| 词条 | Ethyl nitrate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 428846955 | ImageFile = Ethyl Nitrate Structural Formulae V.1.svg | ImageSize = 160 | ImageAlt = Skeletal formula of ethyl nitrate | ImageFile1 = Ethyl nitrate 3D ball.png | ImageSize1 = 160 | ImageAlt1 = Ball-and-stick model of the ethyl nitrate molecule | IUPACName = Ethyl nitrate | OtherNames = Nitric acid ethyl ester |Section1={{Chembox Identifiers | CASNo_Ref = {{cascite|correct|??}} | CASNo = 625-58-1 | PubChem = 12259 | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 11756 | InChI = 1/C2H5NO3/c1-2-6-3(4)5/h2H2,1H3 | InChIKey = IDNUEBSJWINEMI-UHFFFAOYAM | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChI = 1S/C2H5NO3/c1-2-6-3(4)5/h2H2,1H3 | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey = IDNUEBSJWINEMI-UHFFFAOYSA-N | SMILES = CCO[N+](=O)[O-] |Section2={{Chembox Properties | Formula = C2H5NO3 | MolarMass = 91.07 g/mol | Appearance = colorless liquid | Density = 1.10g/cm3 | MeltingPtC = −102 | BoilingPtC = 87.5 | Solubility = soluble |Section3={{Chembox Hazards | MainHazards = | NFPA-H = 2 | NFPA-F = 3 | NFPA-R = 4 | NFPA-S = | FlashPtF = -34 | AutoignitionPtC = | ExploLimits = 4.1%-50% |Section8={{Chembox Related | OtherFunction_label = Alkyl nitrates | OtherFunction = Methyl nitrate Ethylene glycol dinitrate Isopropyl nitrate }}Ethyl nitrate is the ethyl ester of nitric acid and has the chemical formula {{carbon|2}}{{hydrogen|5}}{{nitrogen}}{{oxygen|3}}. It is a colourless, volatile, highly flammable liquid. It is used in organic synthesis and as an intermediate in the preparation of some drugs, dyes, and perfumes.[1] Ethyl nitrate is found in the atmosphere, where it can react with other gases to form smog. Originally thought to be a pollutant, formed mainly by the combustion of fossil fuels, recent analysis of ocean water samples reveal that in places where cool water rises from the deep, the water is saturated with alkyl nitrates, likely formed by natural processes.[2] PreparationEthyl nitrate has been prepared by bubbling gaseous nitryl fluoride through ethanol at −10 °C.[3] The reaction was subsequently studied in detail.[4][5] Ethyl nitrate can be prepared by nitrating ethanol with fuming nitric acid or a mixture of concentrated sulfuric and nitric acids. Further purifying by distillation carries a risk of explosion.[6] References1. ^{{Cite book|url=https://www.worldcat.org/oclc/6357479|title=Aromatic nitration|last=1921-|first=Schofield, Kenneth,|date=1980|publisher=Cambridge University Press|isbn=9780521233620|location=Cambridge|oclc=6357479|page=94}} 2. ^{{cite news | title =Ocean yields gases that had seemed humanmade | author =S. Perkins | publisher = Science News | date = August 12, 2002 | url = http://sciencenews.org/articles/20020817/fob8ref.asp}} 3. ^{{cite journal| title =Nitryl fluoride as a nitrating agent| author =G. Hetherington and R. L. Robinson| date = 1954| journal = J. Chem. Soc. | doi = 10.1039/JR9540003512| pages = 3512 }} 4. ^{{cite journal| author =B. S. Fedorov and L. T. Eremenko| title = Nitration of alcohols by nitryl fluoride| date = 1997| volume = 46| issue = 5| journal = Russian Chemical Bulletin | doi = 10.1007/BF02496138| pages = 1022–1023}} 5. ^Explosives, 6th Edition, R. Meyer, J. Kohler, A. Homburg; page 125 6. ^{{Cite book|url=https://archive.org/details/theoreticalorgan00coherich|title=Theoretical organic chemistry|last=Cohen|first=Julius B. (Julius Berend)|date=1920|publisher=London, Macmillan|others=University of California Libraries|page=189}} 2 : Ethyl esters|Alkyl nitrates |
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