.
MEH-thayn
MEE-thayn
.
“natural gas”
.
*’methane’ is a ‘chemical compound’ with the chemical formula CH4*
1 ‘carbon atom’ bonded to 4 ‘hydrogen atoms’
.
It is a group-14 hydride, the simplest alkane, and the main constituent of natural gas.
The relative abundance of methane on Earth makes it an economically attractive fuel,
although capturing and storing it poses technical challenges due to its gaseous state under normal conditions for temperature and pressure
Naturally occurring methane is found both below ground and under the seafloor and is formed by both geological and biological processes.
The largest reservoir of methane is under the seafloor in the form of methane clathrates.
When methane reaches the surface and the atmosphere, it is known as atmospheric methane.[9] 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.[10] It has also been detected on other planets, including Mars, which has implications for astrobiology research.[11]
Properties and bonding[edit]
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 energy level 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.
Methane is an odorless gas and appears to be colorless.[12] It does absorb visible light especially at the red end of the spectrum due to overtone bands, but the effect is only noticeable if the light path is very long. This is what gives Uranus and Neptune their blue or bluish-green colors, as light passes through their atmospheres containing methane and is then scattered back out.[13]
The familiar smell of natural gas as used in homes is achieved by the addition of an odorant, usually blends containing tert-butylthiol, as a safety measure. Methane has a boiling point of −161.5 °C at a pressure of one atmosphere.[3] As a gas, it is flammable over a range of concentrations (5.4–17%) in air at standard pressure.
Solid methane exists in several modifications. Presently nine are known.[14] Cooling methane at normal pressure results in the formation of methane I. This substance crystallizes in the cubic system (space group Fm3m). The positions of the hydrogen atoms are not fixed in methane I, i.e. methane molecules may rotate freely.
Therefore, it is a plastic crystal
.
Chemical reactions
The primary chemical reactions of methane are combustion, steam reforming to syngas, and halogenation.
In general, methane reactions are difficult to control
.
Selective oxidation
Partial oxidation of methane to methanol, a more convenient, liquid fuel, is challenging because the reaction typically progresses all the way to carbon dioxide and water even with an insufficient supply of oxygen.
The enzyme ‘methane mono-oxygenase’ produces ‘methanol’ from ‘methane’, but cannot be used for ‘industrial-scale reactions’
Some homogeneously catalyzed systems and heterogeneous systems have been developed, but all have significant drawbacks.
These generally operate by generating protected products which are shielded from overoxidation.
Examples include the Catalytica system, copper zeolites, and iron zeolites stabilizing the alpha-oxygen active site.[17]
One group of bacteria catalyze methane oxidation with nitrite as the oxidant in the absence of oxygen, giving rise to the so-called anaerobic oxidation of methane.[18]
Acid–base reactions[edit]
Like other hydrocarbons, methane is an extremely weak acid. Its pKa in DMSO is estimated to be 56.[19] It cannot be deprotonated in solution, but the conjugate base is known in forms such as methyllithium.
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+
- Some of these have been detected in outer space. Methanium can also be produced as diluted solutions from methane with superacids. Cations with higher charge, such as CH2+
6 and CH3+
7, have been studied theoretically and conjectured to be stable.[20]
Despite the strength of its C–H bonds, there is intense interest in catalysts that facilitate C–H bond activation in methane (and other lower numbered alkanes).[21]
Combustion[edit]
A young woman holding a flame in her hands
Methane bubbles can be burned on a wet hand without injury.
Methane’s heat of combustion is 55.5 MJ/kg.[22] Combustion of methane is a multiple step reaction summarized as follows:
CH4 + 2 O2 → CO2 + 2 H2O (ΔH = −891 k J/mol, at standard conditions)
Peters four-step chemistry is a systematically reduced four-step chemistry that explains the burning of methane.
Methane radical reactions[edit]
Given appropriate conditions, methane reacts with halogen radicals as follows:
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 when UV light or some other radical initiator (like peroxides) produces a halogen atom. A two-step chain reaction ensues in which the halogen atom abstracts a hydrogen atom from a methane molecule, resulting in the formation of a hydrogen halide molecule and a methyl radical (CH3•). The methyl radical then reacts with a molecule of the halogen to form a molecule of the halomethane, with a new halogen atom as byproduct.[23] Similar reactions can occur on the halogenated product, leading to replacement of additional hydrogen atoms by halogen atoms with dihalomethane, trihalomethane, and ultimately, tetrahalomethane structures, depending upon reaction conditions and the halogen-to-methane ratio.
Uses[edit]
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[edit]
Methane is used as a fuel for ovens, homes, water heaters, kilns, automobiles,[24][25] turbines, etc. Activated carbon is used to store methane. Refined liquid methane is used as a rocket fuel,[26] when combined with liquid oxygen, as in the BE-4 and Raptor engines.[27]
As the major constituent of natural gas, methane is important for electricity generation by burning it as a fuel in a gas turbine or steam generator.
Compared to other hydrocarbon fuels, methane produces less carbon dioxide for each unit of heat released. At about 891 kJ/mol, methane’s heat of combustion is lower than that of any other hydrocarbon. However, it produces more heat per mass (55.7 kJ/g) than any other organic molecule due to its relatively large content of hydrogen, which accounts for 55% of the heat of combustion[28] but contributes only 25% of the molecular mass of methane. In many cities, methane is piped into homes for domestic heating and cooking. 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. Liquefied natural gas (LNG) is predominantly methane (CH4) converted into liquid form for ease of storage or transport.
As a liquid rocket fuel, methane offers the advantage over kerosene of producing small exhaust molecules. This deposits less soot on the internal parts of rocket motors, reducing the difficulty of booster re-use. The lower molecular weight of the exhaust also increases the fraction of the heat energy which is in the form of kinetic energy available for propulsion, increasing the specific impulse of the rocket.
Liquid methane also has a temperature range (91–112 K) nearly compatible with liquid oxygen (54–90 K)
.
Chemical feedstock
Natural gas, which is mostly composed of methane, is used to produce hydrogen gas on an industrial scale
Steam methane reforming (SMR), or simply known as steam reforming, is the standard industrial method of producing commercial bulk hydrogen gas.
More than 50 million metric tons are produced annually worldwide (2013), principally from the SMR of natural gas
Much of this hydrogen is used in petroleum refineries, in the production of chemicals and in food processing.
Very large quantities of hydrogen are used in the industrial synthesis of ammonia.
At high temperatures (700–1100 °C) and in the presence of a metal-based catalyst (nickel), steam reacts with methane to yield a mixture of CO and H2, known as “water gas” or “syngas”
CH4 + H2O ⇌ CO + 3 H2
This reaction is strongly endothermic (consumes heat, ΔHr = 206 kJ/mol). Additional hydrogen is obtained by the reaction of CO with water via the water-gas shift reaction:
CO + H2O ⇌ CO2 + H2
This reaction is mildly exothermic (produces heat, ΔHr = −41 kJ/mol).
Methane is also subjected to free-radical chlorination in the production of chloromethanes, although methanol is a more typical precursor.[30]
Generation[edit]
Geological routes[edit]
The two main routes for geological methane generation are (i) organic (thermally generated, or thermogenic) and (ii) inorganic (abiotic).[11] Thermogenic methane occurs due to the breakup of organic matter at elevated temperatures and pressures in deep sedimentary strata. Most methane in sedimentary basins is thermogenic; therefore, thermogenic methane is the most important source of natural gas. Thermogenic methane components are typically considered to be relic (from an earlier time). Generally, formation of thermogenic methane (at depth) can occur through organic matter breakup, or organic synthesis. Both ways can involve microorganisms (methanogenesis), but may also occur inorganically. The processes involved can also consume methane, with and without microorganisms.
The more important source of methane at depth (crystalline bedrock) is abiotic. Abiotic means that methane is created from inorganic compounds, without biological activity, either through magmatic processes or via water-rock reactions that occur at low temperatures and pressures, like serpentinization.[31][32]
Biological routes[edit]
Most of Earth’s methane is biogenic and is produced by methanogenesis,[33][34] a form of anaerobic respiration only known to be conducted by some members of the domain Archaea.[35] Methanogens occupy landfills and other soils,[36] ruminants (for example, cattle),[37] the guts of termites, and the anoxic sediments below the seafloor and the bottom of lakes. Rice fields also generate large amounts of methane during plant growth.[38] This multistep process is used by these microorganisms for energy. The net reaction of methanogenesis is:
CO2 + 4 H2→ CH4 + 2 H2O
The final step in the process is catalyzed by the enzyme methyl coenzyme M reductase (MCR).[39]
Testing Australian sheep for exhaled methane production (2001), CSIRO
This image represents a ruminant, specifically a sheep, producing methane in the four stages of hydrolysis, acidogenesis, acetogenesis, and methanogenesis.
Ruminants[edit]
Ruminants, such as cattle, belch methane, accounting for about 22% of the U.S. annual methane emissions to the atmosphere.[40] One study reported that the livestock sector in general (primarily cattle, chickens, and pigs) produces 37% of all human-induced methane.[41] A 2013 study estimated that livestock accounted for 44% of human-induced methane and about 15% of human-induced greenhouse gas emissions.[42] Many efforts are underway to reduce livestock methane production, such as medical treatments and dietary adjustments,[43][44] and to trap the gas to use its combustion energy.[45]
Seafloor sediments[edit]
Most of the subseafloor is anoxic because oxygen is removed by aerobic microorganisms within the first few centimeters of the sediment. Below the oxygen-replete seafloor, methanogens produce methane that is either used by other organisms or becomes trapped in gas hydrates.[35] These other organisms that utilize methane for energy are known as methanotrophs (‘methane-eating’), and are the main reason why little methane generated at depth reaches the sea surface.[35] Consortia of Archaea and Bacteria have been found to oxidize methane via anaerobic oxidation of methane (AOM); the organisms responsible for this are anaerobic methanotrophic Archaea (ANME) and sulfate-reducing bacteria (SRB).[46]
Industrial routes[edit]
Given its cheap abundance in natural gas, there is little incentive to produce methane industrially. 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, which is practiced on a large scale to produce longer-chain molecules than methane.
An example of large-scale coal-to-methane gasification 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 that is otherwise difficult to transport for its weight, ash content, low calorific value and propensity to spontaneous combustion during storage and transport. A number of similar plants exist around the world, although mostly these plants are targeted towards the production of long chain alkanes for use as gasoline, diesel, or feedstock to other processes.
Power to methane is a technology that uses electrical power to produce hydrogen from water by electrolysis and uses the Sabatier reaction to combine hydrogen with carbon dioxide to produce methane. As of 2021, this is mostly under development and not in large-scale use. Theoretically, the process could be used as a buffer for excess and off-peak power generated by highly fluctuating wind turbines and solar arrays. However, as currently very large amounts of natural gas are used in power plants (e.g. CCGT) to produce electric energy, the losses in efficiency are not acceptable.
Laboratory synthesis[edit]
Methane can be produced by protonation of methyl lithium or a methyl Grignard reagent such as methylmagnesium chloride. It can also be made from anhydrous sodium acetate and dry sodium hydroxide, mixed and heated above 300 °C (with sodium carbonate as byproduct).[citation needed] In practice, a requirement for pure methane can easily be fulfilled by steel gas bottle from standard gas suppliers.
Occurrence[edit]
Methane was discovered and isolated by Alessandro Volta between 1776 and 1778 when studying marsh gas from Lake Maggiore. It is the major component of natural gas, about 87% by volume. The major source of methane is extraction from geological deposits known as natural gas fields, with coal seam gas extraction becoming a major source (see coal bed methane extraction, a method for extracting methane from a coal deposit, while enhanced coal bed methane recovery is a method of recovering methane from non-mineable coal seams). It is associated with other hydrocarbon fuels, and sometimes accompanied by helium and nitrogen. Methane is produced at shallow levels (low pressure) by anaerobic decay of organic matter and reworked methane from deep under the Earth’s surface. In general, the sediments that generate natural gas are buried deeper and at higher temperatures than those that contain oil.
Methane is generally transported in bulk by pipeline in its natural gas form, or by LNG carriers in its liquefied form; few countries transport it by truck.
Atmospheric methane[edit]
Methane (CH4) measured by the Advanced Global Atmospheric Gases Experiment (AGAGE) in the lower atmosphere (troposphere) at stations around the world. Abundances are given as pollution free monthly mean mole fractions in parts-per-billion.
In 2010, methane levels in the Arctic were measured at 1850 nmol/mol. This level is over twice as high as at any time in the last 400,000 years. Historic 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 and 700 nmol/mol during the warm interglacial periods. The Earth’s oceans are a potential important source of Arctic methane.[47]
Methane is an important greenhouse gas with a global warming potential of 34 compared to CO2 (potential of 1) over a 100-year period, and 72 over a 20-year period.[48][49]
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. The AR6 of the IPCC states: “Observed increases in well-mixed greenhouse gas (GHG) concentrations since around 1750 are unequivocally caused by human activities. Since 2011 (measurements reported in AR5), concentrations have continued to increase in the atmosphere, reaching annual averages of 410 ppm for carbon dioxide (CO2), 1866 ppb for methane (CH4), and 332 ppb for nitrous oxide (N2O) in 2019. (…) In 2019, atmospheric CO2 concentrations were higher than at any time in at least 2 million years (high confidence), and concentrations of CH4 and N2O were higher than at any time in at least 800,000 years (very high confidence). Since 1750, increases in CO2 (47%) and CH4 (156%) concentrations far exceed, and increases in N2O (23%) are similar to, the natural multi-millennial changes between glacial and interglacial periods over at least the past 800,000 years (very high confidence)”.[10]
From 2015 to 2019 sharp rises in levels of atmospheric methane have been recorded.[50][51] In February 2020, it was reported that fugitive emissions and gas venting from the fossil fuel industry may have been significantly underestimated.[52]
Climate change can increase atmospheric methane levels by increasing methane production in natural ecosystems, forming a Climate change feedback.[35][53]
Clathrates[edit]
Methane clathrates (also known as methane hydrates) are solid cages of water molecules that trap single molecules of methane. Significant reservoirs of methane clathrates have been found in arctic permafrost and along continental margins beneath the ocean floor within the gas clathrate stability zone, located at high pressures (1 to 100 MPa; lower end requires lower temperature) and low temperatures (< 15 °C; upper end requires higher pressure).[54] Methane clathrates can form from biogenic methane, thermogenic methane, or a mix of the two. These deposits are both a potential source of methane fuel as well as a potential contributor to global warming.[55][56] The global mass of carbon stored in gas clathrates is still uncertain and has been estimated as high as 12,500 Gt carbon and as low as 500 Gt carbon.[57] The estimate has declined over time with a most recent estimate of ~1800 Gt carbon.[58] A large part of this uncertainty is due to our knowledge gap in sources and sinks of methane and the distribution of methane clathrates at the global scale. For example, a source of methane was discovered relatively recently in an ultraslow spreading ridge in the Arctic.[59] Some climate models suggest that today’s methane emission regime from the ocean floor is potentially similar to that during the period of the Paleocene–Eocene Thermal Maximum (PETM) around 55.5 million years ago, although there are no data indicating that methane from clathrate dissociation currently reaches the atmosphere.[58] Arctic methane release from permafrost and seafloor methane clathrates is a potential consequence and further cause of global warming; this is known as the clathrate gun hypothesis.[60][61][62][63] Data from 2016 indicate that Arctic permafrost thaws faster than predicted.[64]
[edit]
Interstellar medium[edit]
Methane is abundant in many parts of the Solar System and potentially could be harvested on the surface of another solar-system body (in particular, using methane production from local materials found on Mars[65] or Titan), providing fuel for a return journey.[26][66]
Mars[edit]
Methane has been detected on all planets of the Solar System and most of the larger moons.[citation needed] With the possible exception of Mars, it is believed to have come from abiotic processes.[67][68]
Methane (CH4) on Mars – potential sources and sinks
The Curiosity rover has documented seasonal fluctuations of atmospheric methane levels on Mars. These fluctuations peaked at the end of the Martian summer at 0.6 parts per billion.[69][70][71][72][73][74][75][76]
Methane has been proposed as a possible rocket propellant on future Mars missions due in part to the possibility of synthesizing it on the planet by in situ resource utilization.[77] An adaptation of the Sabatier methanation reaction may be used with 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.[65]
Methane could be produced by a non-biological process called serpentinization[a] involving water, carbon dioxide, and the mineral olivine, which is known to be common on Mars.[78]
History[edit]
In November 1776, methane was first scientifically identified by Italian physicist Alessandro Volta in the marshes of Lake Maggiore straddling Italy and Switzerland. Volta was inspired to search for the substance after reading a paper written by Benjamin Franklin about “flammable air”.[79] Volta collected the gas rising from the marsh, and by 1778 had isolated pure methane.[80] He also demonstrated that the gas could be ignited with an electric spark.[80]
Following the Felling mine disaster of 1812 in which 92 men perished, Sir Humphry Davy established that the feared firedamp was in fact largely methane.[81]
The name “methane” was coined in 1866 by the German chemist August Wilhelm von Hofmann.[82][83] The name was derived from methanol.
Etymology[edit]
Etymologically, the word “methane” is coined from the chemical suffix “-ane”, which denotes substances belonging to the alkane family; and the word “methyl”, which is derived from the German “methyl” (1840) or directly from the French “méthyle”, which is a back-formation from the French “méthylène” (corresponding to English “methylene”), the root of which was coined by Jean-Baptiste Dumas and Eugène Péligot in 1834 from the Greek “methy” (wine) (related to English “mead”) and “hyle” (meaning “wood”). The radical is named after this because it was first detected in methanol, an alcohol first isolated by distillation of wood. The chemical suffix “-ane” is from the coordinating chemical suffix “-ine” which is from Latin feminine suffix “-ina” which is applied to represent abstracts. The coordination of “-ane”, “-ene”, “-one”, etc. was proposed in 1866 by German chemist August Wilhelm von Hofmann (1818–1892).[84]
Abbreviations[edit]
The abbreviation CH4-C can mean the mass of carbon contained in a mass of methane, and the mass of methane is always 1.33 times the mass of CH4-C.[85][86] CH4-C can also mean the methane-carbon ratio, which is 1.33 by mass.[87] Methane at scales of the atmosphere is commonly measured in teragrams (Tg CH4) or millions of metric tons (MMT CH4), which mean the same thing.[88] Other standard units are also used, such as nanomole (nmol, one billionth of a mole), mole (mol), kilogram, and gram.
Safety[edit]
Methane is nontoxic, yet it is extremely flammable and may form explosive mixtures with air. Methane is also an asphyxiant 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.
Methane gas explosions are responsible for many deadly mining disasters.[89] A methane gas explosion was the cause of the Upper Big Branch coal mine disaster in West Virginia on April 5, 2010, killing 29.[90]
See also[edit]
2007 Zasyadko mine disaster
Abiogenic petroleum origin
Aerobic methane production
Anaerobic digestion
Anaerobic respiration
Arctic methane emissions
Biogas
Coal Oil Point seep field
Energy density
Fugitive gas emissions
Global Methane Initiative
Thomas Gold
Halomethane, halogenated methane derivatives.
Hydrogen Cycle
Industrial gas
Lake Kivu (more general: limnic eruption)
List of straight-chain alkanes
Methanation
Methane emissions
Methane on Mars:
atmosphere
climate
Methanogen, archaea that produce methane.
Methanogenesis, microbes that produce methane.
Methanotroph, bacteria that grow with methane.
Methyl group, a functional group related to methane.
Explanatory notes[edit]
^ There are many serpentinization reactions. Olivine is a solid solution between forsterite and fayalite whose general formula is (Fe,Mg)2SiO4. The reaction producing methane from olivine can be written as: Forsterite + Fayalite + Water + Carbonic acid → Serpentine + Magnetite + Methane , or (in balanced form): 18 Mg2SiO4 + 6 Fe2SiO4 + 26 H2O + CO2 → 12 Mg3Si2O5(OH)4 + 4 Fe3O4 + CH4
Citations[edit]
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Cited sources[edit]
Haynes, William M., ed. (2016). CRC Handbook of Chemistry and Physics (97th ed.). CRC Press. ISBN 9781498754293.
External links[edit]
Wikimedia Commons has media related to Methane.
Look up methane in Wiktionary, the free dictionary.
Methane at The Periodic Table of Videos (University of Nottingham)
International Chemical Safety Card 0291
Gas (Methane) Hydrates – A New Frontier – United States Geological Survey
Lunsford, Jack H. (2000). “Catalytic conversion of methane to more useful chemicals and fuels: A challenge for the 21st century”. Catalysis Today. 63 (2–4): 165–174. doi:10.1016/S0920-5861(00)00456-9.
CDC – Handbook for Methane Control in Mining
en.wikipedia.org /wiki/Methane
Methane
Contributors to Wikimedia projects45-56 minutes 8/10/2001
DOI: 10.1039/9781849733069-fp001, Show Details
For the emergency service protocol, see ETHANE.
Methane
Stereo, skeletal formula of methane with some measurements added
Ball and stick model of methane
Spacefill model of methane
Names
Preferred IUPAC name
Methane[1]
Systematic IUPAC name
Carbane (never recommended[1])
Other names
Marsh gas
Natural gas
Carbon tetrahydride
Hydrogen carbide
Identifiers
CAS Number
74-82-8 check
3D model (JSmol)
Interactive image
3DMet
B01453
Beilstein Reference
1718732
ChEBI
CHEBI:16183 check
ChEMBL
ChEMBL17564 check
ChemSpider
291 check
ECHA InfoCard 100.000.739 Edit this at Wikidata
EC Number
200-812-7
Gmelin Reference
59
KEGG
C01438 ☒
MeSH Methane
PubChem CID
297
RTECS number
PA1490000
UNII
OP0UW79H66 check
UN number 1971
CompTox Dashboard (EPA)
DTXSID8025545 Edit this at Wikidata
show
InChI
show
SMILES
Properties
Chemical formula
CH4
Molar mass 16.043 g·mol−1
Appearance Colorless gas
Odor Odorless
Density
0.657 kg·m−3 (gas, 25 °C, 1 atm)
0.717 kg·m−3 (gas, 0 °C, 1 atm)[2]
422.8 g·L−1 (liquid, −162 °C)[3]
Melting point −182.456 °C (−296.421 °F; 90.694 K)[3]
Boiling point −161.5 °C (−258.7 °F; 111.6 K)[3]
Critical point (T, P) 190.56 K, 4.5992 MPa
Solubility in water
22.7 mg·L−1[4]
Solubility Soluble in ethanol, diethyl ether, benzene, toluene, methanol, acetone and insoluble in water
log P 1.09
Henry’s law
constant (kH)
14 nmol·Pa−1·kg−1
Conjugate acid Methanium
Conjugate base Methyl anion
Magnetic susceptibility (χ)
−17.4×10−6 cm3·mol−1[5]
Structure
Point group
Td
Molecular shape
Tetrahedron
Dipole moment
0 D
Thermochemistry[6]
Heat capacity (C)
35.7 J·(K·mol)−1
Std molar
entropy (So298)
186.3 J·(K·mol)−1
Std enthalpy of
formation (ΔfH⦵298)
−74.6 kJ·mol−1
Gibbs free energy (ΔfG˚)
−50.5 kJ·mol−1
Std enthalpy of
combustion (ΔcH⦵298)
−891 kJ·mol−1
Hazards[7]
GHS labelling:
Pictograms
GHS02: Flammable
Signal word
Danger
Hazard statements
H220
Precautionary statements
P210
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
2
4
0
SA
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
Difluoromethane
Iodoform
Carbon tetrachloride
Supplementary data page
Methane (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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