Butane

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Butane
Butan Lewis.svg
Butane simple.svg
Butane-3D-balls.png
Butane-3D-space-filling.png
Names
Preferred IUPAC name
Butane [1]
Systematic IUPAC name
Tetracarbane (never recommended [1] )
Other names
  • Butyl hydride [2]
  • Quartane [3]
  • R600
Identifiers
3D model (JSmol)
969129
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.003.136 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 203-448-7
E number E943a (glazing agents, ...)
1148
KEGG
MeSH butane
PubChem CID
RTECS number
  • EJ4200000
UNII
UN number 1011
  • InChI=1S/C4H10/c1-3-4-2/h3-4H2,1-2H3 Yes check.svgY
    Key: IJDNQMDRQITEOD-UHFFFAOYSA-N Yes check.svgY
  • CCCC
Properties
C4H10
Molar mass 58.124 g·mol−1
AppearanceColorless gas
Odor Gasoline-like or natural gas-like [2]
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))
log P 2.745
Vapor pressure ~170 kPa at 283 K [4]
11 nmol Pa−1 kg−1
−57.4·10−6 cm3/mol
Thermochemistry
98.49 J/(K·mol)
−126.3–−124.9 kJ/mol
−2.8781–−2.8769 MJ/mol
Hazards [5]
GHS labelling:
GHS-pictogram-flamme.svg GHS-pictogram-bottle.svg
Danger
H220
P210
NFPA 704 (fire diamond)
NFPA 704.svgHealth 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 [2]
REL (Recommended)
TWA 800 ppm (1900 mg/m3) [2]
IDLH (Immediate danger)
1600 ppm [2]
Related compounds
Related alkanes
Related compounds
 Perfluorobutane
Supplementary data page
Butane (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yes check.svgY  verify  (what is  Yes check.svgYX mark.svgN ?)

Butane ( /ˈbjuːteɪn/ ) or n-butane is an alkane with the formula C4H10. Butane is a highly flammable, colorless, easily liquefied gas that quickly vaporizes at room temperature and pressure. The name butane comes from the root but- (from butyric acid, named after the Greek word for butter) and the suffix -ane. It was discovered in crude petroleum in 1864 by Edmund Ronalds, who was the first to describe its properties, [6] [7] and commercialized by Walter O. Snelling in the early 1910s.

Butane is one of a group of liquefied petroleum gases (LP gases). The others include propane, propylene, butadiene, butylene, isobutylene, and mixtures thereof. Butane burns more cleanly than both gasoline and coal.

History

The first synthesis of butane was accidentally achieved by British chemist Edward Frankland in 1849 from ethyl iodide and zinc, but he had not realized that the ethyl radical dimerized and misidentified the substance. [8]

Edmund Ronalds was the first individual to isolate and describe butane, which he named "hydride of butyl," [9] based on the naming for the then-known butyric acid, which had been named and described by the French chemist Michel Eugène Chevreul [10] 40 years earlier. Other names arose in the 1860s: "butyl hydride", [11] "hydride of tetryl" [12] and "tetryl hydride", [13] "diethyl" or "ethyl ethylide" [14] and others. August Wilhelm von Hofmann, in his 1866 systemic nomenclature, proposed the name "quartane", [3] and the modern name was introduced to English from German around 1874. [15]

Butane did not have much practical use until the 1910s, when W. Snelling identified butane and propane as components in gasoline and 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. [16] Butane is one of the most produced industrial chemicals in the 21st century with around 80-90 billion lbs (40 million US tons, 36 million metric tons) produced by the United States every year. [17]

Density

The density of butane is highly dependent on temperature and pressure in the reservoir. [18] For example, the density of liquid butane is 571.8±1 kg/m3 (for pressures up to 2MPa and temperature 27±0.2 °C), while the density of liquid butane is 625.5±0.7 kg/m3 (for pressures up to 2MPa and temperature -13±0.2 °C).

Isomers

Common namenormal butane
unbranched butane
n-butane		 isobutane
i-butane
IUPAC namebutanemethylpropane
Molecular
diagram		 Butan Lewis.svg Isobutane 1.svg
Skeletal
diagram		 Butane simple.svg I-Butane-2D-Skeletal.svg

Rotation about the central C−C bond produces two different conformations (trans and gauche) for n-butane. [19]

Reactions

Spectrum of the blue flame from a butane torch showing CH molecular radical band emission and C2 Swan bands Spectrum of blue flame - intensity corrected.png
Spectrum of the blue flame from a butane torch showing CH molecular radical band emission and C2 Swan bands

When oxygen is plentiful, butane burns to form carbon dioxide and water vapor; when oxygen is limited, carbon (soot) or carbon monoxide may also be formed. 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 49.5  MJ / kg (13.8  kWh /kg; 22.5 MJ/ lb ; 21,300  Btu /lb) or by liquid volume 29.7 megajoules per liter (8.3 kWh/L; 112 MJ/U.S. gal; 107,000 Btu/U.S. gal).

The maximum adiabatic flame temperature of butane with air is 2,243 K (1,970 °C; 3,578 °F).

n-Butane is the feedstock for DuPont's catalytic process for the preparation of maleic anhydride:

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

n-Butane, like all hydrocarbons, undergoes free radical chlorination providing both 1-chloro- and 2-chlorobutanes, as well as more highly chlorinated derivatives. The relative rates of the chlorination is partially explained by the differing bond dissociation energies, 425 and 411 kJ/mol for the two types of C-H bonds.

Uses

Normal butane can be used for gasoline blending, as a fuel gas, fragrance extraction solvent, either alone or in a mixture with propane, and as a feedstock for the manufacture of ethylene and butadiene, a key ingredient of synthetic rubber. Isobutane is primarily used by refineries to enhance (increase) the octane number of motor gasoline. [20] [21] [22] [23]

For gasoline blending, n-butane is the main component used to manipulate the Reid 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. [24] n-Butane has a relatively high research octane number (RON) and motor octane number (MON), which are 93 and 92 respectively. [25]

When blended with propane and other hydrocarbons, the mixture may be referred to commercially as liquefied petroleum gas (LPG). It is used as a petrol component, as a feedstock for the production of base petrochemicals in steam cracking, as fuel for cigarette lighters and as a propellant in aerosol sprays such as deodorants. [26]

Pure forms of butane, especially isobutane, are used as refrigerants and have largely replaced the ozone-layer-depleting halomethanes in refrigerators, freezers, and air conditioning systems. The operating pressure for butane is lower than for the halomethanes such as Freon-12 (R-12), so R-12 systems such as those in automotive air conditioning systems, when converted to pure butane, will function poorly. A mixture of isobutane and propane is used instead to give cooling system performance comparable to use of R-12. [27]

Butane is also used as lighter fuel for common lighters or butane torches and is sold bottled as a fuel for cooking, barbecues and camping stoves. In the 20th century the Braun company of Germany made a cordless hair styling device product that used butane as its heat source to produce steam. [28]

As fuel, it is often mixed with small amounts of mercaptans to give the unburned gas an offensive smell easily detected by the human nose. In this way, butane leaks can easily be identified. While hydrogen sulfide and mercaptans are toxic, they are present in levels so low that suffocation and fire hazard by the butane becomes a concern far before toxicity. [29] [30] Most commercially available butane also contains some contaminant oil, which can be removed by filtration and will otherwise leave a deposit at the point of ignition and may eventually block the uniform flow of gas. [31]

The butane used as a solvent for fragrance extraction does not contain these contaminants [32] and butane gas can cause gas explosions in 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.

Effects and health issues

Inhalation of butane can cause euphoria, 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 from asphyxiation and ventricular fibrillation. It enters the blood supply and within seconds produces intoxication. [33] Butane is the most commonly abused volatile substance in the UK, and was the cause of 52% of solvent related deaths in 2000. [34] By spraying butane directly into the throat, the jet of fluid can cool rapidly to −20 °C (−4 °F) by expansion, causing prolonged laryngospasm. [35] "Sudden sniffer's death" syndrome, first described by Bass in 1970, [36] is the most common single cause of solvent related death, resulting in 55% of known fatal cases. [35]

See also

Related Research Articles

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References

  1. 1 2 "Front Matter". Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 4. doi:10.1039/9781849733069-FP001. ISBN   978-0-85404-182-4. 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'.
  2. 1 2 3 4 5 NIOSH Pocket Guide to Chemical Hazards. "#0068". National Institute for Occupational Safety and Health (NIOSH).
  3. 1 2 August 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. S2CID   98496840.
  4. ↑ W. B. Kay (1940). "Pressure-Volume-Temperature Relations for n-Butane". Industrial & Engineering Chemistry. 32 (3): 358–360. doi:10.1021/ie50363a016.
  5. 1 2 "Safety Data Sheet, Material Name: N-Butane" (PDF). USA: Matheson Tri-Gas Incorporated. 5 February 2011. Archived from the original (PDF) on 1 October 2011. Retrieved 11 December 2011.
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  7. ↑ 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. JSTOR   20020618.
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  22. ↑ Targa Resources Partners LP Form10-k. Sec.gov. Retrieved on 2012-12-03.
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  31. ↑ "BHO Mystery Oil". Skunk Pharm Research. 26 August 2013. Retrieved 5 December 2019.
  32. ↑ "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. ISSN   0730-0913. S2CID   208503534.
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  35. 1 2 Ramsey 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. PMID   2777265. S2CID   19617950.
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