Ethyl nitrate

Source: Wikipedia, the free encyclopedia.
Not to be confused with nitroethane or ethyl nitrite.
Ethyl nitrate
Skeletal formula of ethyl nitrate
Ball-and-stick model of the ethyl nitrate molecule
Names
IUPAC name
1-Nitrosooxyethane
Preferred IUPAC name
Ethyl nitrate
Other names
Nitric acid ethyl ester
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.009.913 Edit this at Wikidata
UNII
  • InChI=1S/C2H5NO3/c1-2-6-3(4)5/h2H2,1H3 ☒N
    Key: IDNUEBSJWINEMI-UHFFFAOYSA-N ☒N
  • InChI=1/C2H5NO3/c1-2-6-3(4)5/h2H2,1H3
    Key: IDNUEBSJWINEMI-UHFFFAOYAM
  • CCO[N+](=O)[O-]
Properties
C2H5NO3
Molar mass 91.066 g·mol−1
Appearance colorless liquid
Density 1.10g/cm3
Melting point −102 °C (−152 °F; 171 K)
Boiling point 87.5 °C (189.5 °F; 360.6 K)
soluble
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineInstability 4: Readily capable of detonation or explosive decomposition at normal temperatures and pressures. E.g. nitroglycerinSpecial hazards (white): no code
2
3
4
Flash point −37 °C; −34 °F; 236 K
Explosive limits
 4.1%-50%
Related compounds
Related
Alkyl nitrates
 Methyl nitrate
Ethylene glycol dinitrate
Isopropyl nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Ethyl nitrate is the

drugs, dyes, and perfumes.[1]

Ethyl nitrate is found in the atmosphere, where it can react with other gases to form smog. The

saturated with alkyl nitrates, likely formed by natural processes.[2]

Preparation

Ethyl 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]

References

  1. OCLC 6357479
    .
  2. ^ S. Perkins (August 12, 2002). "Ocean yields gases that had seemed humanmade". Science News (only available to subscribers).
  3. doi:10.1039/JR9540003512
    .
  4. doi:10.1007/BF02496138
    .
  5. ^ Explosives, 6th Edition, R. Meyer, J. Kohler, A. Homburg; page 125
  6. ^ Cohen, Julius B. (Julius Berend) (1920). Theoretical organic chemistry. University of California Libraries. London, Macmillan. p. 189.
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