animals (同)Ca, atomic number 20
any compound of oxygen with another element or a radical

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石灰 / 鳥もち(birdlime) / …‘に'石灰をまく;…‘を'石灰で処理する / …‘に'鳥もちを塗る;…‘を'鳥もちで捕らえる
ボダイジュ,シナノキ
ライム(レモンに似た酸味の強い果実) / ライムの木
『カルシウム』(金属元素;化学記号は『Ca』)
酸化物

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2016/02/03 11:32:40」(JST)

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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.

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.

CaCO_3(s) → CaO_(s) + CO_2(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]

CaO (s) + H₂O (l) Ca(OH)₂ (aq) (ΔH_r = −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

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

UpToDate Contents

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1. 成人における肺高血圧症の治療 treatment of pulmonary hypertension in adults
2. 思春期におけるカルシウムの所要量 calcium requirements in adolescents
3. 呼気中一酸化窒素の分析および適用 exhaled nitric oxide analysis and applications
4. 骨粗鬆症におけるカルシウムおよびビタミンDの補充 calcium and vitamin d supplementation in osteoporosis
5. カルシウムおよびリン酸バランスの調節 regulation of calcium and phosphate balance

English Journal

Effects of CaCO3 treatment on the morphology, crystallinity, rheology and hydrolysis of gelatinized maize starch dispersions.

Garcia-Diaz S1, Hernandez-Jaimes C2, Escalona-Buendia HB1, Bello-Perez LA3, Vernon-Carter EJ4, Alvarez-Ramirez J4.
Food chemistry.Food Chem.2016 Sep 15;207:139-47. doi: 10.1016/j.foodchem.2016.03.095. Epub 2016 Mar 30.
Using calcium salts instead of lime allows for an ecological nixtamalization of maize grains, where the negative contamination impact of the traditional lime nixtamalization is reduced. This work assessed the effects of calcium carbonate (0.0-2.0%w/w CaCO3) on the morphology, crystallinity, rheology
PMID 27080890

Oxygenated heterocyclic compounds to differentiate Citrus spp. essential oils through metabolomic strategies.

Masson J1, Liberto E2, Beolor JC3, Brevard H3, Bicchi C2, Rubiolo P4.
Food chemistry.Food Chem.2016 Sep 1;206:223-33. doi: 10.1016/j.foodchem.2016.03.057. Epub 2016 Mar 17.
This study aimed to characterise and discriminate 44 authenticated commercial samples of citrus essential oils (EO) from seven species (bergamot, lemon, bigarade, orange, mandarin, grapefruit, lime) by analysing the non-volatile oxygenated heterocyclic compounds (OHC) by UHPLC/TOF-HRMS, multivariate
PMID 27041320

Application of ionic liquids for elution of bioactive flavonoid glycosides from lime fruit by miniaturized matrix solid-phase dispersion.

Xu JJ1, Yang R2, Ye LH3, Cao J4, Cao W1, Hu SS1, Peng LQ1.
Food chemistry.Food Chem.2016 Aug 1;204:167-75. doi: 10.1016/j.foodchem.2016.02.012. Epub 2016 Feb 12.
In this work, two flavonoid glycosides (neohesperidin and naringin) in lime fruit were effectively extracted by miniaturized matrix solid phase dispersion (MSPD), followed by ultra-performance liquid chromatography-ultraviolet detection. The best results were obtained using Florisil (150mg) as the s
PMID 26988490

Japanese Journal

P-69 Formation of calcium phosphate on anodic titania nanotubes

Ho Wen-Fu,Hsu Hsueh-Chuan,Tsai Ming-Shiun,Kikuchi Hisaji,Kurotani Tomoko,Wu Shih-Ching,Hsu Shih-Kuang
日本歯科理工学会誌 33(5), 474, 2014-09-20
… Electrochemical formation of tunable nanoscale oxide layers on titanium surfaces has recently drawn much attention in biomaterials research. … These oxide nanotube layers can improve calcium phosphate formation ability and cell activity. … In the current study, the formation of calcium phosphate on nanotube layers of titanium surfaces, anodized at 5 or 10 V for 60 min, was evaluated in simulated body fluids (SBF). …
NAID 110009857519

A-28 酸化カルシウムとポリリン酸からのアパタイト合成 : -第3報- ポリリン酸生成条件(生体組織,一般講演(口頭発表),第64回日本歯科理工学会学術講演会)

成澤英明,柴肇一,大和田弘幸,片岡有,宮崎隆
日本歯科理工学会誌 33(5), 449, 2014-09-20
… Our previous report showed that the big hydroxy apatite crystal grew with polyphosphate and calcium oxide under hydrothermal condition. … 30 g of orthophosphate (85%) were placed in SiC pot, then heat to 200℃ in 10 min, up to 400℃ after 50 min. Kept 0, 1, 6, 96, 192 hours.2 g of the sample, 2.4 g of calcium oxide and 10 ml of water were mixed and placed hydrothermal chamber, 200℃ for 24 hours. …
NAID 110009857494

P-4 水酸化カルシウム圧粉体を用いたカルサイト硬化体の調製 : 処理条件の影響(研究奨励賞審査対象ポスター,第64回日本歯科理工学会学術講演会)

古賀のり子,都留寛治,戸井田力,高橋一郎,石川邦夫
日本歯科理工学会誌 33(5), 390, 2014-09-20
… Effect of treatment condition on carbonation of calcium hydroxide compact was examined. … The result indicated that 100% relative humidity was quite effective for carbonation of calcium hydroxide compact. … When calcium hydroxide compact was prepared under high compaction pressure, the calcite block with high mechanical property could be obtained after the carbonation although it took longer time to transform to calcite. …
NAID 110009857435

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★リンクテーブル★

リンク元	「lime」「酸化カルシウム」
関連記事	「oxide」「calcium」

「lime」

Calcium oxide
Names
	IUPAC name Calcium oxide
	Other names Quicklime, burnt lime, unslaked lime, pebble lime
Identifiers
CAS Number	1305-78-8
ChemSpider	14095
Jmol interactive 3D	Image
PubChem	14778
RTECS number	EW3100000
UNII	C7X2M0VVNH
UN number	1910
	InChI InChI=1/Ca.O/rCaO/c1-2 Key: ODINCKMPIJJUCX-BFMVISLHAU ;
	SMILES [Ca]=O ;
Properties
Chemical formula	CaO
Molar mass	56.0774 g/mol
Appearance	White to pale yellow/brown powder
Odor	Odorless
Density	3.34 g/cm3
Melting point	2,613 °C (4,735 °F; 2,886 K)
Boiling point	3,850 °C (6,960 °F; 4,120 K) (100 hPa)
Solubility in water	Reacts to form calcium hydroxide
Solubility in Methanol	Insoluble (also in diethyl ether, n-octanol)
Acidity (pKa)	12.8
Structure
Crystal structure	NaCl
Thermochemistry
Std molar; entropy (So298)	40 J·mol−1·K−1
Std enthalpy of; formation (ΔfHo298)	−635 kJ·mol−1
Pharmacology
ATCvet code	QP53AX18
Hazards
Safety data sheet	Hazard.com
NFPA 704	0 3 2
Flash point	Non-flammable
	US health exposure limits (NIOSH):
PEL (Permissible)	TWA 5 mg/m3
REL (Recommended)	TWA 2 mg/m3
IDLH (Immediate danger	25 mg/m3
Related compounds
Other anions	Calcium sulfide; Calcium hydroxide
Other cations	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).
	Infobox references