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Ethanol

December 25, 2023

For ethanol as a drug or medicine, see Alcohol (drug) and Alcohols (medicine).
Not to be confused with Ethenol or Ethynol.

Ethanol (also called ethyl alcohol, grain alcohol, drinking alcohol, or simply alcohol) is an organic compound with the chemical formula CH3CH2OH. It is an alcohol, with its formula also written as C2H5OH, C2H6O or EtOH, where Et stands for ethyl. Ethanol is a volatile, flammable, colorless liquid with a characteristic wine-like odor and pungent taste.[13][14] It is a psychoactive recreational drug, and the active ingredient in alcoholic drinks.

Ethanol
Full structural formula of ethanol
Skeletal formula of ethanol
Ball-and-stick model of ethanol
Space-filling model of ethanol
Names
Pronunciation /ˈɛθənɒl/
Preferred IUPAC name
Ethanol[1]
Other names
  • Absolute alcohol
  • Alcohol
  • Cologne spirit
  • Drinking alcohol
  • Ethylic alcohol
  • EtOH
  • Ethyl alcohol
  • Ethyl hydroxide
  • Ethylene hydrate
  • Ethylol
  • Grain alcohol
  • Hydroxyethane
  • Methylcarbinol
Identifiers
  • 64-17-5 Y
3D model (JSmol)
  • Interactive image
3DMet
  • B01253
1718733
ChEBI
  • CHEBI:16236 Y
ChEMBL
  • ChEMBL545 Y
ChemSpider
  • 682 Y
DrugBank
  • DB00898 Y
ECHA InfoCard 100.000.526
787
  • 2299
KEGG
  • C00469
  • 702
UNII
  • 3K9958V90M Y
UN number UN 1170
  • DTXSID9020584
  • InChI=1S/C2H6O/c1-2-3/h3H,2H2,1H3 Y
    Key: LFQSCWFLJHTTHZ-UHFFFAOYSA-N Y
  • InChI=1/C2H6O/c1-2-3/h3H,2H2,1H3
    Key: LFQSCWFLJHTTHZ-UHFFFAOYAB
  • OCC
Properties
C2H6O
Molar mass 46.069 g·mol−1
Appearance Colourless liquid
Odor wine-like, pungent[2]
Density 0.78945 g/cm3 (at 20 °C)[3]
Melting point −114.14 ± 0.03[3] °C (−173.45 ± 0.05 °F; 159.01 ± 0.03 K)
Boiling point 78.23 ± 0.09[3] °C (172.81 ± 0.16 °F; 351.38 ± 0.09 K)
Miscible
log P −0.18
Vapor pressure 5.95 kPa (at 20 °C)
Acidity (pKa) 15.9 (H2O), 29.8 (DMSO)[4][5]
−33.60·10−6 cm3/mol
1.3611[3]
Viscosity 1.2 mPa·s (at 20 °C), 1.074 mPa·s (at 25 °C)[6]
1.69 D[7]
Hazards
GHS labelling:
Danger
H225, H319
P210, P233, P240, P241, P242, P305+P351+P338
NFPA 704 (fire diamond)
Health 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
3
0
Flash point 14 °C (Absolute)[9]
Lethal dose or concentration (LD, LC):
  • 7060 mg/kg (oral, rat)
  • 3450 mg/kg (mouse)
[12]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 1000 ppm (1900 mg/m3)[10]
REL (Recommended)
 TWA 1000 ppm (1900 mg/m3)[10]
IDLH (Immediate danger)
 3300 ppm [11]
Safety data sheet (SDS) [8]
Related compounds
Related compounds
Supplementary data page
Ethanol (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)

Ethanol is naturally produced by the fermentation process of sugars by yeasts or via petrochemical processes such as ethylene hydration. Historically it was used as a general anesthetic, and has modern medical applications as an antiseptic, disinfectant, solvent for some medications, and antidote for methanol poisoning and ethylene glycol poisoning.[15][16] It is used as a chemical solvent and in the synthesis of organic compounds, and as a fuel source. Ethanol also can be dehydrated to make ethylene, an important chemical feedstock. As of 2006, world production of ethanol was 51 gigalitres (1.3×1010 US gallons), coming mostly from Brazil and the U.S.[17]

Etymology edit

Ethanol is the systematic name defined by the International Union of Pure and Applied Chemistry for a compound consisting of an alkyl group with two carbon atoms (prefix "eth-"), having a single bond between them (infix "-an-") and an attached −OH functional group (suffix "-ol").[18]

The "eth-" prefix and the qualifier "ethyl" in "ethyl alcohol" originally came from the name "ethyl" assigned in 1834 to the group C
2H
5− by Justus Liebig. He coined the word from the German name Aether of the compound C
2H
5−O−C
2H
5 (commonly called "ether" in English, more specifically called "diethyl ether").[19] According to the Oxford English Dictionary, Ethyl is a contraction of the Ancient Greek αἰθήρ (aithḗr, "upper air") and the Greek word ὕλη (hýlē, "wood, raw material", hence "matter, substance").[20]

The name ethanol was coined as a result of a resolution on naming alcohols and phenols that was adopted at the International Conference on Chemical Nomenclature that was held in April 1892 in Geneva, Switzerland.[21]

The term alcohol now refers to a wider class of substances in chemistry nomenclature, but in common parlance it remains the name of ethanol. It is a medieval loan from Arabic al-kuḥl, a powdered ore of antimony used since antiquity as a cosmetic, and retained that meaning in Middle Latin.[22] The use of 'alcohol' for ethanol (in full, "alcohol of wine") is modern and was first recorded in 1753. Before the late 18th century the term "alcohol" generally referred to any sublimated substance.[23]

Uses edit

Medical edit

Main article: Alcohol (medicine)

Anesthetic edit

Ethanol is the oldest known sedative, used as an oral general anesthetic during surgery in ancient Mesopotamia and in medieval times.[15][16] Mild intoxication starts at a blood alcohol concentration of 0.03-0.05 % and induces anesthetic coma at 0.4%.[24] However, this use carried the high risk of deadly alcohol intoxication and pulmonary aspiration on vomit, which led to use of alternatives in antiquity, such as opium and cannabis, and later diethyl ether starting in the 1840s.[25]

Antiseptic edit

Ethanol is used in medical wipes and most commonly in antibacterial hand sanitizer gels as an antiseptic for its bactericidal and anti-fungal effects.[26] Ethanol kills microorganisms by dissolving their membrane lipid bilayer and denaturing their proteins, and is effective against most bacteria, fungi and viruses. However, it is ineffective against bacterial spores, but that can be alleviated by using hydrogen peroxide.[27]

A solution of 70% ethanol is more effective than pure ethanol because ethanol relies on water molecules for optimal antimicrobial activity. Absolute ethanol may inactivate microbes without destroying them because the alcohol is unable to fully permeate the microbe's membrane.[28][29] Ethanol can also be used as a disinfectant and antiseptic because it causes cell dehydration by disrupting the osmotic balance across the cell membrane, so water leaves the cell leading to cell death.[30]

Antidote edit

Ethanol may be administered as an antidote to ethylene glycol poisoning[31] and methanol poisoning.[32] Ethanol serves this process by acting as a competitive inhibitor against methanol and ethylene glycol for alcohol dehydrogenase.[33] Though it has more side effects, ethanol is less expensive and more readily available than fomepizole, which is also used as an antidote for methanol and ethylene glycol poisoning.[34]

Medicinal solvent edit

Ethanol, often in high concentrations, is used to dissolve many water-insoluble medications and related compounds. Liquid preparations of pain medications, cough and cold medicines, and mouth washes, for example, may contain up to 25% ethanol[35] and may need to be avoided in individuals with adverse reactions to ethanol such as alcohol-induced respiratory reactions.[36] Ethanol is present mainly as an antimicrobial preservative in over 700 liquid preparations of medicine including acetaminophen, iron supplements, ranitidine, furosemide, mannitol, phenobarbital, trimethoprim/sulfamethoxazole and over-the-counter cough medicine.[37]

Pharmacology edit

In mammals, ethanol is primarily metabolized in the liver and stomach by alcohol dehydrogenase (ADH) enzymes.[38] These enzymes catalyze the oxidation of ethanol into acetaldehyde (ethanal):[39]

CH3CH2OH + NAD+ → CH3CHO + NADH + H+

When present in significant concentrations, this metabolism of ethanol is additionally aided by the cytochrome P450 enzyme CYP2E1 in humans, while trace amounts are also metabolized by catalase.[40]

The resulting intermediate, acetaldehyde, is a known carcinogen, and poses significantly greater toxicity in humans than ethanol itself. Many of the symptoms typically associated with alcohol intoxication—as well as many of the health hazards typically associated with the long-term consumption of ethanol—can be attributed to acetaldehyde toxicity in humans.[41]

The subsequent oxidation of acetaldehyde into acetate is performed by aldehyde dehydrogenase (ALDH) enzymes. A mutation in the ALDH2 gene that encodes for an inactive or dysfunctional form of this enzyme affects roughly 50 % of east Asian populations, contributing to the characteristic alcohol flush reaction that can cause temporary reddening of the skin as well as a number of related, and often unpleasant, symptoms of acetaldehyde toxicity.[42] This mutation is typically accompanied by another mutation in the alcohol dehydrogenase enzyme ADH1B in roughly 80 % of east Asians, which improves the catalytic efficiency of converting ethanol into acetaldehyde.[42]

Recreational edit

Main articles: Alcohol (drug) and Alcoholic drink

As a central nervous system depressant, ethanol is one of the most commonly consumed psychoactive drugs.[43]

Despite alcohol's psychoactive, addictive, and carcinogenic properties, it is readily available and legal for sale in most countries. There are laws regulating the sale, exportation/importation, taxation, manufacturing, consumption, and possession of alcoholic beverages. The most common regulation is prohibition for minors.

Fuel edit

See also: Food vs. fuel
 
Corn vs ethanol production in the United States
  Total corn production (bushels) (left)
  Corn used for Ethanol fuel (bushels) (left)
  Percent of corn used for Ethanol (right)

Engine fuel edit

Main article: Ethanol fuel
Energy content (lower heating value) of some fuels compared with ethanol.
Fuel type MJ/L MJ/kg Research
octane
number
Dry wood (20 % moisture) ~19.5
Methanol 17.9 19.9 108.7[44]
Ethanol 21.2[45] 26.8[45] 108.6[44]
E85
(85 % ethanol, 15 % gasoline)		 25.2 33.2 105
Liquefied natural gas 25.3 ~55
Autogas (LPG)
(60 % propane + 40 % butane)		 26.8 50
Aviation gasoline
(high-octane gasoline, not jet fuel)		 33.5 46.8 100/130 (lean/rich)
Gasohol
(90 % gasoline + 10 % ethanol)		 33.7 47.1 93/94
Regular gasoline/petrol 34.8 44.4[46] min. 91
Premium gasoline/petrol max. 104
Diesel 38.6 45.4 25
Charcoal, extruded 50 23

The largest single use of ethanol is as an engine fuel and fuel additive. Brazil in particular relies heavily upon the use of ethanol as an engine fuel, due in part to its role as one of the world's leading producers of ethanol.[47][48] Gasoline sold in Brazil contains at least 25 % anhydrous ethanol. Hydrous ethanol (about 95% ethanol and 5% water) can be used as fuel in more than 90 % of new gasoline-fueled cars sold in the country.

The US and many other countries primarily use E10 (10 % ethanol, sometimes known as gasohol) and E85 (85 % ethanol) ethanol/gasoline mixtures. Over time, it is believed that a material portion of the ≈150-billion-US-gallon (570,000,000 m3) per year market for gasoline will begin to be replaced with fuel ethanol.[49]

 
USP grade ethanol for laboratory use

Australian law limits the use of pure ethanol from sugarcane waste to 10 % in automobiles. Older cars (and vintage cars designed to use a slower burning fuel) should have the engine valves upgraded or replaced.[50]

According to an industry advocacy group, ethanol as a fuel reduces harmful tailpipe emissions of carbon monoxide, particulate matter, oxides of nitrogen, and other ozone-forming pollutants.[51] Argonne National Laboratory analyzed greenhouse gas emissions of many different engine and fuel combinations, and found that biodiesel/petrodiesel blend (B20) showed a reduction of 8 %, conventional E85 ethanol blend a reduction of 17 % and cellulosic ethanol 64 %, compared with pure gasoline.[52] Ethanol has a much greater research octane number (RON) than gasoline, meaning it is less prone to pre-ignition, allowing for better ignition advance which means more torque, and efficiency in addition to the lower carbon emissions.[53]

Ethanol combustion in an internal combustion engine yields many of the products of incomplete combustion produced by gasoline and significantly larger amounts of formaldehyde and related species such as acetaldehyde.[54] This leads to a significantly larger photochemical reactivity and more ground level ozone.[55] This data has been assembled into The Clean Fuels Report comparison of fuel emissions[56] and show that ethanol exhaust generates 2.14 times as much ozone as gasoline exhaust.[57] When this is added into the custom Localized Pollution Index of The Clean Fuels Report, the local pollution of ethanol (pollution that contributes to smog) is rated 1.7, where gasoline is 1.0 and higher numbers signify greater pollution.[58] The California Air Resources Board formalized this issue in 2008 by recognizing control standards for formaldehydes as an emissions control group, much like the conventional NOx and reactive organic gases (ROGs).[59]

More than 2 0% of Brazilian cars are able to use 100 % ethanol as fuel, which includes ethanol-only engines and flex-fuel engines.[60] Flex-fuel engines in Brazil are able to work with all ethanol, all gasoline or any mixture of both. In the United States, flex-fuel vehicles can run on 0 % to 85 % ethanol (15 % gasoline) since higher ethanol blends are not yet allowed or efficient. Brazil supports this fleet of ethanol-burning automobiles with large national infrastructure that produces ethanol from domestically grown sugarcane.

Ethanol's high miscibility with water makes it unsuitable for shipping through modern pipelines like liquid hydrocarbons.[61] Mechanics have seen increased cases of damage to small engines (in particular, the carburetor) and attribute the damage to the increased water retention by ethanol in fuel.[62]

 
Ethanol pump station in São Paulo, Brazil
 
A Ford Taurus fueled by ethanol in New York City
 
U.S. Postal Service truck running on E85 in Minnesota

Rocket fuel edit

Ethanol was commonly used as fuel in early bipropellant rocket (liquid-propelled) vehicles, in conjunction with an oxidizer such as liquid oxygen. The German A-4 ballistic rocket of World War II (better known by its propaganda name V-2),[63] which is credited as having begun the space age, used ethanol as the main constituent of B-Stoff. Under such nomenclature, the ethanol was mixed with 25% water to reduce the combustion chamber temperature.[64][65] The V-2's design team helped develop U.S. rockets following World War II, including the ethanol-fueled Redstone rocket, which launched the first U.S. satellite.[66] Alcohols fell into general disuse as more energy-dense rocket fuels were developed,[65] although ethanol is currently used in lightweight rocket-powered racing aircraft.[67]

Fuel cells edit

Commercial fuel cells operate on reformed natural gas, hydrogen or methanol. Ethanol is an attractive alternative due to its wide availability, low cost, high purity and low toxicity. There is a wide range of fuel cell concepts that have entered trials including direct-ethanol fuel cells, auto-thermal reforming systems and thermally integrated systems. The majority of work is being conducted at a research level although there are a number of organizations at the beginning of the commercialization of ethanol fuel cells.[68]

Household heating and cooking edit

Ethanol fireplaces can be used for home heating or for decoration. Ethanol can also be used as stove fuel for cooking.[69][70]

Feedstock edit

Further information: § Reactions

Ethanol is an important industrial ingredient. It has widespread use as a precursor for other organic compounds such as ethyl halides, ethyl esters, diethyl ether, acetic acid, and ethyl amines.

Solvent edit

Ethanol is considered a universal solvent, as its molecular structure allows for the dissolving of both polar, hydrophilic and nonpolar, hydrophobic compounds. As ethanol also has a low boiling point, it is easy to remove from a solution that has been used to dissolve other compounds, making it a popular extracting agent for botanical oils. Cannabis oil extraction methods often use ethanol as an extraction solvent,[71] and also as a post-processing solvent to remove oils, waxes, and chlorophyll from solution in a process known as winterization.

Ethanol is found in paints, tinctures, markers, and personal care products such as mouthwashes, perfumes and deodorants. Polysaccharides precipitate from aqueous solution in the presence of alcohol, and ethanol precipitation is used for this reason in the purification of DNA and RNA.

Low-temperature liquid edit

Because of its low freezing point of −114 °C (−173 °F) and low toxicity, ethanol is sometimes used in laboratories (with dry ice or other coolants) as a cooling bath to keep vessels at temperatures below the freezing point of water. For the same reason, it is also used as the active fluid in alcohol thermometers.

Chemistry edit

Further information: Ethanol (data page)

Chemical formula edit

Ethanol is a 2-carbon alcohol. Its molecular formula is CH3CH2OH. The structure of the molecule of ethanol is CH3−CH2−OH (an ethyl group linked to a hydroxyl group), which indicates that the carbon of a methyl group (CH3−) is attached to the carbon of a methylene group (−CH2–), which is attached to the oxygen of a hydroxyl group (−OH). It is a constitutional isomer of dimethyl ether. Ethanol is sometimes abbreviated as EtOH, using the common organic chemistry notation of representing the ethyl group (C2H5−) with Et.

Physical properties edit

 
Ethanol burning with its spectrum depicted

Ethanol is a volatile, colorless liquid that has a slight odor. It burns with a smokeless blue flame that is not always visible in normal light. The physical properties of ethanol stem primarily from the presence of its hydroxyl group and the shortness of its carbon chain. Ethanol's hydroxyl group is able to participate in hydrogen bonding, rendering it more viscous and less volatile than less polar organic compounds of similar molecular weight, such as propane.

Ethanol's adiabatic flame temperature for combustion in air is 2082 °C or 3779 °F.[72]

Ethanol is slightly more refractive than water, having a refractive index of 1.36242 (at λ=589.3 nm and 18.35 °C or 65.03 °F).[73] The triple point for ethanol is 150 ± 20 K.[74]

Solvent properties edit

Ethanol is a versatile solvent, miscible with water and with many organic solvents, including acetic acid, acetone, benzene, carbon tetrachloride, chloroform, diethyl ether, ethylene glycol, glycerol, nitromethane, pyridine, and toluene. Its main use as a solvent is in making tincture of iodine, cough syrups, etc.[73][75] It is also miscible with light aliphatic hydrocarbons, such as pentane and hexane, and with aliphatic chlorides such as trichloroethane and tetrachloroethylene.[75]

Ethanol's miscibility with water contrasts with the immiscibility of longer-chain alcohols (five or more carbon atoms), whose water miscibility decreases sharply as the number of carbons increases.[76] The miscibility of ethanol with alkanes is limited to alkanes up to undecane: mixtures with dodecane and higher alkanes show a miscibility gap below a certain temperature (about 13 °C for dodecane[77]). The miscibility gap tends to get wider with higher alkanes, and the temperature for complete miscibility increases.

Ethanol-water mixtures have less volume than the sum of their individual components at the given fractions. Mixing equal volumes of ethanol and water results in only 1.92 volumes of mixture.[73][78] Mixing ethanol and water is exothermic, with up to 777 J/mol[79] being released at 298 K.

Mixtures of ethanol and water form an azeotrope at about 89 mole-% ethanol and 11 mole-% water[80] or a mixture of 95.6% ethanol by mass (or about 97% alcohol by volume) at normal pressure, which boils at 351 K (78 °C). This azeotropic composition is strongly temperature- and pressure-dependent and vanishes at temperatures below 303 K.[81]

 
Hydrogen bonding in solid ethanol at −186 °C

Hydrogen bonding causes pure ethanol to be hygroscopic to the extent that it readily absorbs water from the air. The polar nature of the hydroxyl group causes ethanol to dissolve many ionic compounds, notably sodium and potassium hydroxides, magnesium chloride, calcium chloride, ammonium chloride, ammonium bromide, and sodium bromide.[75] Sodium and potassium chlorides are slightly soluble in ethanol.[75] Because the ethanol molecule also has a nonpolar end, it will also dissolve nonpolar substances, including most essential oils[82] and numerous flavoring, coloring, and medicinal agents.

The addition of even a few percent of ethanol to water sharply reduces the surface tension of water. This property partially explains the "tears of wine" phenomenon. When wine is swirled in a glass, ethanol evaporates quickly from the thin film of wine on the wall of the glass. As the wine's ethanol content decreases, its surface tension increases and the thin film "beads up" and runs down the glass in channels rather than as a smooth sheet.

Flammability edit

An ethanol–water solution will catch fire if heated above a temperature called its flash point and an ignition source is then applied to it.[83] For 20% alcohol by mass (about 25% by volume), this will occur at about 25 °C (77 °F). The flash point of pure ethanol is 13 °C (55 °F),[84] but may be influenced very slightly by atmospheric composition such as pressure and humidity. Ethanol mixtures can ignite below average room temperature. Ethanol is considered a flammable liquid (Class 3 Hazardous Material) in concentrations above 2.35% by mass (3.0% by volume; 6 proof).[85][86][87]

Flash points of ethanol–water mixtures[88][86][89]
Ethanol
mass fraction, % 		Temperature
°C °F
1 84.5 184.1[86]
2 64 147[86]
2.35 60 140[86][85]
3 51.5 124.7[86]
5 43 109[88]
6 39.5 103.1[86]
10 31 88[88]
20 25 77[86]
30 24 75[88]
40 21.9 71.4[citation needed][88]
50 20 68[88][86]
60 17.9 64.2[citation needed][88]
70 16 61[88]
80 15.8 60.4[86]
90 14 57[88]
100 12.5 54.5[88][86][84]

Dishes using burning alcohol for culinary effects are called flambé.

Natural occurrence edit

Ethanol is a byproduct of the metabolic process of yeast. As such, ethanol will be present in any yeast habitat. Ethanol can commonly be found in overripe fruit.[90] Ethanol produced by symbiotic yeast can be found in bertam palm blossoms. Although some animal species, such as the pentailed treeshrew, exhibit ethanol-seeking behaviors, most show no interest or avoidance of food sources containing ethanol.[91] Ethanol is also produced during the germination of many plants as a result of natural anaerobiosis.[92] Ethanol has been detected in outer space, forming an icy coating around dust grains in interstellar clouds.[93] Minute quantity amounts (average 196 ppb) of endogenous ethanol and acetaldehyde were found in the exhaled breath of healthy volunteers.[94] Auto-brewery syndrome, also known as gut fermentation syndrome, is a rare medical condition in which intoxicating quantities of ethanol are produced through endogenous fermentation within the digestive system.[95]

Production edit

 
94% denatured ethanol sold in a bottle for household use

Ethanol is produced both as a petrochemical, through the hydration of ethylene and, via biological processes, by fermenting sugars with yeast.[96] Which process is more economical depends on prevailing prices of petroleum and grain feed stocks.

Sources edit

World production of ethanol in 2006 was 51 gigalitres (1.3×1010 US gal), with 69% of the world supply coming from Brazil and the U.S.[17] Brazilian ethanol is produced from sugarcane, which has relatively high yields (830% more fuel than the fossil fuels used to produce it) compared to some other energy crops.[97] Sugarcane not only has a greater concentration of sucrose than corn (by about 30%), but is also much easier to extract. The bagasse generated by the process is not discarded, but burned by power plants to produce electricity. Bagasse burning accounts for around 9% of the electricity produced in Brazil.[98]

In the 1970s most industrial ethanol in the U.S. was made as a petrochemical, but in the 1980s the U.S. introduced subsidies for corn-based ethanol.[99] According to the Renewable Fuels Association, as of 30 October 2007, 131 grain ethanol bio-refineries in the U.S. have the capacity to produce 7×10^9 US gal (26,000,000 m3) of ethanol per year. An additional 72 construction projects underway (in the U.S.) can add 6.4 billion US gallons (24,000,000 m3) of new capacity in the next 18 months.[49]

In India ethanol is made from sugarcane.[100] Sweet sorghum is another potential source of ethanol, and is suitable for growing in dryland conditions. The International Crops Research Institute for the Semi-Arid Tropics is investigating the possibility of growing sorghum as a source of fuel, food, and animal feed in arid parts of Asia and Africa.[101] Sweet sorghum has one-third the water requirement of sugarcane over the same time period. It also requires about 22% less water than corn. The world's first sweet sorghum ethanol distillery began commercial production in 2007 in Andhra Pradesh, India.[102]

Hydration edit

Ethanol can be produced from petrochemical feed stocks, primarily by the acid-catalyzed hydration of ethylene. It is often referred to as synthetic ethanol.

C
2H
4 + H
2O → CH
3CH
2OH

The catalyst is most commonly phosphoric acid,[103][104] adsorbed onto a porous support such as silica gel or diatomaceous earth. This catalyst was first used for large-scale ethanol production by the Shell Oil Company in 1947.[105] The reaction is carried out in the presence of high pressure steam at 300 °C (572 °F) where a 5:3 ethylene to steam ratio is maintained.[106][107] This process was used on an industrial scale by Union Carbide Corporation and others. It is no longer practiced in the US as fermentation ethanol produced from corn is more economical.[108]

In an older process, first practiced on the industrial scale in 1930 by Union Carbide[109] but now almost entirely obsolete, ethylene was hydrated indirectly by reacting it with concentrated sulfuric acid to produce ethyl sulfate, which was hydrolyzed to yield ethanol and regenerate the sulfuric acid:[110]

C
2H
4 + H
2SO
4 → CH
3CH
2SO
4H
CH
3CH
2SO
4H + H
2O → CH
3CH
2OH + H
2SO
4

From carbon dioxide edit

Ethanol has been produced in the laboratory by converting carbon dioxide via biological and electrochemical reactions.[111][112]

CO2 + H
2O → CH
3CH
2OH + side products

Fermentation edit

Main article: Ethanol fermentation
See also: Yeast in winemaking

Ethanol in alcoholic beverages and fuel is produced by fermentation. Certain species of yeast (e.g., Saccharomyces cerevisiae) metabolize sugar (namely polysaccharides), producing ethanol and carbon dioxide. The chemical equations below summarize the conversion:

C
6H
12O
6 → 2 CH
3CH
2OH + 2 CO2
C
12H
22O
11 + H
2O → 4 CH
3CH
2OH + 4 CO2

Fermentation is the process of culturing yeast under favorable thermal conditions to produce alcohol. This process is carried out at around 35–40 °C (95–104 °F). Toxicity of ethanol to yeast limits the ethanol concentration obtainable by brewing; higher concentrations, therefore, are obtained by fortification or distillation. The most ethanol-tolerant yeast strains can survive up to approximately 18% ethanol by volume.

To produce ethanol from starchy materials such as cereals, the starch must first be converted into sugars. In brewing beer, this has traditionally been accomplished by allowing the grain to germinate, or malt, which produces the enzyme amylase. When the malted grain is mashed, the amylase converts the remaining starches into sugars.

Cellulose edit

Main article: Cellulosic ethanol

Sugars for ethanol fermentation can be obtained from cellulose. Deployment of this technology could turn a number of cellulose-containing agricultural by-products, such as corncobs, straw, and sawdust, into renewable energy resources. Other agricultural residues such as sugarcane bagasse and energy crops such as switchgrass may also be fermentable sugar sources.[113]

Testing edit

 
Infrared reflection spectra of liquid ethanol, showing the −OH band centered near 3300 cm−1 and C−H bands near 2950 cm−1
 
Near-infrared spectrum of liquid ethanol

Breweries and biofuel plants employ two methods for measuring ethanol concentration. Infrared ethanol sensors measure the vibrational frequency of dissolved ethanol using the C−H band at 2900 cm−1. This method uses a relatively inexpensive solid-state sensor that compares the C−H band with a reference band to calculate the ethanol content. The calculation makes use of the Beer–Lambert law. Alternatively, by measuring the density of the starting material and the density of the product, using a hydrometer, the change in specific gravity during fermentation indicates the alcohol content. This inexpensive and indirect method has a long history in the beer brewing industry.

Purification edit

Distillation edit

Ethylene hydration or brewing produces an ethanol–water mixture. For most industrial and fuel uses, the ethanol must be purified. Fractional distillation at atmospheric pressure can concentrate ethanol to 95.6% by weight (89.5 mole%). This mixture is an azeotrope with a boiling point of 78.1 °C (172.6 °F), and cannot be further purified by distillation. Addition of an entraining agent, such as benzene, cyclohexane, or heptane, allows a new ternary azeotrope comprising the ethanol, water, and the entraining agent to be formed. This lower-boiling ternary azeotrope is removed preferentially, leading to water-free ethanol.[104]

Molecular sieves and desiccants edit

Apart from distillation, ethanol may be dried by addition of a desiccant, such as molecular sieves, cellulose, or cornmeal. The desiccants can be dried and reused.[104] Molecular sieves can be used to selectively absorb the water from the 95.6% ethanol solution.[114] Molecular sieves of pore-size 3 Ångstrom, a type of zeolite, effectively sequester water molecules while excluding ethanol molecules. Heating the wet sieves drives out the water, allowing regeneration of their desiccant capability.[115]

Membranes and reverse osmosis edit

Membranes can also be used to separate ethanol and water. Membrane-based separations are not subject to the limitations of the water-ethanol azeotrope because the separations are not based on vapor-liquid equilibria. Membranes are often used in the so-called hybrid membrane distillation process. This process uses a pre-concentration distillation column as the first separating step. The further separation is then accomplished with a membrane operated either in vapor permeation or pervaporation mode. Vapor permeation uses a vapor membrane feed and pervaporation uses a liquid membrane feed.

Other techniques edit

A variety of other techniques have been discussed, including the following:[104]

Grades of ethanol edit

Denatured alcohol edit

Main article: Denatured alcohol

Pure ethanol and alcoholic beverages are heavily taxed as psychoactive drugs, but ethanol has many uses that do not involve its consumption. To relieve the tax burden on these uses, most jurisdictions waive the tax when an agent has been added to the ethanol to render it unfit to drink. These include bittering agents such as denatonium benzoate and toxins such as methanol, naphtha, and pyridine. Products of this kind are called denatured alcohol.[118][119]

Absolute alcohol edit

Absolute or anhydrous alcohol refers to ethanol with a low water content. There are various grades with maximum water contents ranging from 1% to a few parts per million (ppm). If azeotropic distillation is used to remove water, it will contain trace amounts of the material separation agent (e.g. benzene).[120] Absolute alcohol is not intended for human consumption. Absolute ethanol is used as a solvent for laboratory and industrial applications, where water will react with other chemicals, and as fuel alcohol. Spectroscopic ethanol is an absolute ethanol with a low absorbance in ultraviolet and visible light, fit for use as a solvent in ultraviolet-visible spectroscopy.[121]

Pure ethanol is classed as 200 proof in the US, equivalent to 175 degrees proof in the UK system.[122]

Rectified spirits edit

Rectified spirit, an azeotropic composition of 96% ethanol containing 4% water, is used instead of anhydrous ethanol for various purposes. Spirits of wine are about 94% ethanol (188 proof). The impurities are different from those in 95% (190 proof) laboratory ethanol.[123]

Reactions edit

Further information: Alcohol (chemistry)

Ethanol is classified as a primary alcohol, meaning that the carbon that its hydroxyl group attaches to has at least two hydrogen atoms attached to it as well. Many ethanol reactions occur at its hydroxyl group.

Ester formation edit

In the presence of acid catalysts, ethanol reacts with carboxylic acids to produce ethyl esters and water:

RCOOH + HOCH2CH3 → RCOOCH2CH3 + H2O

This reaction, which is conducted on large scale industrially, requires the removal of the water from the reaction mixture as it is formed. Esters react in the presence of an acid or base to give back the alcohol and a salt. This reaction is known as saponification because it is used in the preparation of soap. Ethanol can also form esters with inorganic acids. Diethyl sulfate and triethyl phosphate are prepared by treating ethanol with sulfur trioxide and phosphorus pentoxide respectively. Diethyl sulfate is a useful ethylating agent in organic synthesis. Ethyl nitrite, prepared from the reaction of ethanol with sodium nitrite and sulfuric acid, was formerly used as a diuretic.

Dehydration edit

In the presence of acid catalysts, alcohols can be converted to alkenes such as ethanol to ethylene. Typically solid acids such as alumina are used.[124]

   CH3CH2OH → H2C=CH2 + H2O

Since water is removed from the same molecule, the reaction is known as intramolecular dehydration. Intramolecular dehydration of an alcohol requires a high temperature and the presence of an acid catalyst such as sulfuric acid.[125]

Ethylene produced from sugar-derived ethanol (primarily in Brazil) competes with ethylene produced from petrochemical feedstocks such as naphtha and ethane.

At a lower temperature than that of intramolecular dehydration, intermolecular alcohol dehydration may occur producing a symmetrical ether. This is a condensation reaction. In the following example, diethyl ether is produced from ethanol:

2 CH3CH2OH → CH3CH2OCH2CH3 + H2O[126]

Combustion edit

Complete combustion of ethanol forms carbon dioxide and water:

C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l); −ΔHc = 1371 kJ/mol[127] = 29.8 kJ/g = 327 kcal/mol = 7.1 kcal/g
C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (g); −ΔHc = 1236 kJ/mol = 26.8 kJ/g = 295.4 kcal/mol = 6.41 kcal/g[128]

Specific heat = 2.44 kJ/(kg·K)

Acid-base chemistry edit

Ethanol is a neutral molecule and the pH of a solution of ethanol in water is nearly 7.00. Ethanol can be quantitatively converted to its conjugate base, the ethoxide ion (CH3CH2O−), by reaction with an alkali metal such as sodium:[76]

2 CH3CH2OH + 2 Na → 2 CH3CH2ONa + H2

or a very strong base such as sodium hydride:

CH3CH2OH + NaH → CH3CH2ONa + H2

The acidities of water and ethanol are nearly the same, as indicated by their pKa of 15.7 and 16 respectively. Thus, sodium ethoxide and sodium hydroxide exist in an equilibrium that is closely balanced:

CH3CH2OH + NaOH ⇌ CH3CH2ONa + H2O

Halogenation edit

Ethanol is not used industrially as a precursor to ethyl halides, but the reactions are illustrative. Ethanol reacts with hydrogen halides to produce ethyl halides such as ethyl chloride and ethyl bromide via an SN2 reaction:

CH3CH2OH + HCl → CH3CH2Cl + H2O

HCl requires a catalyst such as zinc chloride.[110] HBr requires refluxing with a sulfuric acid catalyst.[110] Ethyl halides can, in principle, also be produced by treating ethanol with more specialized halogenating agents, such as thionyl chloride or phosphorus tribromide.[76][110]

CH3CH2OH + SOCl2 → CH3CH2Cl + SO2 + HCl

Upon treatment with halogens in the presence of base, ethanol gives the corresponding haloform (CHX3, where X = Cl, Br, I). This conversion is called the haloform reaction.[129] An intermediate in the reaction with chlorine is the aldehyde called chloral, which forms chloral hydrate upon reaction with water:[130]

4 Cl2 + CH3CH2OH → CCl3CHO + 5 HCl
CCl3CHO + H2O → CCl3C(OH)2H

Oxidation edit

Ethanol can be oxidized to acetaldehyde and further oxidized to acetic acid, depending on the reagents and conditions.[110] This oxidation is of no importance industrially, but in the human body, these oxidation reactions are catalyzed by the enzyme liver alcohol dehydrogenase. The oxidation product of ethanol, acetic acid, is a nutrient for humans, being a precursor to acetyl CoA, where the acetyl group can be spent as energy or used for biosynthesis.

Metabolism edit

Ethanol is similar to macronutrients such as proteins, fats, and carbohydrates in that it provides calories. When consumed and metabolized, it contributes 7 kilocalories per gram via ethanol metabolism.[131]

Safety edit

See also: Alcohol (chemistry) § Toxicity

Ethanol is very flammable and should not be used around an open flame.

Pure ethanol will irritate the skin and eyes.[132] Nausea, vomiting, and intoxication are symptoms of ingestion. Long-term use by ingestion can result in serious liver damage.[133] Atmospheric concentrations above one part per thousand are above the European Union occupational exposure limits.[133]

History edit

Further information: Liquor

The fermentation of sugar into ethanol is one of the earliest biotechnologies employed by humans. Ethanol has historically been identified variously as spirit of wine or ardent spirits,[134] and as aqua vitae or aqua vita. The intoxicating effects of its consumption have been known since ancient times. Ethanol has been used by humans since prehistory as the intoxicating ingredient of alcoholic beverages. Dried residue on 9,000-year-old pottery found in China suggests that Neolithic people consumed alcoholic beverages.[135]

The inflammable nature of the exhalations of wine was already known to ancient natural philosophers such as Aristotle (384–322 BCE), Theophrastus (c. 371–287 BCE), and Pliny the Elder (23/24–79 CE).[136] However, this did not immediately lead to the isolation of ethanol, even despite the development of more advanced distillation techniques in second- and third-century Roman Egypt.[137] An important recognition, first found in one of the writings attributed to Jābir ibn Ḥayyān (ninth century CE), was that by adding salt to boiling wine, which increases the wine's relative volatility, the flammability of the resulting vapors may be enhanced.[138] The distillation of wine is attested in Arabic works attributed to al-Kindī (c. 801–873 CE) and to al-Fārābī (c. 872–950), and in the 28th book of al-Zahrāwī's (Latin: Abulcasis, 936–1013) Kitāb al-Taṣrīf (later translated into Latin as Liber servatoris).[139] In the twelfth century, recipes for the production of aqua ardens ("burning water", i.e., ethanol) by distilling wine with salt started to appear in a number of Latin works, and by the end of the thirteenth century it had become a widely known substance among Western European chemists.[140]

The works of Taddeo Alderotti (1223–1296) describe a method for concentrating ethanol involving repeated fractional distillation through a water-cooled still, by which an ethanol purity of 90% could be obtained.[141] The medicinal properties of ethanol were studied by Arnald of Villanova (1240–1311 CE) and John of Rupescissa (c. 1310–1366), the latter of whom regarded it as a life-preserving substance able to prevent all diseases (the aqua vitae or "water of life", also called by John the quintessence of wine).[142]

In China, archaeological evidence indicates that the true distillation of alcohol began during the Jin (1115–1234) or Southern Song (1127–1279) dynasties.[143] A still has been found at an archaeological site in Qinglong, Hebei, dating to the 12th century.[143] In India, the true distillation of alcohol was introduced from the Middle East, and was in wide use in the Delhi Sultanate by the 14th century.[144]

In 1796, German-Russian chemist Johann Tobias Lowitz obtained pure ethanol by mixing partially purified ethanol (the alcohol-water azeotrope) with an excess of anhydrous alkali and then distilling the mixture over low heat.[145] French chemist Antoine Lavoisier described ethanol as a compound of carbon, hydrogen, and oxygen, and in 1807 Nicolas-Théodore de Saussure determined ethanol's chemical formula.[146][147] Fifty years later, Archibald Scott Couper published the structural formula of ethanol. It was one of the first structural formulas determined.[148]

Ethanol was first prepared synthetically in 1825 by Michael Faraday. He found that sulfuric acid could absorb large volumes of coal gas.[149] He gave the resulting solution to Henry Hennell, a British chemist, who found in 1826 that it contained "sulphovinic acid" (ethyl hydrogen sulfate).[150] In 1828, Hennell and the French chemist Georges-Simon Serullas independently discovered that sulphovinic acid could be decomposed into ethanol.[151][152] Thus, in 1825 Faraday had unwittingly discovered that ethanol could be produced from ethylene (a component of coal gas) by acid-catalyzed hydration, a process similar to current industrial ethanol synthesis.[153]

Ethanol was used as lamp fuel in the U.S. as early as 1840, but a tax levied on industrial alcohol during the Civil War made this use uneconomical. The tax was repealed in 1906.[154] Use as an automotive fuel dates back to 1908, with the Ford Model T able to run on petrol (gasoline) or ethanol.[155] It fuels some spirit lamps.

Ethanol intended for industrial use is often produced from ethylene.[156] Ethanol has widespread use as a solvent of substances intended for human contact or consumption, including scents, flavorings, colorings, and medicines. In chemistry, it is both a solvent and a feedstock for the synthesis of other products. It has a long history as a fuel for heat and light, and more recently as a fuel for internal combustion engines.

See also edit

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Further reading edit

  • Boyce JM, Pittet D (2003). "Hand Hygiene in Healthcare Settings". Atlanta, GA: Centers for Disease Control..
  • Onuki S, Koziel JA, van Leeuwen J, Jenks WS, Grewell D, Cai L (June 2008). Ethanol production, purification, and analysis techniques: a review. 2008 ASABE Annual International Meeting. Providence, RI. Retrieved 16 February 2013.
  • "Explanation of US denatured alcohol designations". Sci-toys.
  • Lange, Norbert Adolph (1967). John Aurie Dean (ed.). Lange's Handbook of Chemistry (10th ed.). McGraw-Hill.

External links edit

 
Look up alcohol or ethanol in Wiktionary, the free dictionary.
 
Wikimedia Commons has media related to Ethanol.
  • Alcohol (Ethanol) at The Periodic Table of Videos (University of Nottingham)
  • International Labour Organization ethanol safety information
  • National Pollutant Inventory – Ethanol Fact Sheet
  • CDC – NIOSH Pocket Guide to Chemical Hazards – Ethyl Alcohol
  • National Institute of Standards and Technology chemical data on ethanol
  • Chicago Board of Trade news and market data on ethanol futures
  • Calculation of vapor pressure, liquid density, dynamic liquid viscosity, surface tension of ethanol
  • A look into the history of ethanol
  • ChemSub Online: Ethyl alcohol

December 25, 2023
ethanol, ethanol, drug, medicine, alcohol, drug, alcohols, medicine, confused, with, ethenol, ethynol, also, called, ethyl, alcohol, grain, alcohol, drinking, alcohol, simply, alcohol, organic, compound, with, chemical, formula, ch3ch2oh, alcohol, with, formul. For ethanol as a drug or medicine see Alcohol drug and Alcohols medicine Not to be confused with Ethenol or Ethynol Ethanol also called ethyl alcohol grain alcohol drinking alcohol or simply alcohol is an organic compound with the chemical formula CH3CH2OH It is an alcohol with its formula also written as C2H5OH C2H6O or EtOH where Et stands for ethyl Ethanol is a volatile flammable colorless liquid with a characteristic wine like odor and pungent taste 13 14 It is a psychoactive recreational drug and the active ingredient in alcoholic drinks Ethanol Full structural formula of ethanol Skeletal formula of ethanolBall and stick model of ethanol Space filling model of ethanolNamesPronunciation ˈ ɛ 8 e n ɒ l Preferred IUPAC name Ethanol 1 Other names Absolute alcoholAlcoholCologne spiritDrinking alcoholEthylic alcoholEtOHEthyl alcoholEthyl hydroxideEthylene hydrateEthylolGrain alcoholHydroxyethaneMethylcarbinolIdentifiersCAS Number 64 17 5 Y3D model JSmol Interactive image3DMet B01253Beilstein Reference 1718733ChEBI CHEBI 16236 YChEMBL ChEMBL545 YChemSpider 682 YDrugBank DB00898 YECHA InfoCard 100 000 526Gmelin Reference 787IUPHAR BPS 2299KEGG C00469PubChem CID 702UNII 3K9958V90M YUN number UN 1170CompTox Dashboard EPA DTXSID9020584InChI InChI 1S C2H6O c1 2 3 h3H 2H2 1H3 YKey LFQSCWFLJHTTHZ UHFFFAOYSA N YInChI 1 C2H6O c1 2 3 h3H 2H2 1H3Key LFQSCWFLJHTTHZ UHFFFAOYABSMILES OCCPropertiesChemical formula C 2H 6OMolar mass 46 069 g mol 1Appearance Colourless liquidOdor wine like pungent 2 Density 0 78945 g cm3 at 20 C 3 Melting point 114 14 0 03 3 C 173 45 0 05 F 159 01 0 03 K Boiling point 78 23 0 09 3 C 172 81 0 16 F 351 38 0 09 K Solubility in water Misciblelog P 0 18Vapor pressure 5 95 kPa at 20 C Acidity pKa 15 9 H2O 29 8 DMSO 4 5 Magnetic susceptibility x 33 60 10 6 cm3 molRefractive index nD 1 3611 3 Viscosity 1 2 mPa s at 20 C 1 074 mPa s at 25 C 6 Dipole moment 1 69 D 7 HazardsGHS labelling PictogramsSignal word DangerHazard statements H225 H319Precautionary statements P210 P233 P240 P241 P242 P305 P351 P338NFPA 704 fire diamond 230Flash point 14 C Absolute 9 Lethal dose or concentration LD LC LD50 median dose 7060 mg kg oral rat 3450 mg kg mouse 12 NIOSH US health exposure limits PEL Permissible TWA 1000 ppm 1900 mg m3 10 REL Recommended TWA 1000 ppm 1900 mg m3 10 IDLH Immediate danger 3300 ppm 11 Safety data sheet SDS 8 Related compoundsRelated compounds EthaneMethanolSupplementary data pageEthanol data page 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 Ethanol is naturally produced by the fermentation process of sugars by yeasts or via petrochemical processes such as ethylene hydration Historically it was used as a general anesthetic and has modern medical applications as an antiseptic disinfectant solvent for some medications and antidote for methanol poisoning and ethylene glycol poisoning 15 16 It is used as a chemical solvent and in the synthesis of organic compounds and as a fuel source Ethanol also can be dehydrated to make ethylene an important chemical feedstock As of 2006 world production of ethanol was 51 gigalitres 1 3 1010 US gallons coming mostly from Brazil and the U S 17 Contents 1 Etymology 2 Uses 2 1 Medical 2 1 1 Anesthetic 2 1 2 Antiseptic 2 1 3 Antidote 2 1 4 Medicinal solvent 2 1 5 Pharmacology 2 2 Recreational 2 3 Fuel 2 3 1 Engine fuel 2 3 2 Rocket fuel 2 3 3 Fuel cells 2 3 4 Household heating and cooking 2 4 Feedstock 2 5 Solvent 2 6 Low temperature liquid 3 Chemistry 3 1 Chemical formula 3 2 Physical properties 3 3 Solvent properties 3 4 Flammability 4 Natural occurrence 5 Production 5 1 Sources 5 2 Hydration 5 3 From carbon dioxide 5 4 Fermentation 5 4 1 Cellulose 5 5 Testing 6 Purification 6 1 Distillation 6 2 Molecular sieves and desiccants 6 3 Membranes and reverse osmosis 6 4 Other techniques 6 5 Grades of ethanol 6 5 1 Denatured alcohol 6 5 2 Absolute alcohol 6 5 3 Rectified spirits 7 Reactions 7 1 Ester formation 7 2 Dehydration 7 3 Combustion 7 4 Acid base chemistry 7 5 Halogenation 7 6 Oxidation 7 7 Metabolism 8 Safety 9 History 10 See also 11 References 12 Further reading 13 External linksEtymology editEthanol is the systematic name defined by the International Union of Pure and Applied Chemistry for a compound consisting of an alkyl group with two carbon atoms prefix eth having a single bond between them infix an and an attached OH functional group suffix ol 18 The eth prefix and the qualifier ethyl in ethyl alcohol originally came from the name ethyl assigned in 1834 to the group C2 H5 by Justus Liebig He coined the word from the German name Aether of the compound C2 H5 O C2 H5 commonly called ether in English more specifically called diethyl ether 19 According to the Oxford English Dictionary Ethyl is a contraction of the Ancient Greek aἰ8hr aithḗr upper air and the Greek word ὕlh hyle wood raw material hence matter substance 20 The name ethanol was coined as a result of a resolution on naming alcohols and phenols that was adopted at the International Conference on Chemical Nomenclature that was held in April 1892 in Geneva Switzerland 21 The term alcohol now refers to a wider class of substances in chemistry nomenclature but in common parlance it remains the name of ethanol It is a medieval loan from Arabic al kuḥl a powdered ore of antimony used since antiquity as a cosmetic and retained that meaning in Middle Latin 22 The use of alcohol for ethanol in full alcohol of wine is modern and was first recorded in 1753 Before the late 18th century the term alcohol generally referred to any sublimated substance 23 Uses editMedical edit Main article Alcohol medicine Anesthetic edit Ethanol is the oldest known sedative used as an oral general anesthetic during surgery in ancient Mesopotamia and in medieval times 15 16 Mild intoxication starts at a blood alcohol concentration of 0 03 0 05 and induces anesthetic coma at 0 4 24 However this use carried the high risk of deadly alcohol intoxication and pulmonary aspiration on vomit which led to use of alternatives in antiquity such as opium and cannabis and later diethyl ether starting in the 1840s 25 Antiseptic edit Ethanol is used in medical wipes and most commonly in antibacterial hand sanitizer gels as an antiseptic for its bactericidal and anti fungal effects 26 Ethanol kills microorganisms by dissolving their membrane lipid bilayer and denaturing their proteins and is effective against most bacteria fungi and viruses However it is ineffective against bacterial spores but that can be alleviated by using hydrogen peroxide 27 A solution of 70 ethanol is more effective than pure ethanol because ethanol relies on water molecules for optimal antimicrobial activity Absolute ethanol may inactivate microbes without destroying them because the alcohol is unable to fully permeate the microbe s membrane 28 29 Ethanol can also be used as a disinfectant and antiseptic because it causes cell dehydration by disrupting the osmotic balance across the cell membrane so water leaves the cell leading to cell death 30 Antidote edit Ethanol may be administered as an antidote to ethylene glycol poisoning 31 and methanol poisoning 32 Ethanol serves this process by acting as a competitive inhibitor against methanol and ethylene glycol for alcohol dehydrogenase 33 Though it has more side effects ethanol is less expensive and more readily available than fomepizole which is also used as an antidote for methanol and ethylene glycol poisoning 34 Medicinal solvent edit Ethanol often in high concentrations is used to dissolve many water insoluble medications and related compounds Liquid preparations of pain medications cough and cold medicines and mouth washes for example may contain up to 25 ethanol 35 and may need to be avoided in individuals with adverse reactions to ethanol such as alcohol induced respiratory reactions 36 Ethanol is present mainly as an antimicrobial preservative in over 700 liquid preparations of medicine including acetaminophen iron supplements ranitidine furosemide mannitol phenobarbital trimethoprim sulfamethoxazole and over the counter cough medicine 37 Pharmacology edit In mammals ethanol is primarily metabolized in the liver and stomach by alcohol dehydrogenase ADH enzymes 38 These enzymes catalyze the oxidation of ethanol into acetaldehyde ethanal 39 CH3CH2OH NAD CH3CHO NADH H When present in significant concentrations this metabolism of ethanol is additionally aided by the cytochrome P450 enzyme CYP2E1 in humans while trace amounts are also metabolized by catalase 40 The resulting intermediate acetaldehyde is a known carcinogen and poses significantly greater toxicity in humans than ethanol itself Many of the symptoms typically associated with alcohol intoxication as well as many of the health hazards typically associated with the long term consumption of ethanol can be attributed to acetaldehyde toxicity in humans 41 The subsequent oxidation of acetaldehyde into acetate is performed by aldehyde dehydrogenase ALDH enzymes A mutation in the ALDH2 gene that encodes for an inactive or dysfunctional form of this enzyme affects roughly 50 of east Asian populations contributing to the characteristic alcohol flush reaction that can cause temporary reddening of the skin as well as a number of related and often unpleasant symptoms of acetaldehyde toxicity 42 This mutation is typically accompanied by another mutation in the alcohol dehydrogenase enzyme ADH1B in roughly 80 of east Asians which improves the catalytic efficiency of converting ethanol into acetaldehyde 42 Recreational edit Main articles Alcohol drug and Alcoholic drink As a central nervous system depressant ethanol is one of the most commonly consumed psychoactive drugs 43 Despite alcohol s psychoactive addictive and carcinogenic properties it is readily available and legal for sale in most countries There are laws regulating the sale exportation importation taxation manufacturing consumption and possession of alcoholic beverages The most common regulation is prohibition for minors Fuel edit See also Food vs fuel nbsp Corn vs ethanol production in the United States Total corn production bushels left Corn used for Ethanol fuel bushels left Percent of corn used for Ethanol right Engine fuel edit Main article Ethanol fuel Energy content lower heating value of some fuels compared with ethanol Fuel type MJ L MJ kg ResearchoctanenumberDry wood 20 moisture 19 5Methanol 17 9 19 9 108 7 44 Ethanol 21 2 45 26 8 45 108 6 44 E85 85 ethanol 15 gasoline 25 2 33 2 105Liquefied natural gas 25 3 55Autogas LPG 60 propane 40 butane 26 8 50Aviation gasoline high octane gasoline not jet fuel 33 5 46 8 100 130 lean rich Gasohol 90 gasoline 10 ethanol 33 7 47 1 93 94Regular gasoline petrol 34 8 44 4 46 min 91Premium gasoline petrol max 104Diesel 38 6 45 4 25Charcoal extruded 50 23The largest single use of ethanol is as an engine fuel and fuel additive Brazil in particular relies heavily upon the use of ethanol as an engine fuel due in part to its role as one of the world s leading producers of ethanol 47 48 Gasoline sold in Brazil contains at least 25 anhydrous ethanol Hydrous ethanol about 95 ethanol and 5 water can be used as fuel in more than 90 of new gasoline fueled cars sold in the country The US and many other countries primarily use E10 10 ethanol sometimes known as gasohol and E85 85 ethanol ethanol gasoline mixtures Over time it is believed that a material portion of the 150 billion US gallon 570 000 000 m3 per year market for gasoline will begin to be replaced with fuel ethanol 49 nbsp USP grade ethanol for laboratory useAustralian law limits the use of pure ethanol from sugarcane waste to 10 in automobiles Older cars and vintage cars designed to use a slower burning fuel should have the engine valves upgraded or replaced 50 According to an industry advocacy group ethanol as a fuel reduces harmful tailpipe emissions of carbon monoxide particulate matter oxides of nitrogen and other ozone forming pollutants 51 Argonne National Laboratory analyzed greenhouse gas emissions of many different engine and fuel combinations and found that biodiesel petrodiesel blend B20 showed a reduction of 8 conventional E85 ethanol blend a reduction of 17 and cellulosic ethanol 64 compared with pure gasoline 52 Ethanol has a much greater research octane number RON than gasoline meaning it is less prone to pre ignition allowing for better ignition advance which means more torque and efficiency in addition to the lower carbon emissions 53 Ethanol combustion in an internal combustion engine yields many of the products of incomplete combustion produced by gasoline and significantly larger amounts of formaldehyde and related species such as acetaldehyde 54 This leads to a significantly larger photochemical reactivity and more ground level ozone 55 This data has been assembled into The Clean Fuels Report comparison of fuel emissions 56 and show that ethanol exhaust generates 2 14 times as much ozone as gasoline exhaust 57 When this is added into the custom Localized Pollution Index of The Clean Fuels Report the local pollution of ethanol pollution that contributes to smog is rated 1 7 where gasoline is 1 0 and higher numbers signify greater pollution 58 The California Air Resources Board formalized this issue in 2008 by recognizing control standards for formaldehydes as an emissions control group much like the conventional NOx and reactive organic gases ROGs 59 More than 2 0 of Brazilian cars are able to use 100 ethanol as fuel which includes ethanol only engines and flex fuel engines 60 Flex fuel engines in Brazil are able to work with all ethanol all gasoline or any mixture of both In the United States flex fuel vehicles can run on 0 to 85 ethanol 15 gasoline since higher ethanol blends are not yet allowed or efficient Brazil supports this fleet of ethanol burning automobiles with large national infrastructure that produces ethanol from domestically grown sugarcane Ethanol s high miscibility with water makes it unsuitable for shipping through modern pipelines like liquid hydrocarbons 61 Mechanics have seen increased cases of damage to small engines in particular the carburetor and attribute the damage to the increased water retention by ethanol in fuel 62 nbsp Ethanol pump station in Sao Paulo Brazil nbsp A Ford Taurus fueled by ethanol in New York City nbsp U S Postal Service truck running on E85 in Minnesota Rocket fuel edit Ethanol was commonly used as fuel in early bipropellant rocket liquid propelled vehicles in conjunction with an oxidizer such as liquid oxygen The German A 4 ballistic rocket of World War II better known by its propaganda name V 2 63 which is credited as having begun the space age used ethanol as the main constituent of B Stoff Under such nomenclature the ethanol was mixed with 25 water to reduce the combustion chamber temperature 64 65 The V 2 s design team helped develop U S rockets following World War II including the ethanol fueled Redstone rocket which launched the first U S satellite 66 Alcohols fell into general disuse as more energy dense rocket fuels were developed 65 although ethanol is currently used in lightweight rocket powered racing aircraft 67 Fuel cells edit Commercial fuel cells operate on reformed natural gas hydrogen or methanol Ethanol is an attractive alternative due to its wide availability low cost high purity and low toxicity There is a wide range of fuel cell concepts that have entered trials including direct ethanol fuel cells auto thermal reforming systems and thermally integrated systems The majority of work is being conducted at a research level although there are a number of organizations at the beginning of the commercialization of ethanol fuel cells 68 Household heating and cooking edit Ethanol fireplaces can be used for home heating or for decoration Ethanol can also be used as stove fuel for cooking 69 70 Feedstock edit Further information Reactions Ethanol is an important industrial ingredient It has widespread use as a precursor for other organic compounds such as ethyl halides ethyl esters diethyl ether acetic acid and ethyl amines Solvent edit Ethanol is considered a universal solvent as its molecular structure allows for the dissolving of both polar hydrophilic and nonpolar hydrophobic compounds As ethanol also has a low boiling point it is easy to remove from a solution that has been used to dissolve other compounds making it a popular extracting agent for botanical oils Cannabis oil extraction methods often use ethanol as an extraction solvent 71 and also as a post processing solvent to remove oils waxes and chlorophyll from solution in a process known as winterization Ethanol is found in paints tinctures markers and personal care products such as mouthwashes perfumes and deodorants Polysaccharides precipitate from aqueous solution in the presence of alcohol and ethanol precipitation is used for this reason in the purification of DNA and RNA Low temperature liquid edit Because of its low freezing point of 114 C 173 F and low toxicity ethanol is sometimes used in laboratories with dry ice or other coolants as a cooling bath to keep vessels at temperatures below the freezing point of water For the same reason it is also used as the active fluid in alcohol thermometers Chemistry editFurther information Ethanol data page Chemical formula edit Ethanol is a 2 carbon alcohol Its molecular formula is CH3CH2OH The structure of the molecule of ethanol is CH3 CH2 OH an ethyl group linked to a hydroxyl group which indicates that the carbon of a methyl group CH3 is attached to the carbon of a methylene group CH2 which is attached to the oxygen of a hydroxyl group OH It is a constitutional isomer of dimethyl ether Ethanol is sometimes abbreviated as EtOH using the common organic chemistry notation of representing the ethyl group C2H5 with Et Physical properties edit nbsp Ethanol burning with its spectrum depictedEthanol is a volatile colorless liquid that has a slight odor It burns with a smokeless blue flame that is not always visible in normal light The physical properties of ethanol stem primarily from the presence of its hydroxyl group and the shortness of its carbon chain Ethanol s hydroxyl group is able to participate in hydrogen bonding rendering it more viscous and less volatile than less polar organic compounds of similar molecular weight such as propane Ethanol s adiabatic flame temperature for combustion in air is 2082 C or 3779 F 72 Ethanol is slightly more refractive than water having a refractive index of 1 36242 at l 589 3 nm and 18 35 C or 65 03 F 73 The triple point for ethanol is 150 20 K 74 Solvent properties edit Ethanol is a versatile solvent miscible with water and with many organic solvents including acetic acid acetone benzene carbon tetrachloride chloroform diethyl ether ethylene glycol glycerol nitromethane pyridine and toluene Its main use as a solvent is in making tincture of iodine cough syrups etc 73 75 It is also miscible with light aliphatic hydrocarbons such as pentane and hexane and with aliphatic chlorides such as trichloroethane and tetrachloroethylene 75 Ethanol s miscibility with water contrasts with the immiscibility of longer chain alcohols five or more carbon atoms whose water miscibility decreases sharply as the number of carbons increases 76 The miscibility of ethanol with alkanes is limited to alkanes up to undecane mixtures with dodecane and higher alkanes show a miscibility gap below a certain temperature about 13 C for dodecane 77 The miscibility gap tends to get wider with higher alkanes and the temperature for complete miscibility increases Ethanol water mixtures have less volume than the sum of their individual components at the given fractions Mixing equal volumes of ethanol and water results in only 1 92 volumes of mixture 73 78 Mixing ethanol and water is exothermic with up to 777 J mol 79 being released at 298 K Mixtures of ethanol and water form an azeotrope at about 89 mole ethanol and 11 mole water 80 or a mixture of 95 6 ethanol by mass or about 97 alcohol by volume at normal pressure which boils at 351 K 78 C This azeotropic composition is strongly temperature and pressure dependent and vanishes at temperatures below 303 K 81 nbsp Hydrogen bonding in solid ethanol at 186 CHydrogen bonding causes pure ethanol to be hygroscopic to the extent that it readily absorbs water from the air The polar nature of the hydroxyl group causes ethanol to dissolve many ionic compounds notably sodium and potassium hydroxides magnesium chloride calcium chloride ammonium chloride ammonium bromide and sodium bromide 75 Sodium and potassium chlorides are slightly soluble in ethanol 75 Because the ethanol molecule also has a nonpolar end it will also dissolve nonpolar substances including most essential oils 82 and numerous flavoring coloring and medicinal agents The addition of even a few percent of ethanol to water sharply reduces the surface tension of water This property partially explains the tears of wine phenomenon When wine is swirled in a glass ethanol evaporates quickly from the thin film of wine on the wall of the glass As the wine s ethanol content decreases its surface tension increases and the thin film beads up and runs down the glass in channels rather than as a smooth sheet Flammability edit An ethanol water solution will catch fire if heated above a temperature called its flash point and an ignition source is then applied to it 83 For 20 alcohol by mass about 25 by volume this will occur at about 25 C 77 F The flash point of pure ethanol is 13 C 55 F 84 but may be influenced very slightly by atmospheric composition such as pressure and humidity Ethanol mixtures can ignite below average room temperature Ethanol is considered a flammable liquid Class 3 Hazardous Material in concentrations above 2 35 by mass 3 0 by volume 6 proof 85 86 87 Flash points of ethanol water mixtures 88 86 89 Ethanol mass fraction Temperature C F1 84 5 184 1 86 2 64 147 86 2 35 60 140 86 85 3 51 5 124 7 86 5 43 109 88 6 39 5 103 1 86 10 31 88 88 20 25 77 86 30 24 75 88 40 21 9 71 4 citation needed 88 50 20 68 88 86 60 17 9 64 2 citation needed 88 70 16 61 88 80 15 8 60 4 86 90 14 57 88 100 12 5 54 5 88 86 84 Dishes using burning alcohol for culinary effects are called flambe Natural occurrence editEthanol is a byproduct of the metabolic process of yeast As such ethanol will be present in any yeast habitat Ethanol can commonly be found in overripe fruit 90 Ethanol produced by symbiotic yeast can be found in bertam palm blossoms Although some animal species such as the pentailed treeshrew exhibit ethanol seeking behaviors most show no interest or avoidance of food sources containing ethanol 91 Ethanol is also produced during the germination of many plants as a result of natural anaerobiosis 92 Ethanol has been detected in outer space forming an icy coating around dust grains in interstellar clouds 93 Minute quantity amounts average 196 ppb of endogenous ethanol and acetaldehyde were found in the exhaled breath of healthy volunteers 94 Auto brewery syndrome also known as gut fermentation syndrome is a rare medical condition in which intoxicating quantities of ethanol are produced through endogenous fermentation within the digestive system 95 Production edit nbsp 94 denatured ethanol sold in a bottle for household useEthanol is produced both as a petrochemical through the hydration of ethylene and via biological processes by fermenting sugars with yeast 96 Which process is more economical depends on prevailing prices of petroleum and grain feed stocks Sources edit World production of ethanol in 2006 was 51 gigalitres 1 3 1010 US gal with 69 of the world supply coming from Brazil and the U S 17 Brazilian ethanol is produced from sugarcane which has relatively high yields 830 more fuel than the fossil fuels used to produce it compared to some other energy crops 97 Sugarcane not only has a greater concentration of sucrose than corn by about 30 but is also much easier to extract The bagasse generated by the process is not discarded but burned by power plants to produce electricity Bagasse burning accounts for around 9 of the electricity produced in Brazil 98 In the 1970s most industrial ethanol in the U S was made as a petrochemical but in the 1980s the U S introduced subsidies for corn based ethanol 99 According to the Renewable Fuels Association as of 30 October 2007 131 grain ethanol bio refineries in the U S have the capacity to produce 7 10 9 US gal 26 000 000 m3 of ethanol per year An additional 72 construction projects underway in the U S can add 6 4 billion US gallons 24 000 000 m3 of new capacity in the next 18 months 49 In India ethanol is made from sugarcane 100 Sweet sorghum is another potential source of ethanol and is suitable for growing in dryland conditions The International Crops Research Institute for the Semi Arid Tropics is investigating the possibility of growing sorghum as a source of fuel food and animal feed in arid parts of Asia and Africa 101 Sweet sorghum has one third the water requirement of sugarcane over the same time period It also requires about 22 less water than corn The world s first sweet sorghum ethanol distillery began commercial production in 2007 in Andhra Pradesh India 102 Hydration edit Ethanol can be produced from petrochemical feed stocks primarily by the acid catalyzed hydration of ethylene It is often referred to as synthetic ethanol C2 H4 H2 O CH3 CH2 OH The catalyst is most commonly phosphoric acid 103 104 adsorbed onto a porous support such as silica gel or diatomaceous earth This catalyst was first used for large scale ethanol production by the Shell Oil Company in 1947 105 The reaction is carried out in the presence of high pressure steam at 300 C 572 F where a 5 3 ethylene to steam ratio is maintained 106 107 This process was used on an industrial scale by Union Carbide Corporation and others It is no longer practiced in the US as fermentation ethanol produced from corn is more economical 108 In an older process first practiced on the industrial scale in 1930 by Union Carbide 109 but now almost entirely obsolete ethylene was hydrated indirectly by reacting it with concentrated sulfuric acid to produce ethyl sulfate which was hydrolyzed to yield ethanol and regenerate the sulfuric acid 110 C2 H4 H2 SO4 CH3 CH2 SO4 H CH3 C H2 SO4 H H2 O CH3 C H2 O H H2 SO4 From carbon dioxide edit Ethanol has been produced in the laboratory by converting carbon dioxide via biological and electrochemical reactions 111 112 CO2 H2 O CH3 CH2 O H side products Fermentation edit Main article Ethanol fermentation See also Yeast in winemaking Ethanol in alcoholic beverages and fuel is produced by fermentation Certain species of yeast e g Saccharomyces cerevisiae metabolize sugar namely polysaccharides producing ethanol and carbon dioxide The chemical equations below summarize the conversion C6 H12 O6 2 CH3 CH2 O H 2 CO2 C12 H22 O11 H2 O 4 CH3 CH2 O H 4 CO2 Fermentation is the process of culturing yeast under favorable thermal conditions to produce alcohol This process is carried out at around 35 40 C 95 104 F Toxicity of ethanol to yeast limits the ethanol concentration obtainable by brewing higher concentrations therefore are obtained by fortification or distillation The most ethanol tolerant yeast strains can survive up to approximately 18 ethanol by volume To produce ethanol from starchy materials such as cereals the starch must first be converted into sugars In brewing beer this has traditionally been accomplished by allowing the grain to germinate or malt which produces the enzyme amylase When the malted grain is mashed the amylase converts the remaining starches into sugars Cellulose edit Main article Cellulosic ethanol Sugars for ethanol fermentation can be obtained from cellulose Deployment of this technology could turn a number of cellulose containing agricultural by products such as corncobs straw and sawdust into renewable energy resources Other agricultural residues such as sugarcane bagasse and energy crops such as switchgrass may also be fermentable sugar sources 113 Testing edit nbsp Infrared reflection spectra of liquid ethanol showing the OH band centered near 3300 cm 1 and C H bands near 2950 cm 1 nbsp Near infrared spectrum of liquid ethanolBreweries and biofuel plants employ two methods for measuring ethanol concentration Infrared ethanol sensors measure the vibrational frequency of dissolved ethanol using the C H band at 2900 cm 1 This method uses a relatively inexpensive solid state sensor that compares the C H band with a reference band to calculate the ethanol content The calculation makes use of the Beer Lambert law Alternatively by measuring the density of the starting material and the density of the product using a hydrometer the change in specific gravity during fermentation indicates the alcohol content This inexpensive and indirect method has a long history in the beer brewing industry Purification editDistillation edit Ethylene hydration or brewing produces an ethanol water mixture For most industrial and fuel uses the ethanol must be purified Fractional distillation at atmospheric pressure can concentrate ethanol to 95 6 by weight 89 5 mole This mixture is an azeotrope with a boiling point of 78 1 C 172 6 F and cannot be further purified by distillation Addition of an entraining agent such as benzene cyclohexane or heptane allows a new ternary azeotrope comprising the ethanol water and the entraining agent to be formed This lower boiling ternary azeotrope is removed preferentially leading to water free ethanol 104 Molecular sieves and desiccants edit Apart from distillation ethanol may be dried by addition of a desiccant such as molecular sieves cellulose or cornmeal The desiccants can be dried and reused 104 Molecular sieves can be used to selectively absorb the water from the 95 6 ethanol solution 114 Molecular sieves of pore size 3 Angstrom a type of zeolite effectively sequester water molecules while excluding ethanol molecules Heating the wet sieves drives out the water allowing regeneration of their desiccant capability 115 Membranes and reverse osmosis edit Membranes can also be used to separate ethanol and water Membrane based separations are not subject to the limitations of the water ethanol azeotrope because the separations are not based on vapor liquid equilibria Membranes are often used in the so called hybrid membrane distillation process This process uses a pre concentration distillation column as the first separating step The further separation is then accomplished with a membrane operated either in vapor permeation or pervaporation mode Vapor permeation uses a vapor membrane feed and pervaporation uses a liquid membrane feed Other techniques edit A variety of other techniques have been discussed including the following 104 Salting using potassium carbonate to exploit its insolubility will cause a phase separation with ethanol and water This offers a very small potassium carbonate impurity to the alcohol that can be removed by distillation This method is very useful in purification of ethanol by distillation as ethanol forms an azeotrope with water Direct electrochemical reduction of carbon dioxide to ethanol under ambient conditions using copper nanoparticles on a carbon nanospike film as the catalyst 116 Extraction of ethanol from grain mash by supercritical carbon dioxide Pervaporation Fractional freezing is also used to concentrate fermented alcoholic solutions such as traditionally made Applejack beverage Pressure swing adsorption 117 Grades of ethanol edit Denatured alcohol edit Main article Denatured alcohol Pure ethanol and alcoholic beverages are heavily taxed as psychoactive drugs but ethanol has many uses that do not involve its consumption To relieve the tax burden on these uses most jurisdictions waive the tax when an agent has been added to the ethanol to render it unfit to drink These include bittering agents such as denatonium benzoate and toxins such as methanol naphtha and pyridine Products of this kind are called denatured alcohol 118 119 Absolute alcohol edit Absolute or anhydrous alcohol refers to ethanol with a low water content There are various grades with maximum water contents ranging from 1 to a few parts per million ppm If azeotropic distillation is used to remove water it will contain trace amounts of the material separation agent e g benzene 120 Absolute alcohol is not intended for human consumption Absolute ethanol is used as a solvent for laboratory and industrial applications where water will react with other chemicals and as fuel alcohol Spectroscopic ethanol is an absolute ethanol with a low absorbance in ultraviolet and visible light fit for use as a solvent in ultraviolet visible spectroscopy 121 Pure ethanol is classed as 200 proof in the US equivalent to 175 degrees proof in the UK system 122 Rectified spirits edit Rectified spirit an azeotropic composition of 96 ethanol containing 4 water is used instead of anhydrous ethanol for various purposes Spirits of wine are about 94 ethanol 188 proof The impurities are different from those in 95 190 proof laboratory ethanol 123 Reactions editFurther information Alcohol chemistry Ethanol is classified as a primary alcohol meaning that the carbon that its hydroxyl group attaches to has at least two hydrogen atoms attached to it as well Many ethanol reactions occur at its hydroxyl group Ester formation edit In the presence of acid catalysts ethanol reacts with carboxylic acids to produce ethyl esters and water RCOOH HOCH2CH3 RCOOCH2CH3 H2OThis reaction which is conducted on large scale industrially requires the removal of the water from the reaction mixture as it is formed Esters react in the presence of an acid or base to give back the alcohol and a salt This reaction is known as saponification because it is used in the preparation of soap Ethanol can also form esters with inorganic acids Diethyl sulfate and triethyl phosphate are prepared by treating ethanol with sulfur trioxide and phosphorus pentoxide respectively Diethyl sulfate is a useful ethylating agent in organic synthesis Ethyl nitrite prepared from the reaction of ethanol with sodium nitrite and sulfuric acid was formerly used as a diuretic Dehydration edit In the presence of acid catalysts alcohols can be converted to alkenes such as ethanol to ethylene Typically solid acids such as alumina are used 124 CH3CH2OH H2C CH2 H2OSince water is removed from the same molecule the reaction is known as intramolecular dehydration Intramolecular dehydration of an alcohol requires a high temperature and the presence of an acid catalyst such as sulfuric acid 125 Ethylene produced from sugar derived ethanol primarily in Brazil competes with ethylene produced from petrochemical feedstocks such as naphtha and ethane At a lower temperature than that of intramolecular dehydration intermolecular alcohol dehydration may occur producing a symmetrical ether This is a condensation reaction In the following example diethyl ether is produced from ethanol 2 CH3CH2OH CH3CH2OCH2CH3 H2O 126 Combustion edit Complete combustion of ethanol forms carbon dioxide and water C2H5OH l 3 O2 g 2 CO2 g 3 H2O l DHc 1371 kJ mol 127 29 8 kJ g 327 kcal mol 7 1 kcal gC2H5OH l 3 O2 g 2 CO2 g 3 H2O g DHc 1236 kJ mol 26 8 kJ g 295 4 kcal mol 6 41 kcal g 128 Specific heat 2 44 kJ kg K Acid base chemistry edit Ethanol is a neutral molecule and the pH of a solution of ethanol in water is nearly 7 00 Ethanol can be quantitatively converted to its conjugate base the ethoxide ion CH3CH2O by reaction with an alkali metal such as sodium 76 2 CH3CH2OH 2 Na 2 CH3CH2ONa H2or a very strong base such as sodium hydride CH3CH2OH NaH CH3CH2ONa H2The acidities of water and ethanol are nearly the same as indicated by their pKa of 15 7 and 16 respectively Thus sodium ethoxide and sodium hydroxide exist in an equilibrium that is closely balanced CH3CH2OH NaOH CH3CH2ONa H2OHalogenation edit Ethanol is not used industrially as a precursor to ethyl halides but the reactions are illustrative Ethanol reacts with hydrogen halides to produce ethyl halides such as ethyl chloride and ethyl bromide via an SN2 reaction CH3CH2OH HCl CH3CH2Cl H2OHCl requires a catalyst such as zinc chloride 110 HBr requires refluxing with a sulfuric acid catalyst 110 Ethyl halides can in principle also be produced by treating ethanol with more specialized halogenating agents such as thionyl chloride or phosphorus tribromide 76 110 CH3CH2OH SOCl2 CH3CH2Cl SO2 HClUpon treatment with halogens in the presence of base ethanol gives the corresponding haloform CHX3 where X Cl Br I This conversion is called the haloform reaction 129 An intermediate in the reaction with chlorine is the aldehyde called chloral which forms chloral hydrate upon reaction with water 130 4 Cl2 CH3CH2OH CCl3CHO 5 HCl CCl3CHO H2O CCl3C OH 2HOxidation edit Ethanol can be oxidized to acetaldehyde and further oxidized to acetic acid depending on the reagents and conditions 110 This oxidation is of no importance industrially but in the human body these oxidation reactions are catalyzed by the enzyme liver alcohol dehydrogenase The oxidation product of ethanol acetic acid is a nutrient for humans being a precursor to acetyl CoA where the acetyl group can be spent as energy or used for biosynthesis Metabolism edit Ethanol is similar to macronutrients such as proteins fats and carbohydrates in that it provides calories When consumed and metabolized it contributes 7 kilocalories per gram via ethanol metabolism 131 Safety editSee also Alcohol chemistry Toxicity Ethanol is very flammable and should not be used around an open flame Pure ethanol will irritate the skin and eyes 132 Nausea vomiting and intoxication are symptoms of ingestion Long term use by ingestion can result in serious liver damage 133 Atmospheric concentrations above one part per thousand are above the European Union occupational exposure limits 133 History editFurther information Liquor The fermentation of sugar into ethanol is one of the earliest biotechnologies employed by humans Ethanol has historically been identified variously as spirit of wine or ardent spirits 134 and as aqua vitae or aqua vita The intoxicating effects of its consumption have been known since ancient times Ethanol has been used by humans since prehistory as the intoxicating ingredient of alcoholic beverages Dried residue on 9 000 year old pottery found in China suggests that Neolithic people consumed alcoholic beverages 135 The inflammable nature of the exhalations of wine was already known to ancient natural philosophers such as Aristotle 384 322 BCE Theophrastus c 371 287 BCE and Pliny the Elder 23 24 79 CE 136 However this did not immediately lead to the isolation of ethanol even despite the development of more advanced distillation techniques in second and third century Roman Egypt 137 An important recognition first found in one of the writings attributed to Jabir ibn Ḥayyan ninth century CE was that by adding salt to boiling wine which increases the wine s relative volatility the flammability of the resulting vapors may be enhanced 138 The distillation of wine is attested in Arabic works attributed to al Kindi c 801 873 CE and to al Farabi c 872 950 and in the 28th book of al Zahrawi s Latin Abulcasis 936 1013 Kitab al Taṣrif later translated into Latin as Liber servatoris 139 In the twelfth century recipes for the production of aqua ardens burning water i e ethanol by distilling wine with salt started to appear in a number of Latin works and by the end of the thirteenth century it had become a widely known substance among Western European chemists 140 The works of Taddeo Alderotti 1223 1296 describe a method for concentrating ethanol involving repeated fractional distillation through a water cooled still by which an ethanol purity of 90 could be obtained 141 The medicinal properties of ethanol were studied by Arnald of Villanova 1240 1311 CE and John of Rupescissa c 1310 1366 the latter of whom regarded it as a life preserving substance able to prevent all diseases the aqua vitae or water of life also called by John the quintessence of wine 142 In China archaeological evidence indicates that the true distillation of alcohol began during the Jin 1115 1234 or Southern Song 1127 1279 dynasties 143 A still has been found at an archaeological site in Qinglong Hebei dating to the 12th century 143 In India the true distillation of alcohol was introduced from the Middle East and was in wide use in the Delhi Sultanate by the 14th century 144 In 1796 German Russian chemist Johann Tobias Lowitz obtained pure ethanol by mixing partially purified ethanol the alcohol water azeotrope with an excess of anhydrous alkali and then distilling the mixture over low heat 145 French chemist Antoine Lavoisier described ethanol as a compound of carbon hydrogen and oxygen and in 1807 Nicolas Theodore de Saussure determined ethanol s chemical formula 146 147 Fifty years later Archibald Scott Couper published the structural formula of ethanol It was one of the first structural formulas determined 148 Ethanol was first prepared synthetically in 1825 by Michael Faraday He found that sulfuric acid could absorb large volumes of coal gas 149 He gave the resulting solution to Henry Hennell a British chemist who found in 1826 that it contained sulphovinic acid ethyl hydrogen sulfate 150 In 1828 Hennell and the French chemist Georges Simon Serullas independently discovered that sulphovinic acid could be decomposed into ethanol 151 152 Thus in 1825 Faraday had unwittingly discovered that ethanol could be produced from ethylene a component of coal gas by acid catalyzed hydration a process similar to current industrial ethanol synthesis 153 Ethanol was used as lamp fuel in the U S as early as 1840 but a tax levied on industrial alcohol during the Civil War made this use uneconomical The tax was repealed in 1906 154 Use as an automotive fuel dates back to 1908 with the Ford Model T able to run on petrol gasoline or ethanol 155 It fuels some spirit lamps Ethanol intended for industrial use is often produced from ethylene 156 Ethanol has widespread use as a solvent of substances intended for human contact or consumption including scents flavorings colorings and medicines In chemistry it is both a solvent and a feedstock for the synthesis of other products It has a long history as a fuel for heat and light and more recently as a fuel for internal combustion engines See also editEthanol induced non lamellar phases in phospholipids Methanol 1 Propanol 2 Propanol Rubbing alcohol tert Butyl alcohol Butanol fuel Timeline of alcohol fuelReferences edit Nomenclature of Organic Chemistry IUPAC Recommendations and 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original on 14 July 2011 Retrieved 3 January 2011 Ottley William Campbell 1826 A dictionary of chemistry and of mineralogy as connected with it Murray Roach J 18 July 2005 9 000 Year Old Beer Re Created From Chinese Recipe National Geographic News Archived from the original on 22 July 2005 Retrieved 3 September 2007 Berthelot amp Houdas 1893 vol I p 137 Berthelot amp Houdas 1893 vol I pp 138 139 al Hassan Ahmad Y 2009 Alcohol and the Distillation of Wine in Arabic Sources from the 8th Century Studies in al Kimya Critical Issues in Latin and Arabic Alchemy and Chemistry Hildesheim Georg Olms Verlag pp 283 298 same content also available on the author s website Archived 29 December 2015 at the Wayback Machine al Hassan 2009 same content also available on the author s website Archived 29 December 2015 at the Wayback Machine cf Berthelot amp Houdas 1893 vol I pp 141 143 Sometimes sulfur was also added to the wine see Berthelot amp Houdas 1893 vol I p 143 Multhauf 1966 pp 204 206 Holmyard Eric John 1957 Alchemy Harmondsworth Penguin Books ISBN 978 0 486 26298 7 pp 51 52 Principe Lawrence M 2013 The Secrets of Alchemy Chicago The University of Chicago Press ISBN 978 0 226 10379 2 pp 69 71 a b Haw SG 2006 Wine women and poison Marco Polo in China Routledge pp 147 148 ISBN 978 1 134 27542 7 Retrieved 10 July 2016 The earliest possible period seems to be the Eastern Han dynasty the most likely period for the beginning of true distillation of spirits for drinking in China is during the Jin and Southern Song dynasties Habib Irfan 2011 Economic History of Medieval India 1200 1500 Pearson Education India pp 55 ISBN 978 81 317 2791 1 Lowitz T 1796 Anzeige eines zur volkommen Entwasserung des Weingeistes nothwendig zu beobachtenden Handgriffs Report of a task that must be done for the complete dehydration of wine spirits i e alcohol water azeotrope Chemische Annalen fur die Freunde der Naturlehre Aerznengelartheit Haushaltungskunde und Manufakturen in German 1 195 204 See pp 197 198 Lowitz dehydrated the azeotrope by mixing it with a 2 1 excess of anhydrous alkali and then distilling the mixture over low heat Chisholm Hugh ed 1911 Alcohol Encyclopaedia Britannica Vol 1 11th ed Cambridge University Press pp 525 527 de Saussure T 1807 Memoire sur la composition de l alcohol et de l ether sulfurique Journal de Physique de Chimie d Histoire Naturelle et des Arts 64 316 354 In his 1807 paper Saussure determined ethanol s composition only roughly a more accurate analysis of ethanol appears on page 300 of his 1814 paper de Saussure Theodore 1814 Nouvelles observations sur la composition de l alcool et de l ether sulfurique Annales de Chimie et de Physique 89 273 305 Couper AS 1858 On a new chemical theory online reprint Philosophical Magazine 16 104 116 Retrieved 3 September 2007 Faraday M 1825 On new compounds of carbon and hydrogen and on certain other products obtained during the decomposition of oil by heat Philosophical Transactions of the Royal Society of London 115 440 466 doi 10 1098 rstl 1825 0022 In a footnote on page 448 Faraday notes the action of sulfuric acid on coal gas and coal gas distillate specifically The sulfuric acid combines directly with carbon and hydrogen and I find when the resulting compound is united with bases it forms a peculiar class of salts somewhat resembling the sulphovinates i e ethyl sulfates but still different from them Hennell H 1826 On the mutual action of sulphuric acid and alcohol with observations on the composition and properties of the resulting compound Philosophical Transactions of the Royal Society of London 116 240 249 doi 10 1098 rstl 1826 0021 S2CID 98278290 On page 248 Hennell mentions that Faraday gave him some sulfuric acid in which coal gas had dissolved and that he Hennell found that it contained sulphovinic acid ethyl hydrogen sulfate Hennell H 1828 On the mutual action of sulfuric acid and alcohol and on the nature of the process by which ether is formed Philosophical Transactions of the Royal Society of London 118 365 371 doi 10 1098 rstl 1828 0021 S2CID 98483646 On page 368 Hennell produces ethanol from sulfovinic acid ethyl hydrogen sulfate Serullas G 1828 Guyton de Morveau L Gay Lussac JL Arago F Michel Eugene Chevreul Marcellin Berthelot Eleuthere Elie Nicolas Mascart Albin Haller eds De l action de l acide sulfurique sur l alcool et des produits qui en resultent Annales de Chimie et de Physique 39 152 186 On page 158 Serullas mentions the production of alcohol from sulfate acid d hydrogene carbone hydrocarbon acid sulfate In 1855 the French chemist Marcellin Berthelot confirmed Faraday s discovery by preparing ethanol from pure ethylene Berthelot M 1855 Arago F Gay Lussac JL eds Sur la formation de l alcool au moyen du bicarbure d hydrogene On the formation of alcohol by means of ethylene Annales de Chimie et de Physique 43 385 405 Note The chemical formulas in Berthelot s paper are wrong because chemists at that time used the wrong atomic masses for the elements e g carbon 6 instead of 12 oxygen 8 instead of 16 etc Siegel R 15 February 2007 Ethanol Once Bypassed Now Surging Ahead NPR Retrieved 22 September 2007 DiPardo J Outlook for Biomass Ethanol Production and Demand PDF United States Department of Energy Archived from the original PDF on 24 September 2015 Retrieved 22 September 2007 Myers RL Myers RL 2007 The 100 most important chemical compounds a reference guide Westport CN Greenwood Press p 122 ISBN 978 0 313 33758 1 Further reading editBoyce JM Pittet D 2003 Hand Hygiene in Healthcare Settings Atlanta GA Centers for Disease Control Onuki S Koziel JA van Leeuwen J Jenks WS Grewell D Cai L June 2008 Ethanol production purification and analysis techniques a review 2008 ASABE Annual International Meeting Providence RI Retrieved 16 February 2013 Explanation of US denatured alcohol designations Sci toys Lange Norbert Adolph 1967 John Aurie Dean ed Lange s Handbook of Chemistry 10th ed McGraw Hill External links edit nbsp Look up alcohol or ethanol in Wiktionary the free dictionary nbsp Wikimedia Commons has media related to Ethanol Alcohol Ethanol at The Periodic Table of Videos University of Nottingham International Labour Organization ethanol safety information National Pollutant Inventory Ethanol Fact Sheet CDC NIOSH Pocket Guide to Chemical Hazards Ethyl Alcohol National Institute of Standards and Technology chemical data on ethanol Chicago Board of Trade news and market data on ethanol futures Calculation of vapor pressure liquid density dynamic liquid viscosity surface tension of ethanol Ethanol History A look into the history of ethanol ChemSub Online Ethyl alcohol Industrial ethanol production process flow diagram using ethylene and sulphuric acid Retrieved from https en wikipedia org w index php title Ethanol amp oldid 1191649035, wikipedia, wiki, book, books, library,

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