View source for Methanol

{{chembox
|   Name = Methanol
|   ImageFileL1 = Methanol-2D.png 
|   ImageSizeL1 = 120px 
|   ImageNameL1 = Methanol 
|   ImageFileR1 = Methanol-3D-balls.png
|   ImageSizeR1 = 120px 
|   ImageNameR1 = Methanol
|   ImageFileR2 = Methanol-3D-vdW.png
|   ImageSizeR2 = 120px 
|   ImageNameR2 = Methanol
|   ImageFileL2 = Methanol_flat_structure.png
|   ImageSizeL2 = 120px
|   ImageNameL2 = Methanol
|   IUPACName = methanol
|   OtherNames = hydroxymethane<br/>methyl alcohol<br/>methyl hydrate</br>wood alcohol<br/>carbinol
| Section1 = {{Chembox Identifiers
|   InChI = 1/CH4O/c1-2/h2H,1H3
|   StdInChI = 1S/CH4O/c1-2/h2H,1H3
|   InChIKey = OKKJLVBELUTLKV-UHFFFAOYAX
|   StdInChIKey = OKKJLVBELUTLKV-UHFFFAOYSA-N
|   EC-number = 200-659-6
|   SMILES = CO 
|   CASNo = 67-56-1
|    CASNo_Ref = {{cascite}}
|   ChemSpiderID = 864
|   RTECS = PC1400000 
  }}
| Section2 = {{Chembox Properties
|   Reference = <ref name="NIST">{{NIST chemistry|id=1S/CH4O/c1-2/h2H,1H3|name=Methyl alcohol|accessdate=2009-08-21}}.</ref><ref name="ICSC">{{ICSC-ref|0057|name=Methanol|date=April 2000}}.</ref><ref>{{RubberBible62nd|page=C-374}}.</ref>
|   Formula = CH<sub>3</sub>OH 
|   MolarMass = 32.042 kJ mol<sup>−1</sup> 
|   Appearance = colorless liquid
|   Density = 0.7914 g cm<sup>−3</sup>
|   Solubility = miscible
|   MeltingPt = –97 °C (176 K) 
|   BoilingPt = 64.7 °C (337.8 K) 
|   TriplePt = –97.7 ºC (175.5 K)
|   CriticalPt = 513 K, 81 bar
|   pKa = approx. 15.5  <!-- unreferenced -->
|   Viscosity = 0.59 mPa s at 20 °C  <!-- unreferenced -->
|   Dipole = 1.69 D (gas) <!-- unreferenced -->
|   LogP = –0.82
|   VaporPressure = 12.3 kPa at 20 ºC
|   RefractIndex = 1.3288 at 20 ºC
  }}
| Section3 = {{Chembox Thermochemistry
|   Reference = <ref name="NIST"/><ref>{{citation | last1 = Maass | first1 = O. | last2 = Walbauer | first2 = L. J. | title = The specific heats and latent heats of fusion of ice and of several organic compounds | journal = J. Am. Chem. Soc. | year = 1925 | volume = 47 | issue = 1 | pages = 1–9 | doi = 10.1021/ja01678a001}}. {{citation | last1 = Chao | first1 = Jing | last2 = Rossini | first2 = F. D. | title = Heats of combustion, formation, and isomerization of nineteen alkanols | journal = J. Chem. Eng. Data | year = 1965 | volume = 10 | issue = 4 | pages = 374–79 | doi = 10.1021/je60027a022}}. {{citation | last1 = Carlson | first1 = H. G. | last2 = Westrum | first2 = Edgar F., Jr. | title = Methanol: heat capacity, enthalpies of transition and melting, and thermodynamic properties from 5–300ºK | journal = J. Chem. Phys. | year = 1971 | volume = 54 | issue = 4 | pages = 1464–71 | doi = 10.1063/1.1675039}}.</ref>
|   DeltaHf = –239.5 kJ mol<sup>−1</sup>
|   DeltaHc = –725.7 kJ mol<sup>−1</sup>
|   Entropy = 127.2 J K<sup>–1</sup> mol<sup>–1</sup>
|   HeatCapacity = 
|   HeatFus = 2.196 kJ mol<sup>−1</sup>
|   HeatVapor = 37 kJ mol<sup>−1</sup>
  }}
| Section7 = {{Chembox Hazards
|   Reference = <ref name="ICSC"/><ref>{{CLP Regulation|index=603-001-00-X|page=476}}</ref><ref>{{PGCH-ref|id=0397|name=Methyl alcohol}}.</ref>
|   EUIndex = 603-001-00-X
|   MSDS = {{ICSC-small|0057}}
|   GHSPictograms =  {{GHS02|Flam. Liq. 2}}{{GHS06|Acute Tox. 3}}{{GHS08|STOT SE 1}}
|   GHSSignalWord = DANGER
|   HPhrases = {{H-phrases|225|331|311|301|370}}
|   FlashPt = 12 °C (54 ºF)
|   Autoignition = 464 ºC (867 ºF)
|   ExploLimits = 5.5–44%
|   PEL = 200 ppm TWA
|   IDLH = 6000 ppm
  }}
| Section8 = {{Chembox Related
|   OtherFunctn = [[Ethanol]]<br/>[[Propanol]]<br/>[[Butanol]]
|    Function = [[alcohol]]s  
|   OtherCpds = [[Chloromethane]]<br/>[[Methoxymethane]]
  }}
}}

'''Methanol''', also known as '''methyl alcohol''', '''carbinol''', '''wood alcohol''', '''wood naphtha''' or '''wood spirits''', is a toxic [[chemical compound|chemical]] with [[chemical formula|formula]] [[carbon|C]][[hydrogen|H]]<sub>3</sub>[[oxygen|O]][[hydrogen|H]] (often abbreviated MeOH).  Drinking 10&nbsp;ml will cause blindness, and as little as 100&nbsp;ml will cause death, as many unfortunate individuals found out during the [[Prohibition in the United States|Prohibition]]. It is the simplest [[alcohol]], and is a light, [[Volatility (chemistry)|volatile]], [[colour]]less, [[flammable]], toxic liquid with a distinctive odor that is very similar to but slightly sweeter than [[ethanol]] (drinking alcohol).<ref name=ershdb>{{Citation | publisher = National Institute for Occupational Safety and Health | series = Emergency Response Safety and Health Database | title = Methanol | date = August 2008 | url = http://www.cdc.gov/niosh/ershdb/EmergencyResponseCard_29750029.html | accessdate = 2009-03-17}}.</ref> At room temperature it is a [[Solvent#Polarity.2C_solubility.2C_and_miscibility|polar liquid]] and is used as an [[antifreeze (coolant)|antifreeze]], [[solvent]], [[fuel]], and as a [[denatured alcohol|denaturant]] for ethanol. It is also used for producing [[biodiesel]] via [[transesterification]] reaction.

Methanol is produced naturally in the [[anaerobic organism|anaerobic]] [[metabolism]] of many varieties of bacteria, and is ubiquitous in the environment.  As a result, there is a small fraction of methanol vapor in the atmosphere. Over the course of several days, atmospheric methanol is [[oxidized]] by oxygen with the help of sunlight to carbon dioxide and water.

Methanol burns in air forming [[carbon dioxide]] and [[water]]:
:2CH<sub>3</sub>OH + 3O<sub>2</sub> → 2CO<sub>2</sub> + 4H<sub>2</sub>O
A methanol flame is almost colorless in bright sunlight conditions, causing an additional safety hazard around open methanol flames.<ref name="ICSC"/>

Because of its toxic properties, methanol is frequently used as a denaturant additive for ethanol manufactured for industrial uses &mdash; this addition of methanol economically exempts industrial ethanol from the rather significant 'liquor' taxes that would otherwise be levied as it is the essence of all potable alcoholic beverages. Methanol is often called wood alcohol because it was once produced chiefly as a byproduct of the destructive distillation of wood. It is now produced synthetically by a multi-step process: [[natural gas]] or [[coal gas]] and steam are reformed in a furnace to produce hydrogen and carbon monoxide; then, hydrogen and carbon monoxide gases react under pressure in the presence of a catalyst.  Methanol is also produced from the gasification of a range of renewable biomass materials, such as wood and black liquor from pulp and paper mills.

==History==<!-- This section is linked from [[Methyl group]] -->
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 [[boxwood]].  It later became known as ''pyroxylic spirit''.  In 1834, the [[France|French]] chemists [[Jean-Baptiste Dumas]] and [[Eugene Peligot]] determined its elemental composition.

They also introduced the word ''methylene'' to organic chemistry, forming it from [[Greek language|Greek]] ''methy'' = "[[wine]]" + ''hȳlē'' = [[wood]] (patch of trees). Its intended origin was "[[alcohol]] made from [[wood]] (substance)", but it has Greek language errors. 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. The [[suffix (linguistics)|suffix]] [[-yl]] used in [[organic chemistry]] to form names of [[carbon]] groups, was extracted from the word "methyl."

In 1923, the [[Germany|German]] chemists Alwin Mittasch and Mathias Pier, working for [[BASF]] developed a means to convert [[syngas|''synthesis gas'']] (a mixture of [[carbon monoxide]], [[carbon dioxide]], and [[hydrogen]]) into methanol. This process used a [[chromium oxide|chromium]] and [[manganese oxide]] [[catalyst]], and required extremely vigorous conditions—pressures ranging from 50–220&nbsp;atm, and temperatures up to 450&nbsp;°C.<ref>{{citation | inventor1-first = Alwin | inventor1-last= Mittasch | inventor2-first = Mathias | inventor2-last = Pier | assignee = Badische-Anilin- & Soda-Fabrik | assigneelink = BASF | title = Synthetic manufacture of methanol | country-code = US | patent-number = 1569775 | description = Patent | year = 1926}}.</ref> 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) was developed by ICI in the late 1960s with the technology now owned{{Fact|date=March 2009}} by Johnson Matthey who is a leading licensor of methanol technology.

The use of methanol as a motor fuel received attention during the oil crises of the 1970s due to its availability, low cost, and environmental benefits.  By the mid-1990s, over 20,000 methanol "flexible fuel vehices" capable of operating on methanol or gasoline were introduced in the U.S.  In addition, low levels of methanol were blending 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 the interest in methanol fuels.

In 2006 astronomers using the [[MERLIN]] array of radio telescopes at [[Jodrell Bank|Jodrell Bank Observatory]] discovered a large cloud of methanol in space, 300 billion miles across.

==Production==
Today, synthesis gas is most commonly produced from the [[methane]] component in [[natural gas]] rather than from coal.  Three processes are commercially practiced.  At moderate pressures of 4&nbsp;MPa (40&nbsp;atm) and high temperatures (around 850&nbsp;°C), methane [[chemical reaction|reacts]] with [[steam]] on a nickel catalyst to produce [[syngas]] according to the [[chemical equation]]:
:CH<sub>4</sub> + H<sub>2</sub>O → CO + 3H<sub>2</sub>

This reaction, commonly called steam-methane reforming or SMR, is [[endothermic]] and the heat transfer limitations place limits on the size of and pressure in the catalytic reactors used.  Methane can also undergo partial oxidation with molecular oxygen to produce syngas, as the following equation shows:
:2CH<sub>4</sub> + O<sub>2</sub> → 2CO + 4 H<sub>2</sub>

This reaction is [[exothermic]] and the heat given off can be used ''in-situ'' to drive the steam-methane reforming reaction.  When the two processes are combined, it is referred to as autothermal reforming. The ratio of CO and H<sub>2</sub> can be adjusted to some extent by the [[water gas shift reaction|water-gas shift reaction]],
:CO + H<sub>2</sub>O → CO<sub>2</sub> + H<sub>2</sub>,

to provide the appropriate stoichiometry for methanol synthesis.

The carbon monoxide and hydrogen then react on a second catalyst to produce methanol.  Today, the most widely used catalyst is a mixture of [[copper]], [[zinc oxide]], and [[alumina]] first used by [[Imperial Chemical Industries|ICI]] in 1966.  At 5–10&nbsp;MPa (50–100&nbsp;atm) and 250&nbsp;°C, it can catalyze the production of methanol from carbon monoxide and hydrogen with high selectivity:
:CO + 2H<sub>2</sub> → CH<sub>3</sub>OH

It is worth noting that the production of synthesis gas from methane produces 3&nbsp;moles of hydrogen for every mole of carbon monoxide, while the methanol synthesis consumes only 2&nbsp;moles of hydrogen for every 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<sub>2</sub> + 3 H<sub>2</sub> → CH<sub>3</sub>OH + H<sub>2</sub>O

Although natural gas is the most economical and widely used feedstock for methanol production, other feedstocks can be used.  Coal is increasingly being used as a feedstock for methanol production, particularly in China.  In addition, mature technologies available for biomass gasification are being utilized for methanol production.

==Applications==
Methanol is a common laboratory solvent. It is especially useful for [[HPLC]] and [[UV/VIS spectroscopy]] due to its low UV cutoff.

===Feedstock===
The largest use of methanol by far is in making other chemicals. About 40% of methanol is converted to [[formaldehyde]], and from there into products as diverse as [[plastic]]s, [[plywood]], [[paint]]s, [[explosive]]s, and [[permanent press]] [[textile]]s.

Also in the early 1970s, a [[Methanol to gasoline]] process was developed by [[Mobil]] for producing gasoline ready for use in vehicles. One such industrial facility was built at [[Motunui]] in [[New Zealand]] in the 1980s. In the 1990s, large amounts of methanol were used in the [[United States]] to produce the gasoline additive [[methyl tert-butyl ether]] (MTBE). While MTBE is no longer marketed in the U.S., it is still widely used in other parts of the world. In addition to direct use as a fuel, methanol (or less commonly, [[ethanol]]) is used as a component in the [[transesterification]] of [[triglycerides]] to yield a form of [[biodiesel]].

Other chemical derivatives of methanol include [[dimethyl ether]], which has replaced [[chlorofluorocarbon]]s as an [[aerosol spray#Propellant|aerosol spray propellant]], and [[acetic acid]].  Dimethyl ether, or "DME" also can be blended with liquified petroleum gas (LPG) for home heating and cooking, and can be used as a diesel replacement transportation fuel.

===Fuel for vehicles===
{{main|Methanol fuel}}
Methanol is used on a limited basis to fuel [[internal combustion engine]]s, mainly by virtue of the fact that it is not nearly as [[flammable]] as [[gasoline]].  Methanol is harder to ignite than gasoline and produces just one-eighth of the heat upon burning. Pure methanol is required by rule to be used in [[Champcars]], [[Monster Trucks]], [[United States Automobile Club|USAC]] sprint cars (as well as midgets, modifieds, etc.), and other dirt track series such as [[World of Outlaws]], and [[Motorcycle Speedway]].  Methanol is also used in [[radio controlled model|radio control]], [[control line]] and [[free flight (model aircraft)|free flight]] [[Model aircraft|airplanes]] (as methanol is required in the "[[Glow plug (model engine)|glow-plug]]" engines that primarily power them), cars and trucks, from such an engine's use of a [[platinum]] filament glow plug being able to ignite the methanol vapor through a catalytic reaction. [[Drag racing|Drag racers]] and mud racers also use methanol as their primary fuel source. Methanol is required with a supercharged engine in a [[Top Alcohol Dragster]] and, until the end of the 2006 season, all vehicles in the [[Indianapolis 500]] had to run methanol. [[Mud racer]]s have mixed methanol with gasoline and [[nitrous oxide]] to produce more power than gasoline and nitrous oxide alone.

One of the drawbacks of methanol as a fuel is its [[corrosion|corrosivity]] to some metals, including [[aluminium]]. Methanol, although a weak acid, attacks the oxide coating that normally protects the aluminium from corrosion:

:6 CH<sub>3</sub>OH + Al<sub>2</sub>O<sub>3</sub> → 2 Al(OCH<sub>3</sub>)<sub>3</sub> + 3 H<sub>2</sub>O

The resulting [[methoxide]] salts are soluble in methanol, resulting in clean aluminium surface, which is readily oxidized by some dissolved [[oxygen]]. Also the methanol can act as an oxidizer:

:6 CH<sub>3</sub>OH + 2 Al → 2 Al(OCH<sub>3</sub>)<sub>3</sub> + 3 H<sub>2</sub>

This reciprocal process effectively fuels corrosion until either the metal is eaten away or the concentration of CH<sub>3</sub>OH is negligible.  Concerns with methanol's corrosivity have been addressed by using methanol compatible materials, and fuel additives that serve as corrosion inhibitors.

When produced from wood or other organic materials, the resulting organic methanol ([[bioalcohol]]) has been suggested as renewable alternative to petroleum-based [[hydrocarbon]]s. Low levels of methanol can be used in existing vehicles, with the use of proper cosolvents and corrosion inhibitors.  The European Fuel Quality Directive allows up to 3% methanol with an equal amount of cosolvent to be blending in gasoline sold in Europe.  Today, China uses more than one billion gallons of methanol per year as a transportation fuel in both low level blends used in existing vehicles, and as high level blends in vehicles designed to accommodate the use of methanol fuels.

===Other applications===
Methanol is a traditional denaturant for ethanol, thus giving the term ''[[methylated spirit]]''.

Methanol is also used as a [[solvent]], and as an [[antifreeze (coolant)|antifreeze]] in [[Pipeline transport|pipelines]] and [[windshield washer fluid]].

In some [[wastewater treatment plant]]s, a small amount of methanol is added to [[wastewater]] to provide a food source of carbon for the [[denitrifying bacteria]], which convert [[nitrate]]s to [[nitrogen]] to reduce the denitrification of sensitive aquifers.

During [[World War II]], methanol was used as a fuel in several German military rocket designs, under name '''M-Stoff''', and in a mixture as [[C-Stoff]].

Methanol is used as a denaturing agent in [[polyacrylamide gel electrophoresis]].

[[Direct-methanol fuel cell]]s are unique in their low temperature, atmospheric pressure operation, allowing them to be miniaturized to an unprecedented degree. 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 for laptop computers and mobile phones.

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.

==Health and safety==
===Toxicity===
Methanol is toxic. If ingested, as little as 10&nbsp;ml can cause permanent [[blindness]] by destruction of the [[optic nerve]].<ref>{{citation | url = http://www.newton.dep.anl.gov/askasci/chem03/chem03561.htm | title = Methanol and Blindness | series = Ask A Scientist: Chemistry Archive | publisher = U.S. Department of Energy | date = May 2005 | accessdate = 2007-05-22}}.</ref>  The usual fatal dose is 100–125&nbsp;ml (about 4&nbsp;fl.&nbsp;oz.).  Toxic effects take hours to start and effective antidotes can often prevent permanent damage.  

Because of its similarities to [[ethanol]] (the alcohol in beverages), it is difficult to differentiate between the two (such is the case with [[denatured alcohol]]).

Methanol is [[toxic]] by two mechanisms. Firstly, methanol (whether it enters the body by [[ingestion]], [[inhalation]], or [[absorption (chemistry)|absorption]] through the [[skin]]) can be fatal due to its [[CNS depressant]] properties in the same manner as [[ethanol]] poisoning. Secondly, in a process of [[toxication]], it is [[metabolism|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]].  The reaction to formate proceeds completely, with no detectable formaldehyde remaining.<ref name=noCHOH>{{citation | last1 = McMartin | first1 = Kenneth E. | last2 = Martin-Amat | first2 = Gladys | last3 = Noker | first3 = Patricia E. | last4 = Tephly | first4 = Thomas R. | title = Lack of a role for formaldehyde in methanol poisoning in the monkey | journal = Biochem. Pharmacol. | volume = 28 | issue = 5 | pages = 645–49 | year = 1979 | pmid = 109089 | doi = 10.1016/0006-2952(79)90149-7}}.</ref>  Formate is toxic because it inhibits mitochondrial [[cytochrome c oxidase]], causing the symptoms of [[hypoxia]] at the cellular level, and also causing [[metabolic acidosis]] among a variety of other metabolic disturbances.<ref>{{citation | last1 = Liesivuori | first1 = Jyrki | last2 = Savolainen | first2 = Heikki | title = Methanol and formic acid toxicity: biochemical mechanisms | journal = Pharmacol. Toxicol. | volume = 69 | issue = 3 | pages = 157–63 | year = 1991 | pmid = 1665561 | doi = 10.1111/j.1600-0773.1991.tb01290.x}}.</ref> Fetal tissue will not tolerate methanol. This is treated using [[ethanol]] or [[fomepizole]].<ref>{{citation | first = Marcel J. | last = Casavant | url = http://pediatrics.aappublications.org/cgi/content/full/107/1/170 | title = Fomepizole in the Treatment of Poisoning | journal = Pediatrics | online = yes | year = 2001 | issue = 1 | volume = 107 | accessdate = 2007-05-22}}.</ref> Both of these drugs acts to slow down the action of [[alcohol dehydrogenase]] on methanol by means of [[competitive inhibition]], so that it is excreted by the [[kidney]]s rather than being transformed into toxic metabolites.

The initial symptoms of methanol intoxication are those of [[central nervous system]] [[depressant|depression]]: headache, dizziness, nausea, lack of coordination, confusion, drowsiness, and with sufficiently large doses, unconsciousness and death.  The initial symptoms of methanol exposure are usually less severe than the symptoms resulting from the ingestion of a similar quantity of ethanol.<ref name=ershdb />

Once the initial symptoms have passed, a second set of symptoms arises, 10 to as much as 30 hours after the initial exposure to methanol, including blurring or complete loss of vision and [[acidosis]].  These symptoms result from the accumulation of toxic levels of [[formate]] in the bloodstream, and may progress to death by [[respiratory failure]]. The [[ester]] derivatives of methanol do not share this toxicity.

Ethanol is sometimes denatured (adulterated), and thus made undrinkable, by the addition of methanol. The result is known as methylated spirit or "meths" (UK use). (The latter should not be confused with ''meth'', a common U.S. abbreviation for [[methamphetamine]].)

===Safety in automotive fuels===
Pure methanol has been used in [[open wheel car|open wheel auto racing]] since the mid-1960s. Unlike petroleum fires, methanol fires can be [[active fire protection|extinguished]] with plain water. A methanol-based fire burns invisibly, unlike gasoline, which burns with a visible flame. If a fire occurs on the track, there is no flame or smoke to obstruct the view of fast approaching drivers, but this can also delay visual detection of the fire and the initiation of fire suppression actions. The decision to permanently switch to methanol in American [[American Championship Car Racing|IndyCar]] racing was a result of the devastating crash and explosion at the [[1964 Indianapolis 500]] which killed drivers [[Eddie Sachs]] and [[Dave MacDonald]].<ref>{{Citation | last =  McDonald | first = Norris | title = Green no longer bad luck at Indy | newspaper = Toronto Star | url = http://www.thestar.com/comment/columnists/article/205088 | date = April 21, 2007}}.</ref> In 2007 IndyCars switched from methanol to ethanol.<ref>{{citation | url = http://www.indycar.com/tech/ethanol.php}}.</ref>

Methanol is readily biodegradable in both aerobic (oxygen present) and anaerobic (oxygen absent) environments. Methanol will not persist in the environment.  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&nbsp;days).  Since methanol is infinitely soluble in water and biodegradable, methanol is unlikely to accumulate in groundwater, surface water, air or soil.<ref>{{citation | title = Evaluation of the Fate and Transport of Methanol in the Environment | url = http://www.methanol.org/pdf/evaluation.pdf | first = Malcolm | last = Pirnie | publisher = American Methanol Institute | location = Washington, DC | date = January 1999}}.</ref>

==See also==
* [[Liquid fuel]]s
* [[Methanol fuel]]
* [[List of Stoffs]]
* [[Methanol (data page)]]
* [[Methanol economy]]
* [[Deuterated methanol]]
* [[Pärnu methanol tragedy]]

==References==
{{reflist}}

==Further reading==
*[[Robert Boyle]], ''[[The Sceptical Chymist]]'' (1661) &ndash; contains account of distillation of wood alcohol.
* {{citation | last1 = Gallucci | first1 =  F. | last2 = Basile | first2 = A. | last3 = Drioli | first3 = E. | title = Methanol as an energy source and/or energy carrier in membrane processes | journal = Separ. Purif. Rev. | volume = 36 | issue = 2 | pages = 175–202}}.

==External links==
*{{ICSC|0057}}
*{{PGCH|0397}}
*{{NPI|id=54|name=Methanol}}
*[http://www.racecarbook.com Race Car Book] RaceCarBook.com, includes technical articles and methanol racing book information.
*[http://www.methanol.org The Methanol Institute] Industry trade group, lots of information on methanol's use in fuel cells and as an alternative fuel.
* [http://www.ensec.org/index.php?option=com_content&view=article&id=148:chinatakesgoldinmethanolfuel&catid=82:asia&Itemid=324 China Takes Gold in Methanol Fuel]
*[http://www.setamericafree.org/Rnichols.pdf The methanol story: a sustainable fuel for the future] article by Ford Motor's Roberta Nichols, the mother of the flexible fuel vehicle, discussing Gasoline-Ethanol-Methanol flexibility in the Journal of Scientific & Industrial Research
*[http://www.labnews.co.uk/new_labnews/article.php?artid=1017&categoryid=2&scheme=2 Methanol Discovered in Space]
* Calculation of [http://ddbonline.ddbst.de/AntoineCalculation/AntoineCalculationCGI.exe?component=Methanol vapor pressure], [http://ddbonline.ddbst.de/DIPPR105DensityCalculation/DIPPR105CalculationCGI.exe?component=Methanol liquid density], [http://ddbonline.ddbst.de/VogelCalculation/VogelCalculationCGI.exe?component=Methanol dynamic liquid viscosity], [http://ddbonline.ddbst.de/DIPPR106SFTCalculation/DIPPR106SFTCalculationCGI.exe?component=Methanol surface tension] of methanol

[[Category:Alcohols]]

{{Imported from Wikipedia|name=Methanol|id=306061590}}