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Butane

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Not to be confused withbutene,butyne,orBhutan.

Butane
Skeletal formula of butane with all carbon and hydrogen atoms shown
Skeletal formula of butane with all implicit hydrogens shown
Ball-and-stick model of the butane molecule
Space-filling model of the butane molecule
Names
Preferred IUPAC name
Butane[3]
Systematic IUPAC name
Tetracarbane (never recommended[3])
Other names
  • Butyl hydride[1]
  • Quartane[2]
  • R600
Identifiers
3D model (JSmol)
969129
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.003.136Edit this at Wikidata
EC Number
  • 203-448-7
E number E943a(glazing agents,...)
1148
KEGG
MeSH butane
RTECS number
  • EJ4200000
UNII
UN number 1011
  • InChI=1S/C4H10/c1-3-4-2/h3-4H2,1-2H3checkY
    Key: IJDNQMDRQITEOD-UHFFFAOYSA-NcheckY
  • CCCC
Properties
C4H10
Molar mass 58.124g·mol−1
Appearance Colorless gas
Odor Gasoline-like or natural gas-like[1]
Density 2.48 kg/m3(at 15 °C (59 °F))
Melting point −140 to −134 °C; −220 to −209 °F; 133 to 139 K
Boiling point −1 to 1 °C; 30 to 34 °F; 272 to 274 K
61 mg/L (at 20 °C (68 °F))
logP 2.745
Vapor pressure ~170 kPa at 283 K[4]
11 nmol Pa−1kg−1
−57.4·10−6cm3/mol
Thermochemistry
98.49 J/(K·mol)
−126.3–−124.9 kJ/mol
−2.8781–−2.8769 MJ/mol
Hazards[5]
GHSlabelling:
GHS02: Flammable
Danger
H220
P210
NFPA 704(fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazard SA: Simple asphyxiant gas. E.g. nitrogen, helium
1
4
0
SA
Flash point −60 °C (−76 °F; 213 K)
405 °C (761 °F; 678 K)
Explosive limits 1.8–8.4%
NIOSH(US health exposure limits):
PEL(Permissible)
 none[1]
REL(Recommended)
 TWA 800 ppm (1900 mg/m3)[1]
IDLH(Immediate danger)
 1600 ppm[1]
Related compounds
Related alkanes
Related compounds
 Perfluorobutane
Supplementary data page
Butane (data page)
Except where otherwise noted, data are given for materials in theirstandard state(at 25 °C [77 °F], 100 kPa).

Butane(/ˈbjuːteɪn/) is analkanewith the formula C4H10.Butane exists as two isomers,n-butane with connectivityCH3CH2CH2CH3and iso-butane with the formula(CH3)3CH.Both isomers are highly flammable, colorless, easilyliquefiedgasesthat quickly vaporize at room temperature and pressure. Butanes are a trace components ofnatural gases(NG gases). The other hydrocarbons in NG includepropane,ethane,and especiallymethane,which are more abundant.Liquified natural gasis a mixture of propane and some butanes.[6]

The name butane comes from the rootbut-(frombutyric acid,named after the Greek word forbutter) and the suffix-ane.

History

[edit]

The first synthesis of butane was accidentally achieved by British chemistEdward Franklandin 1849 fromethyl iodideandzinc,but he had not realized that theethyl radicaldimerized and misidentified the substance.[7]

It was discovered in crude petroleum in 1864 byEdmund Ronalds,who was the first to describe its properties,[8][9]which he named "hydride ofbutyl",[10]based on the naming for the then-knownbutyric acid,which had been named and described by the French chemistMichel Eugène Chevreul[11]40 years earlier. Other names arose in the 1860s: "butyl hydride",[12]"hydride of tetryl"[13]and "tetryl hydride",[14]"diethyl" or "ethyl ethylide"[15]and others.August Wilhelm von Hofmann,in his 1866 systemic nomenclature, proposed the name "quartane",[2]and the modern name was introduced to English from German around 1874.[16]

Butane did not have much practical use until the 1910s, when W. Snelling identified butane and propane as components in gasoline. He found that if they were cooled, they could be stored in a volume-reduced liquified state in pressurized containers. In 1911, Snelling's liquified petroleum gas was publicly available, and his process for producing the mixture was patented in 1913.[17]Butane is one of the most produced industrial chemicals in the 21st century, with around 80-90 billionlbs(40 million US tons, 36 millionmetric tons) produced by theUnited Statesevery year.[18]

Density

[edit]

The density of butane is highly dependent on temperature and pressure in the reservoir.[19]For example, the density of liquid butane is 571.8±1 kg/m3(for pressures up to 2 MPa and temperature 27±0.2 °C), while the density of liquid butane is 625.5±0.7 kg/m3(for pressures up to 2 MPa and temperature −13±0.2 °C).

Isomers

[edit]
Common name normal butane
unbranched butane
n-butane 		isobutane
i-butane
IUPAC name butane methylpropane
Molecular
diagram
Skeletal
diagram

Rotationabout the central C−Cbondproduces two differentconformations(transandgauche) forn-butane.[20]

Reactions

[edit]
Spectrum of the blue flame from abutane torchshowing CH molecularradicalband emission and C2Swan bands

When oxygen is plentiful, butane undergoescomplete combustionto formcarbon dioxideandwater vapor;when oxygen is limited, due toincomplete combustion,carbon (soot) orcarbon monoxidemay be formed instead of carbon dioxide. Butane is denser than air.

When there is sufficient oxygen:

2 C4H10+ 13 O2→ 8 CO2+ 10 H2O

When oxygen is limited:

2 C4H10+ 9 O2→ 8 CO + 10 H2O

By weight, butane contains about 49.5MJ/kg(13.8kWh/kg; 22.5 MJ/lb;21,300Btu/lb) or by liquid volume 29.7megajoulesperliter(8.3 kWh/L; 112 MJ/U.S. gal; 107,000 Btu/U.S. gal).

The maximumadiabatic flametemperature of butane with air is 2,243 K (1,970 °C; 3,578 °F).

n-Butane is the feedstock forDuPont's catalytic process for the preparation ofmaleic anhydride:

2 CH3CH2CH2CH3+ 7 O2→ 2 C2H2(CO)2O + 8 H2O

n-Butane, like allhydrocarbons,undergoesfree radicalchlorination providing both 1-chloro- and 2-chlorobutanes, as well as more highly chlorinated derivatives. The relative rates of the chlorinations are partially explained by the differingbond dissociation energies:425 and 411kJ/molfor the two types of C-H bonds.

Uses

[edit]

Normal butane can be used forgasolineblending, as a fuel gas, fragrance extraction solvent, either alone or in a mixture withpropane,and as a feedstock for the manufacture ofethyleneandbutadiene,a key ingredient ofsynthetic rubber.Isobutaneis primarily used byrefineriesto enhance (increase) theoctanenumber of motor gasoline.[21][22][23][24]

For gasoline blending, n-butane is the main component used to manipulate theReid vapor pressure(RVP). Since winter fuels require much higher vapor pressure for engines to start, refineries raise the RVP by blending more butane into the fuel.[25]n-Butane has a relatively highresearch octane number(RON) andmotor octane number(MON), which are 93 and 92 respectively.[26]

When blended withpropaneand other hydrocarbons, the mixture may be referred to commercially asliquefied petroleum gas(LPG). It is used as a petrol component, as a feedstock for the production of basepetrochemicalsinsteam cracking,as fuel for cigarettelightersand as apropellantinaerosol sprayssuch asdeodorants.[27]

Pure forms of butane, especially isobutane, are used asrefrigerantsand have largely replaced theozone-layer-depletinghalomethanesin refrigerators, freezers, and air conditioning systems. The operating pressure for butane is lower than operating pressures for halomethanes such asFreon-12(R-12). Hence, R-12 systems, such as those in automotive air conditioning systems, when converted to pure butane, will function poorly. Instead, a mixture of isobutane and propane is used to give cooling system performance comparable to R-12.[28]

Butane is also used as lighter fuel for commonlightersorbutane torches,and is sold bottled as a fuel for cooking, barbecues and camping stoves. In the 20th century, theBrauncompany ofGermanymade a cordless hair styling device product that used butane as its heat source to producesteam.[29]

As fuel, butane is often mixed with small amounts ofmercaptansto give the unburned gas an offensive smell easily detected by the human nose. In this way, butane leaks can easily be identified. Whilehydrogen sulfideand mercaptans are toxic, they are present in levels so low thatsuffocationandfire hazardby the butane becomes a concern far beforetoxicity.[30][31]Most commercially available butane also contains some contaminant oil, which can be removed by filtration. If not removed, it will otherwise leave a deposit at the point of ignition and may eventually block the uniform flow of gas.[32]

The butane used as a solvent for fragrance extraction does not contain these contaminants.[33]Butane gas can causegas explosionsin poorly ventilated areas if leaks go unnoticed and are ignited by spark or flame.[5]Purified butane is used as a solvent in the industrial extraction of cannabis oils.

  • Butane fuel canisters for use in camping stoves
    Butane fuel canisters for use in camping stoves
  • Butane lighter, showing liquid butane reservoir
    Butane lighter, showing liquid butane reservoir
  • An aerosol spray can, which may be using butane as a propellant
    An aerosol spray can, which may be using butane as a propellant
  • Butane gas cylinder used for cooking
    Butane gas cylinder used for cooking

Health effects

[edit]
Table from the 2010 ISCD study ranking various drugs (legal and illegal) based on statements by drug-harm experts. Butane was found to be the 14th overall most dangerous drug.[34]

Inhalation of butane can causeeuphoria,drowsiness,unconsciousness,asphyxia,cardiac arrhythmia,fluctuations in blood pressure and temporary memory loss, when abused directly from a highly pressurized container, and can result in death fromasphyxiationandventricular fibrillation.Butane enters the blood supply, and within seconds, leads to intoxication.[35]Butane is the most commonly abusedvolatilesubstance in the UK, and was the cause of 52% of solvent related deaths in 2000.[36]By spraying butane directly into the throat, the jet of fluid can cool rapidly to −20 °C (−4 °F) by expansion, causing prolongedlaryngospasm.[37]"Sudden sniffer's death"syndrome, first described by Bass in 1970,[38]is the most common single cause of solvent related deaths, resulting in 55% of known fatal cases.[37]

See also

[edit]

References

[edit]
  1. ^abcdeNIOSH Pocket Guide to Chemical Hazards."#0068".National Institute for Occupational Safety and Health(NIOSH).
  2. ^abAugust Wilhelm Von Hofmann (1867)."I. On the action of trichloride of phosphorus on the salts of the aromatic monamines".Proceedings of the Royal Society of London.15:54–62.doi:10.1098/rspl.1866.0018.S2CID98496840.
  3. ^ab"General Principles, Rules, and Conventions".Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book).Cambridge:The Royal Society of Chemistry.2014. P-12.1.doi:10.1039/9781849733069-00001.ISBN978-0-85404-182-4.Similarly, the retained names 'ethane', 'propane', and 'butane' were never replaced by systematic names 'dicarbane', 'tricarbane', and 'tetracarbane' as recommended for analogues of silane, 'disilane'; phosphane, 'triphosphane'; and sulfane, 'tetrasulfane'.
  4. ^W. B. Kay (1940). "Pressure-Volume-Temperature Relations for n-Butane".Industrial & Engineering Chemistry.32(3): 358–360.doi:10.1021/ie50363a016.
  5. ^ab"Safety Data Sheet, Material Name: N-Butane"(PDF).USA: Matheson Tri-Gas Incorporated. 5 February 2011. Archived fromthe original(PDF)on 1 October 2011.Retrieved11 December2011.
  6. ^Hammer, Georg; Lübcke, Torsten; Kettner, Roland; Pillarella, Mark R.; Recknagel, Herta; Commichau, Axel; Neumann, Hans-Joachim; Paczynska-Lahme, Barbara (2006). "Natural Gas".Ullmann's Encyclopedia of Industrial Chemistry.doi:10.1002/14356007.a17_073.pub2.ISBN978-3-527-30385-4.
  7. ^Seyferth, Dietmar (2001)."Zinc Alkyls, Edward Frankland, and the Beginnings of Main-Group Organometallic Chemistry".Organometallics.20(14): 2940–2955.doi:10.1021/om010439f.
  8. ^Watts, H.; Muir, M. M. P.; Morley, H. F. (1894).Watts' Dictionary of Chemistry.Vol. 4. Longmans, Green. p. 385.
  9. ^Maybery, C. F. (1896). "On the Composition of the Ohio and Canadian Sulphur Petroleums".Proceedings of the American Academy of Arts and Sciences.31:1–66.doi:10.2307/20020618.JSTOR20020618.
  10. ^"Journal of the Chemical Society".1865.
  11. ^Chevreul (1817)"Extrait d'une lettre de M. Chevreul à MM. les Rédacteurs du Journal de Pharmacie"(Extract of a letter from Mr. Chevreul to the editors of the Journal of Pharmacy),Journal de Pharmacie et des sciences accessoires,3:79–81. On p. 81, he named butyric acid:"Ce principe, que j'ai appelé depuis acid butérique,…"(This principle [i.e., constituent], which I have since named "butyric acid",… )
  12. ^Norman Tate, A. (1863)."Petroleum and Its Products: An Accoumt of the Properties, Uses, and Commercial Value Etc., of Petroleum, the Methods Employed in Refining it and the Properties, Uses, Etc., of Its Product".
  13. ^Watts, Henry (1865)."A Dictionary of Chemistry".
  14. ^Miller, William Allen (1867)."Elements of chemistry pt. 3 1867".
  15. ^Miller, William Allen (1869)."Elements of Chemistry: Theoretical and Practical: Organic chemistry".
  16. ^Schorlemmer, Carl (1874)."A Manual of the Chemistry of the Carbon Compounds: Or, Organic Chemistry".
  17. ^Texas Propane (2022)."The History of Propane".
  18. ^"Chemical Production Data".2024.
  19. ^Zivenko, Oleksiy (2019)."LPG Accounting Specificity During ITS Storage and Transportation".Measuring Equipment and Metrology.80(3): 21–27.doi:10.23939/istcmtm2019.03.021.ISSN0368-6418.S2CID211776025.
  20. ^Roman M. Balabin(2009). "Enthalpy Difference between Conformations of Normal Alkanes: Raman Spectroscopy Study ofn-Pentane andn-Butane ".J. Phys. Chem. A.113(6): 1012–9.Bibcode:2009JPCA..113.1012B.doi:10.1021/jp809639s.PMID19152252.
  21. ^MarkWest Energy Partners, L.P. Form 10-K.Sec.gov.
  22. ^Copano Energy, L.L.C. Form 10-K.Sec.gov. Retrieved on 2012-12-03.
  23. ^Targa Resources Partners LP Form10-k.Sec.gov. Retrieved on 2012-12-03.
  24. ^Crosstex Energy, L.P. FORM 10-K.Sec.gov.
  25. ^Maurice Stewart, Ken Arnold."Reid Vapour Pressure".Science Direct.Archivedfrom the original on 13 June 2020.
  26. ^Jechura, John."octane rating"(PDF).Colorado School of Mines.Archived(PDF)from the original on 1 May 2015.
  27. ^A Primer on Gasoline BlendingArchived30 June 2013 at theWayback Machine.An EPRINC Briefing Memorandum.
  28. ^"R600a | Product Information".www.agas.com.Retrieved1 December2023.
  29. ^"Braun C 100 TS Styling Iron User Manual Type 3589".Inmar-OIQ, LLC. n.d.
  30. ^Gresham, Chip (16 November 2019)."Hydrogen Sulfide Toxicity: Practice Essentials, Pathophysiology, Etiology".Medscape Reference.Retrieved22 March2021.
  31. ^Committee on Acute Exposure Guideline Levels; Committee on Toxicology; Board on Environmental Studies and Toxicology; Division on Earth and Life Studies; National Research Council (26 September 2013).2. Methyl Mercaptan Acute Exposure Guideline Levels.National Academies Press (US) – via NCBI Bookshelf.
  32. ^"BHO Mystery Oil".Skunk Pharm Research.26 August 2013.Retrieved5 December2019.
  33. ^"Final Report of the Safety Assessment of Isobutane, Isopentane, n-Butane, and Propane".Journal of the American College of Toxicology.1(4). SAGE Publications: 127–142. 1982.doi:10.3109/10915818209021266.ISSN0730-0913.S2CID208503534.
  34. ^Nutt DJ, King LA, Phillips LD (November 2010). "Drug harms in the UK: a multicriteria decision analysis".Lancet.376(9752): 1558–1565.CiteSeerX10.1.1.690.1283.doi:10.1016/S0140-6736(10)61462-6.PMID21036393.S2CID5667719.
  35. ^"Neurotoxic Effects from Butane Gas".thcfarmer.com.19 December 2009.Retrieved3 October2016.
  36. ^Field-Smith M, Bland JM, Taylor JC, et al."Trends in death Associated with Abuse of Volatile Substances 1971–2004"(PDF).Department of Public Health Sciences. London: St George’s Medical School. Archived fromthe original(PDF)on 27 March 2007.
  37. ^abRamsey J, Anderson HR, Bloor K, et al. (1989). "An introduction to the practice, prevalence and chemical toxicology of volatile substance abuse".Hum Toxicol.8(4): 261–269.doi:10.1177/096032718900800403.PMID2777265.S2CID19617950.
  38. ^Bass M (1970). "Sudden sniffing death".JAMA.212(12): 2075–2079.doi:10.1001/jama.1970.03170250031004.PMID5467774.
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