Methane

Methane
IUPAC name Methane[1](substitutive) Tetrahydridocarbon[1] (additive)
Other names Carbane Marsh Gas
Identifiers
CAS number	Y
PubChem
ChemSpider	Y
EC number
UN number	1971
KEGG	N
MeSH
ChEBI	Y
ChEMBL	Y
RTECS number	PA1490000
Beilstein Reference	1718732
Gmelin Reference	59
3DMet
Jmol-3D images	Image 1
SMILES C
InChI InChI=1S/CH4/h1H4 Y Key: VNWKTOKETHGBQD-UHFFFAOYSA-N Y
Properties
Molecular formula	CH4
Molar mass	16.04 g mol−1
Appearance	Colorless gas
Odor	Odorless
Density	0.656 g/L at 25 °C, 1 atm 0.716 g/L at 0 °C, 1 atm 0.42262 g cm−3 (at 111 K [−162 °C; −260 °F])[2]
Melting point	−182.5 °C; −296.4 °F; 90.7 K
Boiling point	−161.49 °C; −258.68 °F; 111.66 K
Solubility in water	22.7 mg L−1
Solubility	soluble in ethanol, diethyl ether, benzene, toluene, methanol, acetone
log P	1.09
kH	14 nmol Pa−1 kg−1
Structure
Point group	Td
Molecular shape	Tetrahedron
Dipole moment	0 D
Thermochemistry
Specific heat capacity C	35.69 J K−1 mol−1
Std molar entropy So298	186.25 J K−1 mol−1
Std enthalpy of formation ΔfHo298	−74.87 kJ mol−1
Std enthalpy of combustion ΔcHo298	−891.1 to −890.3 kJ mol−1
Hazards[3]
MSDS	External MSDS
GHS pictograms
GHS signal word	DANGER
GHS hazard statements	H220
GHS precautionary statements	P210
EU Index	601-001-00-4
EU classification	F+
R-phrases	R12
S-phrases	(S2), S16, S33
NFPA 704	4 1 0
Flash point	−188 °C (−306.4 °F; 85.1 K)
Autoignition temperature	537 °C (999 °F; 810 K)
Explosive limits	4.4–17%
Related compounds
Related alkanes	Methyl iodide Diiodomethane Iodoform Carbon tetraiodide Ethane Ethyl iodide
Supplementary data page
Structure and properties	n, εr, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
N   Y/N?)

Methane ( or ) is a chemical compound with the chemical formula CH
4 (one atom of carbon and four atoms of hydrogen). It is the simplest alkane and the main component of natural gas. The relative abundance of methane makes it an attractive fuel, though capturing and storing it poses challenges due to its gaseous state found at normal conditions. In its natural state, methane is found both below ground, and under the sea floor, where it often finds its way to the surface and in the earth's atmosphere where it is known as atmospheric methane.^[4]

History

In November 1776, methane was first scientifically identified by Italian physicist Alessandro Volta in the marshes of Lake Maggiore straddling Italy and Switzerland, having been inspired to search for the substance after reading a paper written by Benjamin Franklin about "flammable air".^[5] Volta captured the gas rising from the marsh, and by 1778 had isolated the pure gas.^[6] He also demonstrated means to ignite the gas with an electric spark.^[6]

Properties and bonding

Methane is a tetrahedral molecule with four equivalent C-H bonds. Its electronic structure is described by four bonding molecular orbitals (MOs) resulting from the overlap of the valence orbitals on C and H. The lowest energy MO is the result of the overlap of the 2s orbital on carbon with the in-phase combination of the 1s orbitals on the four hydrogen atoms. Above this level in energy is a triply degenerate set of MOs that involve overlap of the 2p orbitals on carbon with various linear combinations of the 1s orbitals on hydrogen. The resulting "three-over-one" bonding scheme is consistent with photoelectron spectroscopic measurements.

At room temperature and standard pressure, methane is a colorless, odorless gas.^[7] The familiar smell of natural gas as used in homes is a safety measure achieved by the addition of an odorant, usually blends containing tert-butylthiol. Methane has a boiling point of −161 °C (−257.8 °F) at a pressure of one atmosphere.^[8] As a gas it is flammable over a range of concentrations (4.4–17%) in air at standard pressure.

Chemical reactions

Main reactions with methane are: combustion, steam reforming to syngas, and halogenation. In general, methane reactions are difficult to control. Partial oxidation to methanol, for example, is challenging because the reaction typically progresses all the way to carbon dioxide and water even with incomplete amounts of oxygen. The enzymes methane monooxygenase can produce methanol from methane, but they cannot be used for industrial scale reactions.^[9]

Acid-base reactions

Like other hydrocarbons, methane is a very weak acid. Its pKa in DMSO is estimated to be 56.^[10] It cannot be deprotonated in solution, but the conjugate base with methyllithium is known.

A variety of positive ions derived from methane have been observed, mostly as unstable species in low-pressure gas mixtures. These include methenium or methyl cation CH+
3, methane cation CH+
4, and methanium or protonated methane CH+
5. Some of these have been detected in outer space. Methanium can also be produced as diluted solutions from methane with super acids. Cations with higher charge, such as CH2+
6 and CH3+
7, have been studied theoretically and conjectured to be stable.^[11]

Despite the strength of its C-H bonds, there is intense interest in catalysts that facilitate C–H bond activation in methane (and other low alkanes).^[12]

Combustion

Methane's heat of combustion is 55.5 MJ/kg.^[13] Combustion of methane is a multiple step reaction. The following equations are part of the process, with the net result being:

CH₄ + 2 O₂ → CO₂ + 2 H₂O (ΔH = −891 kJ/mol (at standard conditions))

1. CH₄+ M^* → CH₃ + H + M
2. CH₄ + O₂ → CH₃ + HO₂
3. CH₄ + HO₂ → CH₃ + 2 OH
4. CH₄ + OH → CH₃ + H₂O
5. O₂ + H → O + OH
6. CH₄ + O → CH₃ + OH
7. CH₃ + O₂ → CH₂O + OH
8. CH₂O + O → CHO + OH
9. CH₂O + OH → CHO + H₂O
10. CH₂O + H → CHO + H₂
11. CHO + O → CO + OH
12. CHO + OH → CO + H₂O
13. CHO + H → CO + H₂
14. H₂ + O → H + OH
15. H₂ + OH → H + H₂O
16. CO + OH → CO₂ + H
17. H + OH + M → H₂O + M^*
18. H + H + M → H₂ + M^*
19. H + O₂ + M → HO₂ + M^*

The species M^* signifies an energetic third body, from which energy is transferred during a molecular collision. Formaldehyde (HCHO or H
2CO) is an early intermediate (reaction 7). Oxidation of formaldehyde gives the formyl radical (HCO; reactions 8–10), which then give carbon monoxide (CO) (reactions 11, 12 & 13). Any resulting H₂ oxidizes to H₂O or other intermediates (reaction 14, 15). Finally, the CO oxidizes, forming CO₂ (reaction 16). In the final stages (reactions 17–19), energy is transferred back to other third bodies. The overall speed of reaction is a function of the concentration of the various entities during the combustion process. The higher the temperature, the greater the concentration of radical species and the more rapid the combustion process.^[14]

Reactions with halogens

Methane reacts with halogens given appropriate conditions as follows:

X₂ + UV → 2 X•

X• + CH₄ → HX + CH₃•

CH₃• + X₂ → CH₃X + X•

where X is a halogen: fluorine (F), chlorine (Cl), bromine (Br), or iodine (I). This mechanism for this process is called free radical halogenation. It is initiated with UV light or some other radical initiator. A chlorine atom is generated from elemental chlorine, which abstracts a hydrogen atom from methane, resulting in the formation of hydrogen chloride. The resulting methyl radical, CH₃•, can combine with another chlorine molecule to give methyl chloride (CH₃Cl) and a chlorine atom. This chlorine atom can then react with another methane (or methyl chloride) molecule, repeating the chlorination cycle.^[15] Similar reactions can produce dichloromethane (CH₂Cl₂), chloroform (CHCl₃), and, ultimately, carbon tetrachloride (CCl₄), depending upon reaction conditions and the chlorine to methane ratio.

Uses

Methane is used in industrial chemical processes and may be transported as a refrigerated liquid (liquefied natural gas, or LNG). While leaks from a refrigerated liquid container are initially heavier than air due to the increased density of the cold gas, the gas at ambient temperature is lighter than air. Gas pipelines distribute large amounts of natural gas, of which methane is the principal component.

Fuel

Natural gas

Methane is important for electrical generation by burning it as a fuel in a gas turbine or steam generator. Compared to other hydrocarbon fuels, burning methane produces less carbon dioxide for each unit of heat released. At about 891 kJ/mol, methane's heat of combustion is lower than any other hydrocarbon but the ratio of the heat of combustion (891 kJ/mol) to the molecular mass (16.0 g/mol, of which 12.0 g/mol is carbon) shows that methane, being the simplest hydrocarbon, produces more heat per mass unit (55.7 kJ/g) than other complex hydrocarbons. In many cities, methane is piped into homes for domestic heating and cooking purposes. In this context it is usually known as natural gas, which is considered to have an energy content of 39 megajoules per cubic meter, or 1,000 BTU per standard cubic foot.

Methane in the form of compressed natural gas is used as a vehicle fuel and is claimed to be more environmentally friendly than other fossil fuels such as gasoline/petrol and diesel.^[16] Research into adsorption methods of methane storage for use as an automotive fuel has been conducted.^[17]

Liquefied natural gas

Liquefied natural gas or LNG is natural gas (predominantly methane, CH₄) that has been converted to liquid form for ease of storage or transport.

Liquefied natural gas takes up about 1/600th the volume of natural gas in the gaseous state. It is odorless, colorless, non-toxic and non-corrosive. Hazards include flammability after vaporization into a gaseous state, freezing and asphyxia.

The liquefaction process involves removal of certain components, such as dust, acid gases, helium, water, and heavy hydrocarbons, which could cause difficulty downstream. The natural gas is then condensed into a liquid at close to atmospheric pressure (maximum transport pressure set at around 25 kPa or 3.6 psi) by cooling it to approximately −162 °C (−260 °F).

LNG achieves a higher reduction in volume than compressed natural gas (CNG) so that the energy density of LNG is 2.4 times greater than that of CNG or 60% of that of diesel fuel.^[18] This makes LNG cost efficient to transport over long distances where pipelines do not exist. Specially designed cryogenic sea vessels (LNG carriers) or cryogenic road tankers are used for its transport.

LNG, when it is not highly refined for special uses, is principally used for transporting natural gas to markets, where it is regasified and distributed as pipeline natural gas. It is also used in LNG-fueled road vehicles as is beginning to be seen with some trucks in commercial operation, which have been achieving payback periods of approximately four years on the higher initial investment required in LNG equipment on the trucks and LNG infrastructure to support fueling.^[19] However, it remains more common to design vehicles to use compressed natural gas. As of 2002, the relatively higher cost of LNG production and the need to store LNG in more expensive cryogenic tanks had slowed widespread commercial use.^[20]

Power to gas

Power to gas is a technology which converts electrical power to a gas fuel. The method is used to convert carbon dioxide and water to methane, (see natural gas) using electrolysis and the Sabatier reaction. The excess power or off peak power generated by wind generators or solar arrays could theoretically be used for load balancing in the energy grid.

Liquid methane rocket fuel

In a highly refined form, liquid methane is used as a rocket fuel.^[21]

While investigations of methane use have existed for decades, no production methane engines have yet been used on orbital spaceflights.^[22] This is changing, and liquid methane has recently been selected for the active development of a variety of bipropellant rocket engines.

Since the 1990s, a number of Russian rockets have been proposed to use liquid methane.^[23][24] One 1990s Russian engine proposal was the RD-192, a methane/LOX variant of the RD-191.^[24]

In 2005, US companies, Orbitech and XCOR Aerospace, developed a demonstration liquid oxygen/liquid methane rocket engine and a larger 7,500 pounds-force (33 kN)-thrust engine in 2007 for potential use as the CEV lunar return engine, before the CEV program was later cancelled.^[25][26][27]

More recently the American private space company SpaceX announced in 2012 an initiative to develop liquid methane rocket engines,^[28] including, initially, the very large Raptor rocket engine.^[29]

Raptor is being designed to produce 4.4 meganewtons (1,000,000 lbf) of thrust with a vacuum specific impulse (I_sp) of 363 seconds and a sea-level I_sp of 321 seconds,^[30] and is expected to begin component-level testing in 2014.^[31] In February 2014, the Raptor engine design was revealed to be of the highly efficient and theoretically more reliable full-flow staged combustion cycle type, where both propellant streams—oxidizer and fuel—will be completely in the gas phase before they enter the combustion chamber. Prior to 2014, only two full-flow rocket engines have ever progressed sufficiently to be tested on test stands, but neither engine completed development or flew on a flight vehicle.^[30]

In October 2013, the China Aerospace Science and Technology Corporation, a state-owned contractor for the Chinese space program, announced that it had completed a first ignition test on a new LOX methane rocket engine. No engine size was provided.^[32]

In September 2014, another American private space company—Blue Origin announced work on a large methane rocket engine. The new engine, the Blue Engine 4, or BE-4, has been designed to produce 2,400 kilonewtons (550,000 lbf) of thrust. While initially planned to be used exclusively on a Blue Origin proprietary launch vehicle, it will now be used on a new United Launch Alliance (ULA) engine on an new launch vehicle that is a successor to the Atlas V. ULA expects the first flight of the new launch vehicle no earlier than 2019.^[33]

One advantage of methane is that it is abundant in many parts of the solar system and it could potentially be harvested on the surface of another solar-system body (in particular, using In Situ Resource Utilization on Mars^[34] and Titan), providing fuel for a return journey.^[21][35]

NASA's Project Morpheus has developed a restartable LOX methane rocket engine with 5,000 pounds-force (22 kN) thrust and a specific impulse of 321 seconds suitable for inspace applications including landers. Small LOX methane thrusters 5–15 pounds-force (22–67 N) were also developed suitable for use in a Reaction Control System (RCS).^[36][37]

Chemical feedstock

Although there is great interest in converting methane into useful or more easily liquefied compounds, the only practical processes are relatively unselective. In the chemical industry, methane is converted to synthesis gas, a mixture of carbon monoxide and hydrogen, by steam reforming. This endergonic process (requiring energy) utilizes nickel catalysts and requires high temperatures, around 700–1100 °C:

CH₄ + H₂O → CO + 3 H₂

Related chemistries are exploited in the Haber-Bosch Synthesis of ammonia from air, which is reduced with natural gas to a mixture of carbon dioxide, water, and ammonia.

Methane is also subjected to free-radical chlorination in the production of chloromethanes, although methanol is a more typical precursor.^[38]

Production

Biological routes

Naturally occurring methane is mainly produced by the process of methanogenesis. This multistep process is used by microorganisms as an energy source. The net reaction is:

CO₂ + 8 H⁺ + 8 e⁻ → CH₄ + 2 H₂O

The final step in the process is catalyzed by the enzyme landfill, ruminants (e.g., cattle), and the guts of termites.

It is uncertain if plants are a source of methane emissions.^[39][40][41]

Serpentinization

Methane could also be produced by a non-biological process called serpentinization^[1] involving water, carbon dioxide, and the mineral olivine, which is known to be common on Mars.^[42]

Industrial routes

Methane can be produced by hydrogenating carbon dioxide through the Sabatier process. Methane is also a side product of the hydrogenation of carbon monoxide in the Fischer-Tropsch process. This technology is practiced on a large scale to produce longer chain molecules than methane.

Natural gas is so abundant that the intentional production of methane is relatively rare. The only large scale facility of this kind is the Great Plains Synfuels plant, started in 1984 in Beulah, North Dakota as a way to develop abundant local resources of low grade lignite, a resource which is otherwise very hard to transport for its weight, ash content, low calorific value and propensity to spontaneous combustion during storage and transport.

An adaptation of the Sabatier methanation reaction may be used via a mixed catalyst bed and a reverse water gas shift in a single reactor to produce methane from the raw materials available on Mars, utilizing water from the Martian subsoil and carbon dioxide in the Martian atmosphere.^[34]

Laboratory synthesis

Methane can also be produced by the destructive distillation of acetic acid in the presence of soda lime or similar. Acetic acid is decarboxylated in this process. Methane can also be prepared by reaction of aluminium carbide with water or strong acids.

Occurrence

Methane was discovered and isolated by oil generate natural gas.

It is generally transported in bulk by pipeline in its natural gas form, or LNG carriers in its liquefied form; few countries transport it by truck.

Alternative sources

Testing Australian sheep for exhaled methane production (2001), CSIRO

Apart from gas fields, an alternative method of obtaining methane is via manure, wastewater sludge, municipal solid waste (including landfills), or any other biodegradable feedstock, under anaerobic conditions. Rice fields also generate large amounts of methane during plant growth. Methane hydrates/clathrates (ice-like combinations of methane and water on the sea floor, found in vast quantities) are a potential future source of methane. Cattle belch methane accounts for 16% of the world's annual methane emissions to the atmosphere.^[43] One study reported that the livestock sector in general (primarily cattle, chickens, and pigs) produces 37% of all human-induced methane.^[44] Early research has found a number of medical treatments and dietary adjustments that help slightly limit the production of methane in ruminants.^[45][46] A more recent study, in 2009, found that at a conservative estimate, at least 51% of global greenhouse gas emissions were attributable to the life cycle and supply chain of livestock products, meaning all meat, dairy, and by-products, and their transportation.^[47] Many efforts are underway to reduce livestock methane production and trap the gas to use as energy.^[48]

Paleoclimatology research published in Current Biology suggests that flatulence from dinosaurs may have warmed the Earth.^[49]

Atmospheric methane

2011 methane concentration in the upper troposphere^[50]

Methane is created near the Earth's surface, primarily by microorganisms by the process of methanogenesis. It is carried into the stratosphere by rising air in the tropics. Uncontrolled build-up of methane in the atmosphere is naturally checked – although human influence can upset this natural regulation – by methane's reaction with hydroxyl radicals formed from singlet oxygen atoms and with water vapor. It has a net lifetime of about 10 years,^[51] and is primarily removed by conversion to carbon dioxide and water.

Methane also affects the degradation of the ozone layer.^[52][53]

In addition, there is a large (but unknown) amount of methane in methane clathrates in the ocean floors as well as the Earth's crust. Most methane is the result of biological process called methanogenesis.

In 2010, methane levels in the Arctic were measured at 1850 nmol/mol, a level over twice as high as at any time in the 400,000 years prior to the industrial revolution. Historically, methane concentrations in the world's atmosphere have ranged between 300 and 400 nmol/mol during glacial periods commonly known as ice ages, and between 600 to 700 nmol/mol during the warm interglacial periods. Recent research suggests that the Earth's oceans are a potentially important new source of Arctic methane.^[54]

A

Molecules detected in outer space Molecules Diatomic Aluminium monochloride Aluminium monofluoride Aluminium monoxide Argon hydride Carbon monophosphide Carbon monosulfide Carbon monoxide Carborundum Cyanogen radical Diatomic carbon Fluoromethylidynium Hydrogen chloride Hydrogen fluoride Hydrogen (molecular) Hydroxyl radical Iron(II) oxide Magnesium monohydride cation Methylidyne radical Nitric oxide Nitrogen (molecular) Nitrogen monohydride Nitrogen sulfide Oxygen (molecular) Phosphorus monoxide Phosphorus nitride Potassium chloride Silicon carbide Silicon mononitride Silicon monoxide Silicon monosulfide Sodium chloride Sodium iodide Sulfur monohydride Sulfur monoxide Titanium oxide Triatomic Aluminium hydroxide Aluminium isocyanide Amino radical Carbon dioxide Carbonyl sulfide CCP radical Chloronium Diazenylium Dicarbon monoxide Ethynyl radical Formyl radical Hydrogen cyanide Hydrogen isocyanide (HCN) Hydrogen isocyanide (HNC) Hydrogen sulfide Hydroperoxyl Iron cyanide Isoformyl Magnesium cyanide Magnesium isocyanide Methylene radical N2H+ Nitrous oxide Nitroxyl Ozone Phosphaethyne Potassium cyanide Protonated molecular hydrogen Sodium cyanide Sodium hydroxide Silicon carbonitride c-Silicon dicarbide Silicon naphthalocyanine Sulfur dioxide Thioformyl Thioxoethenylidene Titanium dioxide Tricarbon Water Four atoms Acetylene Ammonia Cyanic acid Cyanoethynyl Cyclopropynylidyne Formaldehyde Fulminic acid HCCN Hydrogen peroxide Hydromagnesium isocyanide Isocyanic acid Isothiocyanic acid Methylene amidogen Methyl radical Propynylidyne Protonated carbon dioxide Protonated hydrogen cyanide Silicon tricarbide Thioformaldehyde Tricarbon monoxide Tricarbon sulfide Thiocyanic acid Five atoms Ammonium Ion Butadiynyl Carbodiimide Cyanamide Cyanoacetylene Cyanoformaldehyde Cyanomethyl Cyclopropenylidene Formic acid Isocyanoacetylene Ketene Methane Methoxy radical Methylenimine Propadienylidene Protonated formaldehyde Protonated formaldehyde Silane Silicon-carbide cluster Six atoms Acetonitrile Cyanobutadiynyl radical E-Cyanomethanimine Cyclopropenone Diacetylene Ethylene Formamide HC4N Ketenimine Methanethiol Methanol Methyl isocyanide Pentynylidyne Propynal Protonated cyanoacetylene Seven atoms Acetaldehyde Acrylonitrile Cyanodiacetylene Ethylene oxide Hexatriynyl radical Methylacetylene Methylamine Vinyl alcohol Eight atoms Acetic acid Aminoacetonitrile Cyanoallene Ethanimine Glycolaldehyde Heptatrienyl radical Hexapentaenylidene Methylcyanoacetylene Methyl formate Propenal Nine atoms Acetamide Cyanohexatriyne Cyanotriacetylene Dimethyl ether Ethanol Methyldiacetylene Octatetraynyl radical Propene Propionitrile Ten atoms or more Acetone Benzene Buckminsterfullerene (C60 fullerene) ("bucky-ball") C70 fullerene Cyanodecapentayne Cyanopentaacetylene Cyanotetra-acetylene Ethylene glycol Ethyl formate Methyl acetate Methyl-cyano-diacetylene Methyltriacetylene Propanal n-Propyl cyanide Deuterated molecules Ammonia Ammonium ion Formaldehyde Formyl radical Heavy water Hydrogen cyanide Hydrogen deuteride Hydrogen isocyanide Methylacetylene N2D+ Trihydrogen cation Unconfirmed Anthracene Dihydroxyacetone Ethyl methyl ether Glycine Graphene H2NCO+ Linear C5 Naphthalene cation Phosphine Pyrene Silylidine Related Abiogenesis Astrobiology Astrochemistry Atomic and molecular astrophysics Chemical formula Circumstellar envelope Cosmic dust Cosmic ray Cosmochemistry Diffuse interstellar band Extraterrestrial life Extraterrestrial liquid water Forbidden mechanism Helium hydride ion Homochirality Intergalactic dust Interplanetary medium Interstellar medium Iron–sulfur world theory Kerogen Life Organic compound Outer space PAH world hypothesis Panspermia Polycyclic aromatic hydrocarbon (PAH) RNA world hypothesis Spectroscopy Tholin Book:Chemistry Category:Astrochemistry Category:Molecules Portal:Astrobiology Portal:Chemistry

Fuel gas Types Manufactured fuel gas (History) Coal gas (Coal gasification) Producer gas Wood gas Water gas Mond gas Pintsch gas Syngas Blau gas Biogas Gasification Regasification Landfill gas Blast furnace gas Natural gas APG CBM CNG LNG HCNG NGC SNG Bio-SNG LPG Propane Butane Autogas Infrastructure Compressor station Gas carrier Gas holder Gas meter Gas works Natural-gas processing Natural gas storage Odorizer Pipeline transport Uses Gas lighting (Gas mantle) Gas stove Gas heater Gas burner Gas engine Gas turbine Bunsen burner Pilot light

• Methane at The Periodic Table of Videos (University of Nottingham)
• Methane thermodynamics
• International Chemical Safety Card 0291
• Methane Hydrates
• Safety data for methane
• Catalytic conversion of methane to more useful chemicals and fuels
• CDC – Handbook for Methane Control in Mining

External links

References

Notes

See also

• Uranus – the atmosphere contains 2.3% methane^[98]
  • Ariel – methane is believed to be a constituent of Ariel's surface ice
  • Miranda
  • Oberon – about 20% of Oberon's surface ice is composed of methane-related carbon/nitrogen compounds
  • Titania – about 20% of Titania's surface ice is composed of methane-related organic compounds
  • Umbriel – methane is a constituent of Umbriel's surface ice
• Neptune – the atmosphere contains 1.5 ± 0.5% methane^[99]
  • Triton – Triton has a tenuous nitrogen atmosphere with small amounts of methane near the surface.^[100][101]
• Pluto – spectroscopic analysis of Pluto's surface reveals it to contain traces of methane^[102][103]
  • Charon – methane is believed present on Charon, but it is not completely confirmed^[104]
• Eris – infrared light from the object revealed the presence of methane ice^[105]
• Halley's Comet
• Comet Hyakutake – terrestrial observations found ethane and methane in the comet^[106]
• [108]
• Interstellar clouds^[109]

Polar clouds, made of methane, on Titan (left) compared with polar clouds on Earth (right).

• Mars – the Martian atmosphere contains 10 nmol/mol methane.^[69] The source of methane on Mars has not been determined. Recent research suggests that methane may come from volcanoes, fault lines, or methanogens,^[70] or that it may be a byproduct of electrical discharges from dust devils and dust storms,^[71] or that it may be the result of UV radiation.^[72] In January 2009, NASA scientists announced that they had discovered that the planet often vents methane into the atmosphere in specific areas, leading some to speculate this may be a sign of biological activity going on below the surface.^[73] Analysis of observations made by a Weather Research and Forecasting model for Mars (MarsWRF) and related Mars general circulation model (MGCM) suggests that it is potentially possible to isolate methane plume source locations to within tens of kilometers, which is within the roving capabilities of future Mars rovers.^[74] The Curiosity rover, which landed on Mars in August 2012, is able to make measurements that distinguish between different isotopologues of methane;^[75] but even if the mission is to determine that microscopic Martian life is the source of the methane, the life forms likely reside far below the surface, outside of the rover's reach.^[76] Curiosity’s Sample Analysis at Mars (SAM) instrument is capable of tracking the presence of methane over time to determine if it is constant, variable, seasonal, or random, providing further clues about its source.^[77] The first measurements with the Tunable Laser Spectrometer (TLS) indicated that there is less than 5 ppb of methane at the landing site at the point of the measurement.^{[78][79][80][81]} The Mars Trace Gas Mission orbiter planned to launch in 2016 would further study the methane,^[82][83] as well as its decomposition products such as formaldehyde and methanol. Alternatively, these compounds may instead be replenished by volcanic or other geological means, such as serpentinization.^[42] On July 19, 2013, NASA scientists reported finding "not much methane" (i.e., "an upper limit of 2.7 parts per billion of methane") around the Gale Crater area where the Curiosity rover landed in August 2012.^[84][85][86] On September 19, 2013, NASA scientists, on the basis of further measurements by Curiosity, reported no detection of atmospheric methane with a measured value of 0.18±0.67 ppbv corresponding to an upper limit of only 1.3 ppbv (95% confidence limit) and, as a result, conclude that the probability of current methanogenic microbial activity on Mars is reduced.^[87][88][89]
• Saturn – the atmosphere contains 4500 ± 2000 ppm methane^[90]
  • Enceladus – the atmosphere contains 1.7% methane^[91]
  • Iapetus
  • Titan – the atmosphere contains 1.6% methane and thousands of methane lakes have been detected on the surface.^[92] In the upper atmosphere the methane is converted into more complex molecules including acetylene, a process that also produces molecular hydrogen. There is evidence that acetylene and hydrogen are recycled into methane near the surface. This suggests the presence either of an exotic catalyst, or an unfamiliar form of methanogenic life.^[93] An apparent lake of liquid methane has been spotted by the Cassini-Huygens probe, causing researchers to speculate about the possibility of life on Titan.^[94] Methane showers, probably prompted by changing seasons, have also been observed.^[95] On October 24, 2014, methane was found in polar clouds on Titan.^[96][97]

Methane on Mars – "potential sources and sinks" (November 2, 2012).

• Mercury – the tenuous atmosphere contains trace amounts of methane.^[66]
• Venus – the atmosphere contains a large amount of methane from 60 km (37 mi) to the surface according to data collected by the Pioneer Venus Large Probe Neutral Mass Spectrometer^[67]
• Moon – traces are outgassed from the surface^[68]

Methane has been detected or is believed to exist on all planets of the solar system, as well as on most of the larger moons. In most cases, it is believed to have been created by abiotic processes. Possible exceptions are Mars and Titan.

Extraterrestrial methane

Methane gas explosions are responsible for many deadly mining disasters.^[64] A methane gas explosion was the cause of the Upper Big Branch coal mine disaster in West Virginia on April 5, 2010, killing 25.^[65]

Methane is not toxic, yet it is extremely flammable and may form explosive mixtures with air. Methane is violently reactive with oxidizers, halogen, and some halogen-containing compounds. Methane is also an asphyxiant and may displace oxygen in an enclosed space. Asphyxia may result if the oxygen concentration is reduced to below about 16% by displacement, as most people can tolerate a reduction from 21% to 16% without ill effects. The concentration of methane at which asphyxiation risk becomes significant is much higher than the 5–15% concentration in a flammable or explosive mixture. Methane off-gas can penetrate the interiors of buildings near landfills and expose occupants to significant levels of methane. Some buildings have specially engineered recovery systems below their basements to actively capture this gas and vent it away from the building.

Safety

Arctic methane release from permafrost and methane clathrates is an expected consequence and further cause of global warming.^[61][62][63]

Methane is essentially insoluble in water, but it can be trapped in ice forming a similar solid. Significant deposits of methane clathrate have been found under sediments on the ocean floors of Earth at large depths.

Clathrates

Methane has a large effect for a brief period (a net lifetime of 8.4 years in the atmosphere), whereas carbon dioxide has a small effect for a long period (over 100 years). Because of this difference in effect and time period, the global warming potential of methane over a 20-year time period is 72. The Earth's atmospheric methane concentration has increased by about 150% since 1750, and it accounts for 20% of the total radiative forcing from all of the long-lived and globally mixed greenhouse gases (these gases don't include water vapor which is by far the largest component of the greenhouse effect).^[60] Usually, excess methane from landfills and other natural producers of methane is burned so CO₂ is released into the atmosphere instead of methane, because methane is a more effective greenhouse gas. Recently, methane emitted from coal mines has been successfully utilized to generate electricity.

The IPCC Fifth Assessment Report determined that methane in the Earth's atmosphere is an important greenhouse gas with a global warming potential of 34 compared to CO₂ over a 100-year period (although accepted figures probably represent an underestimate^[57][58]). This means that a methane emission will have 34 times the effect on temperature of a carbon dioxide emission of the same mass over the following 100 years. And methane has 33 times the effect when accounted for aerosol interactions.^[59]

^[56] Possible adverse effects projected as the gas escapes into the atmosphere are estimated to have the potential of a sixty trillion dollar impact on the world economy.[55]