Chemistry:Methanol

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Short description: CH3OH; simplest alcohol
Template:Chembox DeltaHc high
Methanol
Skeletal formula of methanol with some explicit hydrogens added
Spacefill model of methanol
Space filling model of methanol
Ball and stick model of methanol
A sample of methanol
Names
Preferred IUPAC name
Methanol[1]
Other names
Carbinol
Columbian spirits
Hydroxymethane
MeOH
Methyl alcohol
Methyl hydroxide
Methylic alcohol
Methylol
Methylene hydrate, primary alcohol
Pyroligneous spirit
Wood alcohol
Wood naphtha
Wood spirit
Identifiers
3D model (JSmol)
3DMet
1098229
ChEBI
ChEMBL
ChemSpider
EC Number
  • 200-659-6
449
KEGG
MeSH Methanol
RTECS number
  • PC1400000
UNII
UN number 1230
Properties
CH
3OH
Molar mass 32.042 g·mol−1
Appearance Colourless liquid
Odor Faint and similar to ethanol
Density 0.792 g/cm3[2]
Melting point −97.6 °C (−143.7 °F; 175.6 K)
Boiling point 64.7 °C (148.5 °F; 337.8 K)
miscible
log P −0.69
Vapor pressure 13.02 kPa (at 20 °C)
Acidity (pKa) 15.5[3]
Conjugate acid Methyloxonium[4]
Conjugate base Methanolate[5]
−21.40·10−6 cm3/mol
1.33141[6]
Viscosity 0.545 mPa·s (at 25 °C)[7]
1.69 D
Thermochemistry
Hazards[12][13]
Main hazards Methanol and its vapours are flammable.

Moderately toxic for small animals – Highly toxic to large animals and humans (in high concentrations) – May be fatal/lethal or cause blindness and damage to the liver, kidneys, and heart if swallowed – Toxicity effects from repeated over exposure have an accumulative effect on the central nervous system, especially the optic nerve – Symptoms may be delayed, become severe after 12 to 18 hours, and linger for several days after exposure[9]

Safety data sheet [1]
GHS pictograms GHS02: FlammableGHS06: ToxicGHS08: Health hazard[8]
GHS Signal word Danger[8]
H225, H301, H302, H305, H311, H331, H370[8]
P210, P233, P240, P241, P242, P243, P260, P264, P270, P271, P280, P301+330+331, P310, P302+352, P312, P303+361+353, P304+340, P311, P305+351+338, P307+311, P337+313, P361, P363, P370+378, P403+233[8]
NFPA 704 (fire diamond)
Flash point 11 to 12 °C (52 to 54 °F; 284 to 285 K)
470 °C (878 °F; 743 K)[15]

385 °C (725 °F; 658 K)[16]

Explosive limits 6–36%[10]
Lethal dose or concentration (LD, LC):
5628 mg/kg (rat, oral)
7300 mg/kg (mouse, oral)
12880 mg/kg (rat, oral)
14200 mg/kg (rabbit, oral)[11]
64,000 ppm (rat, 4 h)[11]
33,082 ppm (cat, 6 h)
37,594 ppm (mouse, 2 h)[11]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 200 ppm (260 mg/m3)[10]
REL (Recommended)
 TWA 200 ppm (260 mg/m3) ST 250 ppm (325 mg/m3) [skin][10]
IDLH (Immediate danger)
 6000 ppm[10]
Related compounds
Related compounds
 Methanethiol
Silanol
Ethanol
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references

Methanol (also called methyl alcohol and wood spirit, amongst other names) is an organic chemical compound and the simplest aliphatic alcohol, with the chemical formula CH
3OH (a methyl group linked to a hydroxyl group, often abbreviated as MeOH). It is a light, volatile, colorless and flammable liquid with a distinctive alcoholic odour similar to that of ethanol (potable alcohol).[17] Methanol acquired the name wood alcohol because it was once produced chiefly by the destructive distillation of wood. Today, methanol is mainly produced industrially by hydrogenation of carbon monoxide.[18]

Methanol consists of a methyl group linked to a polar hydroxyl group. With more than 20 million tons produced annually, it is used as a precursor to other commodity chemicals, including formaldehyde, acetic acid, methyl tert-butyl ether, methyl benzoate, anisole, peroxyacids, as well as a host of more specialised chemicals.[18]


Occurrence

Small amounts of methanol are present in normal, healthy human individuals. One study found a mean of 4.5 ppm in the exhaled breath of test subjects.[19] The mean endogenous methanol in humans of 0.45 g/d may be metabolized from pectin found in fruit; one kilogram of apple produces up to 1.4 g of pectin (0.6 g of methanol.)[20]

Methanol is produced by anaerobic bacteria and phytoplankton.[21][22]

Interstellar medium

Methanol is also found in abundant quantities in star-forming regions of space and is used in astronomy as a marker for such regions. It is detected through its spectral emission lines.[23]

In 2006, astronomers using the MERLIN array of radio telescopes at Jodrell Bank Observatory discovered a large cloud of methanol in space 463 terametres (288 billion miles) across.[24][25] In 2016, astronomers detected methanol in a planet-forming disc around the young star TW Hydrae using the Atacama Large Millimeter Array radio telescope.[26]

History

In their embalming process, the ancient Egyptians used a mixture of substances, including methanol, which they obtained from the pyrolysis of wood. Pure methanol, however, was first isolated in 1661 by Robert Boyle, when he produced it via the distillation of buxus (boxwood).[27] It later became known as "pyroxylic spirit". In 1834, the French chemists Jean-Baptiste Dumas and Eugene Peligot determined its elemental composition.[28]

They also introduced the word "methylène" to organic chemistry, forming it from Greek methy = "alcoholic liquid" + hȳlē = "forest, wood, timber, material". "Methylène" designated a "radical" that was about 14% hydrogen by weight and contained one carbon atom. This would be CH
2, but at the time carbon was thought to have an atomic weight only six times that of hydrogen, so they gave the formula as CH.[28] They then called wood alcohol (l'esprit de bois) "bihydrate de méthylène" (bihydrate because they thought the formula was C
4H
8O
4 or (CH)
4(H
2O)
2). The term "methyl" was derived in about 1840 by back-formation from "methylene", and was then applied to describe "methyl alcohol". This was shortened to "methanol" in 1892 by the International Conference on Chemical Nomenclature.[29] The suffix -yl, which, in organic chemistry, forms names of carbon groups, is from the word methyl.

French chemist Paul Sabatier presented the first process that could be used to produce methanol synthetically in 1905. This process suggested that carbon dioxide and hydrogen could be reacted to produce methanol.[9] German chemists Alwin Mittasch and Mathias Pier, working for Badische-Anilin & Soda-Fabrik (BASF), developed a means to convert synthesis gas (a mixture of carbon monoxide, carbon dioxide, and hydrogen) into methanol and received a patent. According to Bozzano and Manenti, BASF's process was first utilized in Leuna, Germany in 1923. Operating conditions consisted of "high" temperatures (between 300 and 400 °C) and pressures (between 250 and 350 atm) with a zinc/chromium oxide catalyst.[30]

US patent 1,569,775 ( US patent 1569775) was applied for on 4 Sep 1924 and issued on 12 January 1926 to BASF; the process used a chromium and manganese oxide catalyst with extremely vigorous conditions: pressures ranging from 50 to 220 atm, and temperatures up to 450 °C. Modern methanol production has been made more efficient through use of catalysts (commonly copper) capable of operating at lower pressures. The modern low pressure methanol (LPM) process was developed by ICI in the late 1960s US patent 3326956 with the technology patent long since expired.

During World War II, methanol was used as a fuel in several German military rocket designs, under the name M-Stoff, and in a roughly 50/50 mixture with hydrazine, known as C-Stoff.

The use of methanol as a motor fuel received attention during the oil crises of the 1970s. By the mid-1990s, over 20,000 methanol "flexible fuel vehicles" (FFV) capable of operating on methanol or gasoline were introduced in the U.S. In addition, low levels of methanol were blended in gasoline fuels sold in Europe during much of the 1980s and early-1990s. Automakers stopped building methanol FFVs by the late-1990s, switching their attention to ethanol-fueled vehicles. While the methanol FFV program was a technical success, rising methanol pricing in the mid- to late-1990s during a period of slumping gasoline pump prices diminished interest in methanol fuels.[31]

In the early 1970s, a process was developed by Mobil for producing gasoline fuel from methanol.[32]

Between the 1960s and 1980s methanol emerged as a precursor to the feedstock chemicals acetic acid and acetic anhydride. These processes include the Monsanto acetic acid synthesis, Cativa process, and Tennessee Eastman acetic anhydride process.

Applications

Production of formaldehyde, acetic acid, methyl tert-butyl ether

Methanol is primarily converted to formaldehyde, which is widely used in many areas, especially polymers. The conversion entails oxidation:

2 CH
3OH + O
2 → 2 CH
2O + 2 H
2O

Acetic acid can be produced from methanol.

The Cativa process converts methanol into acetic acid.[33]

Methanol and isobutene are combined to give methyl tert-butyl ether (MTBE). MTBE is a major octane booster in gasoline.

Methanol to hydrocarbons, olefins, gasoline

Condensation of methanol to produce hydrocarbons and even aromatic systems is the basis of several technologies related to gas to liquids. These include methanol-to-hydrocarbons (MtH), methanol to gasoline (MtG), methanol to olefins (MtO), and methanol to propylene (MtP). These conversions are catalyzed by zeolites as heterogeneous catalysts. The MtG process was once commercialized at Motunui in New Zealand.[34][35]

Gasoline additive

The European Fuel Quality Directive allows fuel producers to blend up to 3% methanol, with an equal amount of cosolvent, with gasoline sold in Europe. China uses more than 4.5 billion liters of methanol per year as a transportation fuel in low level blends for conventional vehicles, and high level blends in vehicles designed for methanol fuels.[citation needed]

Other chemicals

Methanol is the precursor to most simple methylamines, methyl halides, and methyl ethers.[18] Methyl esters are produced from methanol, including the transesterification of fats and production of biodiesel via transesterification.[36][37]

Niche and potential uses

Energy carrier

Methanol is a promising energy carrier because, as a liquid, it is easier to store than hydrogen and natural gas. Its energy density is, however, lower than methane, per kg. Its combustion energy density is 15.6 MJ/L (LHV), whereas that of ethanol is 24 and gasoline is 33 MJ/L.

Further advantages for methanol is its ready biodegradability and low environmental toxicity. It does not persist in either aerobic (oxygen-present) or anaerobic (oxygen-absent) environments. The half-life for methanol in groundwater is just one to seven days, while many common gasoline components have half-lives in the hundreds of days (such as benzene at 10–730 days). Since methanol is miscible with water and biodegradable, it is unlikely to accumulate in groundwater, surface water, air or soil.[38]

Fuel

Main pages: Chemistry:Methanol fuel and Chemistry:Methanol economy

Methanol is occasionally used to fuel internal combustion engines. It burns forming carbon dioxide and water:

2 CH
3OH + 3 O
2 → 2 CO
2 + 4 H
2O

Methanol fuel has been proposed for ground transportation. The chief advantage of a methanol economy is that it could be adapted to gasoline internal combustion engines with minimum modification to the engines and to the infrastructure that delivers and stores liquid fuel. Its energy density, however, is less than gasoline, meaning more frequent fill ups would be required. However, it is equivalent to super high-octane gasoline in horsepower, and most modern computer-controlled fuel injection systems can already use it.[39]

Methanol is an alternative fuel for ships that helps the shipping industry meet increasingly strict emissions regulations. It significantly reduces emissions of sulfur oxides (SOx), nitrogen oxides (NOx) and particulate matter. Methanol can be used with high efficiency in marine diesel engines after minor modifications using a small amount of pilot fuel (dual fuel).[40][41]

In China, methanol fuels industrial boilers, which are used extensively to generate heat and steam for various industrial applications and residential heating. Its use is displacing coal, which is under pressure from increasingly stringent environmental regulations.[42]

Direct-methanol fuel cells are unique in their low temperature, atmospheric pressure operation, which lets them be greatly miniaturized.[43][44] This, combined with the relatively easy and safe storage and handling of methanol, may open the possibility of fuel cell-powered consumer electronics, such as laptop computers and mobile phones.[45]

Methanol is also a widely used fuel in camping and boating stoves. Methanol burns well in an unpressurized burner, so alcohol stoves are often very simple, sometimes little more than a cup to hold fuel. This lack of complexity makes them a favorite of hikers who spend extended time in the wilderness. Similarly, the alcohol can be gelled to reduce risk of leaking or spilling, as with the brand "Sterno".

Methanol is mixed with water and injected into high performance diesel and gasoline engines for an increase of power and a decrease in intake air temperature in a process known as water methanol injection.

Other applications

Methanol is used as a denaturant for ethanol, the product being known as "denatured alcohol" or "methylated spirit". This was commonly used during the U.S. prohibition to discourage consumption of bootlegged liquor, and ended up causing several deaths.[46]

Methanol is used as a solvent and as an antifreeze in pipelines and windshield washer fluid. Methanol was used as an automobile coolant antifreeze in the early 1900s.[47] As of May 2018, methanol was banned in the EU for use in windscreen washing or defrosting due to its risk of human consumption[48][49] as a result of 2012 Czech Republic methanol poisonings.[50]

In some wastewater treatment plants, a small amount of methanol is added to wastewater to provide a carbon food source for the denitrifying bacteria, which convert nitrates to nitrogen gas and reduce the nitrification of sensitive aquifers.

Methanol is used as a destaining agent in polyacrylamide gel electrophoresis.

Production

From synthesis gas

Carbon monoxide and hydrogen react over a catalyst to produce methanol. Today, the most widely used catalyst is a mixture of copper and zinc oxides, supported on alumina, as first used by ICI in 1966. At 5–10 MPa (50–100 atm) and 250 °C (482 °F), the reaction

CO + 2 H
2 → CH
3OH

is characterized by high selectivity (>99.8%). The production of synthesis gas from methane produces three moles of hydrogen for every mole of carbon monoxide, whereas the synthesis consumes only two moles of hydrogen gas per mole of carbon monoxide. One way of dealing with the excess hydrogen is to inject carbon dioxide into the methanol synthesis reactor, where it, too, reacts to form methanol according to the equation

CO
2 + 3 H
2 → CH
3OH + H
2O

In terms of mechanism, the process occurs via initial conversion of CO into CO
2, which is then hydrogenated:[51]

CO
2 + 3 H
2 → CH
3OH + H
2O

where the H
2O byproduct is recycled via the water-gas shift reaction

CO + H
2O → CO
2 + H
2

This gives an overall reaction

CO + 2 H
2 → CH
3OH

which is the same as listed above. In a process closely related to methanol production from synthesis gas, a feed of hydrogen and CO
2 can be used directly.[52] The main advantage of this process is that captured CO
2 and hydrogen sourced from electrolysis could be used, removing the dependence on fossil fuels.

Biosynthesis

The catalytic conversion of methane to methanol is effected by enzymes including methane monooxygenases. These enzymes are mixed-function oxygenases, i.e. oxygenation is coupled with production of water[53] and NAD+
:[54]

CH
4 + O
2 + NADPH + H+
 → CH
3OH + H
2O + NAD+

Both Fe- and Cu-dependent enzymes have been characterized.[54] Intense but largely fruitless efforts have been undertaken to emulate this reactivity.[55][56] Methanol is more easily oxidized than is the feedstock methane, so the reactions tend not to be selective. Some strategies exist to circumvent this problem. Examples include Shilov systems and Fe- and Cu-containing zeolites.[57] These systems do not necessarily mimic the mechanisms employed by metalloenzymes, but draw some inspiration from them. Active sites can vary substantially from those known in the enzymes. For example, a dinuclear active site is proposed in the sMMO enzyme, whereas a mononuclear iron (alpha-oxygen) is proposed in the Fe-zeolite.[58]

Global emissions of methanol by plants are estimated at between 180 and 250 million tons per year.[59] This is between two and three times larger than man-made industrial production of methanol.

Green methanol

As of 2023, 0.2% of global methanol production is produced in ways that have relatively low greenhouse gas emissions; this is known as "green" methanol.[60] Most green methanol is produced from gasification of biomass.[60] Syngas is produced from biomass gasification and further converted into green methanol.[61]

Another method of producing green methanol involves combining hydrogen, carbon dioxide, and a catalyst under high heat and pressure.[60] To be classified as green methanol, the hydrogen must be green hydrogen, which is produced using renewable electricity.[60] Additionally, the carbon dioxide in this process must be a product of carbon capture and storage or direct air capture or biomass of recent origin.[60] Some definitions of green methanol specify that the carbon dioxide must be captured during the burning of bioenergy.[62]

Quality specifications and analysis

Methanol is available commercially in various purity grades. Commercial methanol is generally classified according to ASTM purity grades A and AA. Both grade A and grade AA purity are 99.85% methanol by weight. Grade "AA" methanol contains trace amounts of ethanol as well.[30]

Methanol for chemical use normally corresponds to Grade AA. In addition to water, typical impurities include acetone and ethanol (which are very difficult to separate by distillation). UV-vis spectroscopy is a convenient method for detecting aromatic impurities. Water content can be determined by the Karl-Fischer titration.

Safety

Methanol is highly flammable. Its vapours are slightly heavier than air and can travel to a distant ignition source and ignite. Methanol fires should be extinguished with dry chemical, carbon dioxide, water spray or alcohol-resistant foam.[12] Methanol flames are invisible in daylight.

Toxicity

Main page: Medicine:Methanol toxicity

Ingesting as little as 10 mL (0.34 US fl oz) of pure methanol can cause permanent blindness by destruction of the optic nerve. 30 mL (1.0 US fl oz) is potentially fatal.[63] The median lethal dose is 100 mL (3.4 US fl oz), i.e., 1–2 mL/kg body weight of pure methanol.[64] The reference dose for methanol is 0.5 mg/kg in a day.[65][66] Toxic effects begin hours after ingestion, and antidotes can often prevent permanent damage.[63] Because of its similarities in both appearance and odor to ethanol (the alcohol in beverages), it is difficult to differentiate between the two; such is also the case with denatured alcohol, adulterated liquors or very low quality alcoholic beverages.

Methanol is toxic by two mechanisms. First, methanol can be fatal due to effects on the central nervous system, acting as a central nervous system depressant in the same manner as ethanol poisoning. Second, in a process of toxication, it is metabolised to formic acid (which is present as the formate ion) via formaldehyde in a process initiated by the enzyme alcohol dehydrogenase in the liver.[67] Methanol is converted to formaldehyde via alcohol dehydrogenase (ADH) and formaldehyde is converted to formic acid (formate) via aldehyde dehydrogenase (ALDH). The conversion to formate via ALDH proceeds completely, with no detectable formaldehyde remaining.[68] Formate is toxic because it inhibits mitochondrial cytochrome c oxidase, causing hypoxia at the cellular level, and metabolic acidosis, among a variety of other metabolic disturbances.[69]

Outbreaks of methanol poisoning have occurred primarily due to contamination of drinking alcohol. This is more common in the developing world.[70] In 2013 more than 1700 cases nonetheless occurred in the United States. Those affected are often adult men.[71] Outcomes may be good with early treatment.[72] Toxicity to methanol was described as early as 1856.[73]

Because of its toxic properties, methanol is frequently used as a denaturant additive for ethanol manufactured for industrial uses. This addition of methanol exempts industrial ethanol (commonly known as "denatured alcohol" or "methylated spirit") from liquor excise taxation in the U.S. and other countries.

See also

References

  1. ↑ Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 692. doi:10.1039/9781849733069-00648. ISBN 978-0-85404-182-4. 
  2. ↑ Lide, D. R., ed (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5. 
  3. ↑ Ballinger, P.; Long, F. A. (1960). "Acid Ionization Constants of Alcohols. II. Acidities of Some Substituted Methanols and Related Compounds". J. Am. Chem. Soc. 82 (4): 795–798. doi:10.1021/ja01489a008. 
  4. ↑ "Methyloxonium". https://pubchem.ncbi.nlm.nih.gov/compound/12660727. 
  5. ↑ "Methanolate". https://pubchem.ncbi.nlm.nih.gov/compound/3826051#section=Top. "Methoxide is an organic anion that is the conjugate base of methanol. ... It is a conjugate base of a methanol." 
  6. ↑ "RefractiveIndex.INFO – Refractive index database". http://refractiveindex.info/?group=LIQUIDS&material=Methanol. 
  7. ↑ González, Begoña (2007). "Density, dynamic viscosity, and derived properties of binary mixtures of methanol or ethanol with water, ethyl acetate, and methyl acetate at T = (293.15, 298.15, and 303.15) K". The Journal of Chemical Thermodynamics 39 (12): 1578–1588. doi:10.1016/j.jct.2007.05.004. 
  8. ↑ 8.0 8.1 8.2 8.3 "Methanol". Valtech. http://www.labchem.com/tools/msds/msds/VT430.pdf. 
  9. ↑ 9.0 9.1 Toxicity on PubChem
  10. ↑ 10.0 10.1 10.2 10.3 NIOSH Pocket Guide to Chemical Hazards. "#0397". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0397.html. 
  11. ↑ 11.0 11.1 11.2 "Methanol". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/67561.html. 
  12. ↑ 12.0 12.1 12.2 "The Emergency Response Safety and Health Database: Systematic Agent: METHANOL". Centers for Disease Control and Prevention. https://www.cdc.gov/niosh/ershdb/EmergencyResponseCard_29750029.html#er. 
  13. ↑ "PubChem: Safety and Hazards - GHS Classification". National Center for Biotechnology Information, U.S. National Library of Medicine. https://pubchem.ncbi.nlm.nih.gov/compound/887#section=Safety-and-Hazards. 
  14. ↑ "Methanol Safe Handling Manual". 2017. p. 253. http://www.methanol.org/wp-content/uploads/2017/03/Safe-Handling-Manual.pdf. 
  15. ↑ "Technical Information & Safe Handling Guide for Methanol". Methanex Corporation. http://www.methanol.org/Health-And-Safety/Safety-Resources/Health---Safety/Methanex-TISH-Guide.aspx. 
  16. ↑ "Methanol Safe Handling Manual". 2017. p. 243. http://www.methanol.org/wp-content/uploads/2017/03/Safe-Handling-Manual.pdf. 
  17. ↑ National Institute for Occupational Safety and Health (22 August 2008). "The Emergency Response Safety and Health Database: Methanol". https://www.cdc.gov/niosh/ershdb/EmergencyResponseCard_29750029.html. 
  18. ↑ 18.0 18.1 18.2 Fiedler, E.; Grossmann, G.; Burkhard Kersebohm, D.; Weiss, G.; Witte, C. (2005). "Methanol". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_465. ISBN 978-3-527-30673-2. 
  19. ↑ Turner C (2006). "A longitudinal study of methanol in the exhaled breath of 30 healthy volunteers using selected ion flow tube mass spectrometry, SIFT-MS". Physiological Measurement 27 (7): 637–48. doi:10.1088/0967-3334/27/7/007. PMID 16705261. Bibcode: 2006PhyM...27..637T. 
  20. ↑ Lindinger W (1997). "Endogenous production of methanol after the consumption of fruit". Alcoholism: Clinical and Experimental Research 21 (5): 939–43. doi:10.1111/j.1530-0277.1997.tb03862.x. PMID 9267548. 
  21. ↑ "Major Source of Methanol in the Ocean Identified". 10 March 2016. http://www.whoi.edu/news-release/major-source-of-methanol-in-the-ocean-identified. 
  22. ↑ Mincer, Tracy J.; Aicher, Athena C. (2016). "Methanol Production by a Broad Phylogenetic Array of Marine Phytoplankton". PLOS ONE 11 (3): e0150820. doi:10.1371/journal.pone.0150820. PMID 26963515. Bibcode: 2016PLoSO..1150820M. 
  23. ↑ Brooks Hays (17 April 2015). "Why astronomers hate the lawn-mowing Roomba". Space Daily. http://www.spacedaily.com/reports/Why_astronomers_hate_the_lawn-mowing_Roomba_999.html. 
  24. ↑ "Upgraded MERLIN spies cloud of alcohol spanning 288 billion miles" (Press release). Jodrell Bank Centre for Astrophysics. 19 April 2006. Archived from the original on 20 July 2011.
  25. ↑ Amos, Jonathan (5 April 2006). "Merlin sees vast alcohol stream". BBC News. http://news.bbc.co.uk/2/hi/science/nature/4878048.stm. 
  26. ↑ "First Detection of Methyl Alcohol in a Planet-forming Disc". http://www.eso.org/public/news/eso1619/. 
  27. ↑ Boyle discusses the distillation of liquids from the wood of the box shrub in: Robert Boyle, The Sceptical Chymist (London, England: J. Cadwell, 1661), pp. 192–195.
  28. ↑ 28.0 28.1 A report on methanol to the French Academy of Sciences by J. Dumas and E. Péligot began during the Academy's meeting of 27 October 1834 and finished during the meeting of 3 November 1834. See: Procès-verbaux des séances de l'Académie, 10 : 600–601. Available on: Gallica . The complete report appears in: J. Dumas and E. Péligot (1835) "Mémoire sur l'espirit de bois et sur les divers composés ethérés qui en proviennent" (Memoir on spirit of wood and on the various ethereal compounds that derive therefrom), Annales de chimie et de physique, 58 : 5–74; from page 9: Nous donnerons le nom de méthylène (1) à un radical ... (1) Μεθυ, vin, et υλη, bois; c'est-à-dire vin ou liqueur spiritueuse du bois. (We will give the name methylene (1) to a radical ... (1) methy, wine, and hulē, wood; that is, wine or spirit of wood.)
  29. ↑ For a report on the International Conference on Chemical Nomenclature that was held in April 1892 in Geneva, Switzerland, see:
  30. ↑ 30.0 30.1 Bozzano, Giulia; Manenti, Flavio (2016-09-01). "Efficient methanol synthesis: Perspectives, technologies and optimization strategies" (in en). Progress in Energy and Combustion Science 56: 71–105. doi:10.1016/j.pecs.2016.06.001. ISSN 0360-1285. https://www.sciencedirect.com/science/article/abs/pii/S0360128515300484. Retrieved 25 September 2021. 
  31. ↑ Halderman, James D.; Martin, Tony (2009). Hybrid and alternative fuel vehicles. Pearson/Prentice Hall. ISBN 978-0-13-504414-8. https://books.google.com/books?id=LqgeAQAAIAAJ. 
  32. ↑ Ronald Smith (1 December 2011). "Methanol to Gasoline: A Private Report by the Process Economics Program". https://ihsmarkit.com/pdf/RP282_toc_173824110917062932.pdf. 
  33. ↑ Sunley, G. J.; Watson, D. J. (2000). "High productivity methanol carbonylation catalysis using iridium – The Cativa process for the manufacture of acetic acid". Catalysis Today 58 (4): 293–307. doi:10.1016/S0920-5861(00)00263-7. 
  34. ↑ Olsbye, U.; Svelle, S.; Bjorgen, M.; Beato, P.; Janssens, T. V. W.; Joensen, F.; Bordiga, S.; Lillerud, K. P. (2012). "Conversion of Methanol to Hydrocarbons: How Zeolite Cavity and Pore Size Controls Product Selectivity". Angew. Chem. Int. Ed. 51 (24): 5810–5831. doi:10.1002/anie.201103657. PMID 22511469. 
  35. ↑ Tian, P.; Wei, Y.; Ye, M.; Liu, Z. (2015). "Methanol to Olefins (MTO): From Fundamentals to Commercialization". ACS Catal. 5 (3): 1922–1938. doi:10.1021/acscatal.5b00007. 
  36. ↑ "Biodiesel – METHANOL INSTITUTE". METHANOL INSTITUTE. http://www.methanol.org/biodiesel/. 
  37. ↑ "Biodiesel Production Principles and Processes – eXtension". http://articles.extension.org/pages/27137/biodiesel-production-principles-and-processes. 
  38. ↑ Evaluation of the Fate and Transport of Methanol in the Environment , Malcolm Pirnie, Inc., January 1999.
  39. ↑ "Methanol Wins". December 2011. https://www.nationalreview.com/2011/12/methanol-wins-robert-zubrin/. 
  40. ↑ "Methanol as a Marine Fuel". Methanex Corporation. https://www.methanex.com/about-methanol/methanol-marine-fuel. 
  41. ↑ Andersson, Karin; Márquez Salazar, Carlos (2015). Methanol as a Marine Fuel Report (Report). FC Business Intelligence. http://www.methanol.org/wp-content/uploads/2018/03/FCBI-Methanol-Marine-Fuel-Report-Final-English.pdf. Retrieved 2021-04-10. 
  42. ↑ "Methanol as an Industrial Boiler Fuel". Methanex Corporation. https://www.methanex.com/about-methanol/methanol-industrial-boiler-fuel. 
  43. ↑ Kamitani, A.; Morishita, S.; Kotaki, H.; Arscott, S. (2008). "Miniaturized microDMFC using silicon microsystems techniques: Performances at low fuel flow rates". Journal of Micromechanics and Microengineering 18 (12): 125019. doi:10.1088/0960-1317/18/12/125019. Bibcode: 2008JMiMi..18l5019K. https://hal.archives-ouvertes.fr/hal-02347363/file/kamitani_et_al_2008.pdf. Retrieved 30 October 2021. 
  44. ↑ Kamitani, A.; Morishita, S.; Kotaki, H.; Arscott, S. (2011). "Microfabricated microfluidic fuel cells". Sensors and Actuators B: Chemical 154 (2): 174. doi:10.1016/j.snb.2009.11.014. 
  45. ↑ Berger, Sandy (30 September 2006). "Methanol Laptop Fuel". Compu·Kiss. http://www.compukiss.com/populartopics/tech_gadgetshtm/article887.htm. 
  46. ↑ Blum, Deborah (19 February 2010). "The little-told story of how the U.S. government poisoned alcohol during Prohibition". http://www.slate.com/id/2245188/. 
  47. ↑ Yant, W. P.; Schrenk, H. H.; Sayers, R. R. (1931). "Methanol Antifreeze and Methanol Poisoning". Industrial & Engineering Chemistry 23 (5): 551. doi:10.1021/ie50257a020. 
  48. ↑ "EUR-Lex – 32018R0589 – EN – EUR-Lex". https://eur-lex.europa.eu/legal-content/EN/ALL/?uri=CELEX:32018R0589. 
  49. ↑ "Corrigendum to Commission Regulation (EU) 2018/589 of 18 April 2018 amending Annex XVII to Regulation (EC) No 1907/2006 of the European Parliament and of the Council concerning the Registration, Evaluation, Authorisation and Restriction of Chemicals (REACH) as regards methanol (OJ L 99, 19.4.2018)" (in en). 2018-04-23. http://data.europa.eu/eli/reg/2018/589/corrigendum/2018-04-23/oj/eng. 
  50. ↑ "Annex XV Restriction Report: Proposal For a Restriction Substance Name: Methanol – table D.1-4-page 79". 2015-01-16. https://echa.europa.eu/documents/10162/78b0f856-3751-434b-b6bc-6d33cd630c85. 
  51. ↑ Deutschmann, Olaf; Knözinger, Helmut; Kochloefl, Karl and Turek, Thomas (2012) "Heterogeneous Catalysis and Solid Catalysts, 3. Industrial Applications" in Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH, Weinheim. doi:10.1002/14356007.o05_o03
  52. ↑ Bozzano, Giulia; Manenti, Flavio (2016). "Efficient methanol synthesis: Perspectives, technologies and optimization strategies" (in en). Progress in Energy and Combustion Science 56: 76. doi:10.1016/j.pecs.2016.06.001. ISSN 0360-1285. https://www.sciencedirect.com/science/article/pii/S0360128515300484. 
  53. ↑ Mu-Hyun Baik; Martin Newcomb; Richard A. Friesner; Stephen J. Lippard (2003). "Mechanistic Studies on the Hydroxylation of Methane by Methane Monooxygenase". Chem. Rev. 103 (6): 2385–2420. doi:10.1021/cr950244f. PMID 12797835. 
  54. ↑ 54.0 54.1 Lawton, T. J.; Rosenzweig, A. C. (2016). "Biocatalysts for methane conversion: big progress on breaking a small substrate". Curr. Opin. Chem. Biol. 35: 142–149. doi:10.1016/j.cbpa.2016.10.001. PMID 27768948. 
  55. ↑ Alayon, E. M. C.; Nachtegaal, M.; Ranocchiari, M.; Van Bokhoven, J. A. (2012). "Catalytic Conversion of Methane to Methanol Using Cu-Zeolites". CHIMIA International Journal for Chemistry 66 (9): 668–674. doi:10.2533/chimia.2012.668. PMID 23211724. https://www.dora.lib4ri.ch/psi/islandora/object/psi%3A20913. Retrieved 10 May 2021. 
  56. ↑ Hammond, C.; Jenkins, R. L.; Dimitratos, N.; Lopez-Sanchez, J. A.; Ab Rahim, M. H.; Forde, M.M.; Thetford, A.; Murphy, D.M. et al. (2012). "Catalytic and Mechanistic Insights of the Low-Temperature Selective Oxidation of Methane over Cu-Promoted Fe-ZSM-5". Chemistry: A European Journal 18 (49): 15735–45. doi:10.1002/chem.201202802. PMID 23150452. 
  57. ↑ Snyder, Benjamin E. R.; Bols, Max L.; Schoonheydt, Robert A.; Sels, Bert F.; Solomon, Edward I. (2017-12-19). "Iron and Copper Active Sites in Zeolites and Their Correlation to Metalloenzymes". Chemical Reviews 118 (5): 2718–2768. doi:10.1021/acs.chemrev.7b00344. PMID 29256242. https://limo.libis.be/primo-explore/fulldisplay?docid=LIRIAS1644877&context=L&vid=Lirias&search_scope=Lirias&tab=default_tab&lang=en_US&fromSitemap=1. Retrieved 25 September 2021. 
  58. ↑ Snyder, Benjamin E. R.; Vanelderen, Pieter; Bols, Max L.; Hallaert, Simon D.; Böttger, Lars H.; Ungur, Liviu; Pierloot, Kristine; Schoonheydt, Robert A. et al. (2016). "The active site of low-temperature methane hydroxylation in iron-containing zeolites". Nature 536 (7616): 317–321. doi:10.1038/nature19059. PMID 27535535. Bibcode: 2016Natur.536..317S. 
  59. ↑ Stavrakou, T.; Guenther, A.; Razavi, A.; Clarisse, L.; Clerbaux, C.; Coheur, P.-F.; Hurtmans, D.; Karagulian, F. et al. (2011-05-25). "First space-based derivation of the global atmospheric methanol emission fluxes" (in en). Atmospheric Chemistry and Physics 11 (10): 4873–4898. doi:10.5194/acp-11-4873-2011. ISSN 1680-7324. Bibcode: 2011ACP....11.4873S. https://acp.copernicus.org/articles/11/4873/2011/. Retrieved 26 September 2022. 
  60. ↑ 60.0 60.1 60.2 60.3 60.4 Sollai, Stefano; Porcu, Andrea; Tola, Vittorio; Ferrara, Francesca; Pettinau, Alberto (2023-02-01). "Renewable methanol production from green hydrogen and captured CO2: A techno-economic assessment". Journal of CO2 Utilization 68: 102345. doi:10.1016/j.jcou.2022.102345. ISSN 2212-9820. 
  61. ↑ Sasidhar, Nallapaneni (November 2023). "Carbon Neutral Fuels and Chemicals from Standalone Biomass Refineries". Indian Journal of Environment Engineering 3 (2): 1–8. doi:10.54105/ijee.B1845.113223. ISSN 2582-9289. https://www.ijee.latticescipub.com/wp-content/uploads/papers/v3i2/B1845113223.pdf. Retrieved 3 December 2023. 
  62. ↑ "Green Hydrogen for Industry: A Guide to Policy Making" (in en). 2022-03-08. p. 18. https://www.irena.org/publications/2022/Mar/Green-Hydrogen-for-Industry. 
  63. ↑ 63.0 63.1 Vale A (2007). "Methanol". Medicine 35 (12): 633–4. doi:10.1016/j.mpmed.2007.09.014. 
  64. ↑ "Methanol Poisoning Overview". Antizol. http://www.antizol.com/mpoisono.htm. 
  65. ↑ "Integrated Risk Information System". US EPA, ORD, NCEA, IRISD. 15 March 2013. http://www.epa.gov/iris/subst/0305.htm. 
  66. ↑ "Toxicological Review of Methanol (Noncancer) (CAS No. 67-56-1) In Support of Summary Information on the Integrated Risk Information System (IRIS)". EPA. September 2013. https://cfpub.epa.gov/ncea/iris/iris_documents/documents/toxreviews/0305tr.pdf. 
  67. ↑ "A seaman with blindness and confusion". BMJ 339: b3929. 2009. doi:10.1136/bmj.b3929. PMID 19793790. http://www.bmj.com/cgi/content/full/339/sep30_1/b3929. Retrieved 3 October 2009. 
  68. ↑ "Lack of a role for formaldehyde in methanol poisoning in the monkey". Biochem. Pharmacol. 28 (5): 645–9. 1979. doi:10.1016/0006-2952(79)90149-7. PMID 109089. 
  69. ↑ "Methanol and formic acid toxicity: biochemical mechanisms". Pharmacol. Toxicol. 69 (3): 157–63. September 1991. doi:10.1111/j.1600-0773.1991.tb01290.x. PMID 1665561. 
  70. ↑ Beauchamp, GA; Valento, M (September 2016). "Toxic Alcohol Ingestion: Prompt Recognition And Management in the Emergency Department". Emergency Medicine Practice 18 (9): 1–20. PMID 27538060. 
  71. ↑ Ferri, Fred F. (2016). Ferri's Clinical Advisor 2017: 5 Books in 1. Elsevier Health Sciences. p. 794. ISBN 978-0-323-44838-3. https://books.google.com/books?id=rRhCDAAAQBAJ&pg=PA794. Retrieved 22 August 2019. 
  72. ↑ Kruse, JA (October 2012). "Methanol and ethylene glycol intoxication". Critical Care Clinics 28 (4): 661–711. doi:10.1016/j.ccc.2012.07.002. PMID 22998995. 
  73. ↑ Clary, John J. (2013). The Toxicology of Methanol. John Wiley & Sons. p. 3.4.1. ISBN 978-1-118-35310-3. https://books.google.com/books?id=xSs8oDQV4uYC&&pg=PA44. 

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