|Preferred IUPAC name
|Systematic IUPAC name
Tetracarbane (never recommended)
3D model (JSmol)
|E number||E943a (glazing agents, ...)|
CompTox Dashboard (EPA)
|Molar mass||g·mol−1 58.124|
|Odor||Gasoline-like or natural gas-like|
|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−1 (at 20 °C (68 °F))|
|Vapor pressure||~170 kPa at 283 K |
|11 nmol Pa−1 kg−1|
Heat capacity (C)
|98.49 J K−1 mol−1|
Std enthalpy of
|−126.3–−124.9 kJ mol−1|
Std enthalpy of
|−2.8781–−2.8769 MJ mol−1|
|Safety data sheet||See: data page|
|GHS signal word||DANGER|
|Flash point||−60 °C (−76 °F; 213 K)|
|405 °C (761 °F; 678 K)|
|US health exposure limits (NIOSH):|
|TWA 800 ppm (1900 mg/m3)|
IDLH (Immediate danger)
|Supplementary data page|
|Refractive index (n),|
Dielectric constant (εr), etc.
|UV, IR, NMR, MS|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Butane (//) is an organic compound with the formula C4H10 that is an alkane with four carbon atoms. Butane is a gas at room temperature and atmospheric pressure. The term may refer to either of two structural isomers, n-butane or isobutane (also called "methylpropane"), or to a mixture of these isomers. In the IUPAC nomenclature, however, "butane" refers only to the n-butane isomer (which is the isomer with the unbranched structure). Butanes are highly flammable, colorless, easily liquefied gases that quickly vaporize at room temperature. The name butane comes from the roots but- (from butyric acid, named after the Greek word for butter) and -ane. It was discovered by the chemist Edward Frankland in 1849. It was found dissolved in crude petroleum in 1864 by Edmund Ronalds, who was the first to describe its properties.
|Common name||normal butane
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
- 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.
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.
When blended with propane and other hydrocarbons, it may be referred to commercially as LPG, for liquefied petroleum gas. 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.
Very pure forms of butane, especially isobutane, can be used as refrigerants and have largely replaced the ozone-layer-depleting halomethanes, for instance in household refrigerators and freezers. The system operating pressure for butane is lower than for the halomethanes, such as R-12, so R-12 systems such as in automotive air conditioning systems, when converted to pure butane will not function optimally and therefore a mix of isobutane and propane is used to give cooling system performance comparable to R-12.
Butane is also used as lighter fuel for a common lighter or butane torch and is sold bottled as a fuel for cooking, barbecues and camping stoves. Butane canisters are almost exclusively manufactured in South Korea with the only exception being one manufacturer in Houston, Texas. Butane canisters manufactured in South Korea contain butane from Saudi Arabia, while the American manufacturer fills canisters with domestic butane.
In this form it is often mixed with small amounts of hydrogen sulfide and mercaptans which will 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. Most commercially available butane also contains a certain amount of contaminant oil which can be removed through filtration but which will otherwise leave a deposit at the point of ignition and may eventually block the uniform flow of gas. Contaminants are not used in fragrance extraction and butane gasses can cause gas explosions in poorly ventilated areas if leaks go unnoticed and are ignited by spark or flame.
|Butane fuel canisters for use in camping stoves.||Butane lighter, showing liquid butane reservoir||Butane being sprayed from an aerosol spray can||Butane gas cylinder used for cooking|
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. Butane is the most commonly misused volatile substance in the UK, and was the cause of 52% of solvent related deaths in 2000. By spraying butane directly into the throat, the jet of fluid can cool rapidly to −20 °C (−4 °F) by expansion, causing prolonged laryngospasm. "Sudden sniffer's death" syndrome, first described by Bass in 1970, is the most common single cause of solvent related death, resulting in 55% of known fatal cases.
A small amount of nitrogen dioxide, a toxic gas, results from burning butane gas, along with any combustion in the earth's atmosphere, and represents a human health hazard from home heaters and stoves.
- Dimethyl ether
- Volatile substance abuse
- Butane (data page)
- Liquefied petroleum gas
- Industrial gas
- Butane torch
- Gas explosions
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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’.
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