The Info List - Ethanol

--- Advertisement ---

Ethanol, also called alcohol, ethyl alcohol, and drinking alcohol, is a chemical compound, a simple alcohol with the chemical formula C 2H 5OH. Its formula can be written also as CH 3−CH 2−OH or C 2H 5−OH (an ethyl group linked to a hydroxyl group), and is often abbreviated as EtOH. Ethanol
is a volatile, flammable, colorless liquid with a slight characteristic odor. It is a psychoactive substance and is the principal type of alcohol found in alcoholic drinks. Ethanol
is naturally produced by the fermentation of sugars by yeasts or via petrochemical processes, and is most commonly consumed as a popular recreational drug. It also has medical applications as an antiseptic and disinfectant. The compound is widely used as a chemical solvent, either for scientific chemical testing or in synthesis of other organic compounds, and is a vital substance utilized across many different kinds of manufacturing industries. Ethanol
is also used as a clean-burning fuel source.


1 Etymology 2 Uses

2.1 Medical

2.1.1 Antiseptic 2.1.2 Antidote 2.1.3 Medicinal solvent 2.1.4 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

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 Ethylene
hydration 5.2 From CO2 5.3 From lipids 5.4 Fermentation

5.4.1 Cellulose

5.5 Testing

6 Purification

6.1 Distillation 6.2 Molecular sieves
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

8 Safety 9 History 10 See also 11 References 12 Further reading 13 External links

Etymology[edit] Ethanol
is the systematic name defined by the International Union of Pure and Applied Chemistry
(IUPAC) for a compound consisting of alkyl group with two carbon atoms (prefix “eth-”), having a single bond between them (infix “-an-”), attached functional group −OH group (suffix “-ol”).[1] The “eth-” prefix and the qualifier “ethyl” in “ethyl alcohol” originally come 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”).[7] According to the Oxford English Dictionary, Ethyl is a contraction of the Ancient Greek αἰθήρ (aithḗr, “upper air”) and the Greek word ὕλη (hýlē, “substance”).[8] The name ethanol was coined as a result of a resolution that was adopted at the International Conference on Chemical Nomenclature that was held in April 1892 in Geneva, Switzerland.[9] The term “alcohol” now refers to a wider class of substances in chemistry nomenclature, but in common parlance it remains the name of ethanol. The Oxford English Dictionary
Oxford English Dictionary
claims that 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.[10] The use of “alcohol” for ethanol (in full, “alcohol of wine”) is modern, first recorded 1753, and by the later 17th century referred to “any sublimated substance; distilled spirit” use for “the spirit of wine” (shortened from a full expression alcohol of wine). The systematic use in chemistry dates to 1850. Uses[edit] Main article: Short-term uses and function of alcohol Medical[edit] Main article: Alcohol
(medicine) Antiseptic[edit] Ethanol
is used in medical wipes and most common antibacterial hand sanitizer gels as an antiseptic. Ethanol
kills organisms by denaturing their proteins and dissolving their lipids and is effective against most bacteria and fungi, and many viruses. However, ethanol is ineffective against bacterial spores.[11] 70% ethanol is the most effective concentration, particularly because of osmotic pressure. Absolute ethanol may inactivate microbes without destroying them because the alcohol is unable to fully permeate the microbe's membrane.[12][13] Antidote[edit] Ethanol
may be administered as an antidote to methanol[14] and ethylene glycol poisoning.[15] Medicinal solvent[edit] Ethanol, often in high concentrations, is used to dissolve many water-insoluble medications and related compounds. Liquid preparations of cough and cold remedies, pain medication, and mouth washes may be dissolved in 1 to 25% concentrations of ethanol and may need to be avoided in individuals with adverse reactions to ethanol such as alcohol-induced respiratory reactions.[16] 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.[17] Pharmacology[edit] Ethyl Alcohol
is extensively metabolized by the liver, particularly via the enzyme CYP450.[18] Ethyl Alcohol
increases the secretion of acids in the stomach.[18] The metabolite acetaldehyde is responsible for much of the short term, and long term effects of ethyl alcohol toxicity.[19] Recreational[edit] Main articles: Alcohol (drug)
Alcohol (drug)
and Alcoholic drink As a central nervous system depressant, ethanol is one of the most commonly consumed psychoactive drugs.[20] It can lift mood, cause feelings of euphoria, decrease anxiety, and increase sociability and talkativeness.[citation needed] Fuel[edit] Engine fuel[edit] Main article: Ethanol

Energy content of some fuels compared with ethanol:[21]

type MJ/L MJ/kg Research octane number

Dry wood (20% moisture)


Methanol 17.9 19.9 108.7[22]

Ethanol 21.2[23] 26.8[23] 108.6[22]

E85 (85% ethanol, 15% gasoline) 25.2 33.2 105

Liquefied natural gas 25.3 ~55

(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[24] 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 the globe's leading producer of ethanol.[25] 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. Brazilian ethanol is produced from sugar cane and noted for high carbon sequestration.[26] The US and many other countries primarily use E10 (10% ethanol, sometimes known as gasohol) and E85
(85% ethanol) ethanol/gasoline mixtures.

USP grade ethanol for laboratory use.

has been used as rocket fuel and is currently in lightweight rocket-powered racing aircraft.[27] 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.[28] 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.[29] 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.[30] 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.[31] This leads to a significantly larger photochemical reactivity and more ground level ozone.[32] These data have been assembled into The Clean Fuels Report comparison of fuel emissions[33] and show that ethanol exhaust generates 2.14 times as much ozone as gasoline exhaust.[34] When this is added into the custom Localised Pollution Index (LPI) 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.[35] The California Air Resources Board
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).[36] 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 United States.[37] More than 20% of Brazilian cars are able to use 100% ethanol as fuel, which includes ethanol-only engines and flex-fuel engines.[38] Flex-fuel engines in Brazil
are able to work with all ethanol, all gasoline or any mixture of both. In the US 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 population of ethanol-burning automobiles with large national infrastructure that produces ethanol from domestically grown sugar cane. Sugar
cane 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 wasted, but is used in power plants to produce electricity.[citation needed] In the United States, the ethanol fuel industry is based largely on corn. According to the Renewable Fuels Association, as of 30 October 2007, 131 grain ethanol bio-refineries in the United States have the capacity to produce 7.0 billion US gallons (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. 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.[39] Sweet sorghum
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 (ICRISAT) is investigating the possibility of growing sorgham as a source of fuel, food, and animal feed in arid parts of Asia
and Africa.[40] Sweet sorghum
Sweet sorghum
has one-third the water requirement of sugarcane over the same time period. It also requires about 22% less water than corn (also known as maize). The world’s first sweet sorghum ethanol distillery began commercial production in 2007 in Andhra Pradesh, India.[41] Ethanol's high miscibility with water makes it unsuitable for shipping through modern pipelines like liquid hydrocarbons.[42] 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.[43]

pump station in São Paulo, Brazil

A Ford Taurus
Ford Taurus
fueled by ethanol in New York City

USPS truck running on E85
in Minnesota

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 V-2 rocket
V-2 rocket
of World War II, credited with beginning the space age, used ethanol, mixed with 25% of water to reduce the combustion chamber temperature.[44][45] 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.[46] Alcohols fell into general disuse as more efficient rocket fuels were developed.[45] 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 are a wide range of fuel cell concepts that have been trialled 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 commercialization of ethanol fuel cells.[47] Household heating[edit] Ethanol
fireplaces can be used for home heating or for decoration.[48] 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 miscible with water and is a good general purpose solvent. It is found in paints, tinctures, markers, and personal care products such as mouthwashes, perfumes and deodorants. However, 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 melting point (−114.14 °C) 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. An alternative notation is CH3−CH2−OH, 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]

burning with its spectrum depicted

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
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).[49] The triple point for ethanol is 150 K at a pressure of 4.3 × 10−4 Pa.[50] 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.[49][51] It is also miscible with light aliphatic hydrocarbons, such as pentane and hexane, and with aliphatic chlorides such as trichloroethane and tetrachloroethylene.[51] 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.[52] 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[53]). 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.[49][54] Mixing ethanol and water is exothermic, with up to 777 J/mol[55] being released at 298 K. Mixtures of ethanol and water form an azeotrope at about 89 mole-% ethanol and 11 mole-% water[56] or a mixture of 95.6 percent ethanol by mass (or about 97% alcohol by volume) at normal pressure, which boils at 351K (78 °C). This azeotropic composition is strongly temperature- and pressure-dependent and vanishes at temperatures below 303 K.[57]

bonding in solid ethanol at −186 °C

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.[51] Sodium
and potassium chlorides are slightly soluble in ethanol.[51] Because the ethanol molecule also has a nonpolar end, it will also dissolve nonpolar substances, including most essential oils[58] 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 that contains 40% alcohol by weight (about 56% by volume) will catch fire if heated to about 26 °C (79 °F) and if an ignition source is applied to it. This is called its flash point.[59] The flash point of pure ethanol is 16.60 °C (61.88 °F), less than average room temperature.

The flash points of ethanol wt % concentrations[60]

wt % Temperature

10% 49 °C (120 °F)

20% 36 °C (97 °F)

30% 29 °C (84 °F)

40% 26 °C (79 °F)

50% 24 °C (75 °F)

60% 22 °C (72 °F)

70% 21 °C (70 °F)

80% 20 °C (68 °F)

90% 17 °C (63 °F)

96% 17 °C (63 °F)

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.[61] 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.[62] Ethanol
is also produced during the germination of many plants as a result of natural anerobiosis.[63] Ethanol
has been detected in outer space, forming an icy coating around dust grains in interstellar clouds.[64] Minute quantity amounts (average 196 ppb) of endogenous ethanol and acetaldehyde were found in the exhaled breath of healthy volunteers.[65] 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.[66] Production[edit]

94% denatured ethanol sold in a bottle for household use

is produced both as a petrochemical, through the hydration of ethylene and, via biological processes, by fermenting sugars with yeast.[67] Which process is more economical depends on prevailing prices of petroleum and grain feed stocks. In the 1970s most industrial ethanol in the United States was made as a petrochemical, but in the 1980s the United States introduced subsidies for corn based ethanol and today it is almost all made from that source.[68] Ethylene
hydration[edit] Ethanol
for use as an industrial feedstock or solvent (sometimes referred to as synthetic ethanol) is made from petrochemical feed stocks, primarily by the acid-catalyzed hydration of ethylene:

C 2H 4 + H 2O → CH 3CH 2OH

The catalyst is most commonly phosphoric acid,[69][70] 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.[71] 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.[72][73] In the U.S., this process was used on an industrial scale by Union Carbide
Union Carbide
Corporation and others, but now only LyondellBasell
uses it commercially. In an older process, first practiced on the industrial scale in 1930 by Union Carbide,[74] 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:[75]

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

From CO2[edit] CO2 can also be used as the raw material. CO2 can be converted using such organisms as Clostridium ljungdahlii, Clostridium autoethanogenum or Moorella sp. HUC22-1.[76][77] CO2 can be converted using electrochemical reactions at room temperature and pressure.[78][79] From lipids[edit] Lipids can also be used to make ethanol and can be found in such raw materials such as algae.[80] 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, 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

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 cereal grains, 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 sugar cane bagasse and energy crops such as switchgrass may also be a sources of fermentable sugars.[81] Testing[edit]

Infrared reflection spectra of liquid ethanol, showing the -OH band centered at ≈3300 cm−1 and C-H bands at ≈2950 cm−1.

Near infrared spectrum
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 CH band at 2900 cm−1. This method uses a relatively inexpensive solid state sensor that compares the CH 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
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.[70] At pressures less than atmospheric pressure, the composition of the ethanol-water azeotrope shifts to more ethanol-rich mixtures, and at pressures less than 70 torr (9.333 kPa), there is no azeotrope, and it is possible to distill absolute ethanol from an ethanol-water mixture. While vacuum distillation of ethanol is not presently economical, pressure-swing distillation is a topic of current research. In this technique, a reduced-pressure distillation first yields an ethanol-water mixture of more than 95.6% ethanol. Then, fractional distillation of this mixture at atmospheric pressure distills off the 95.6% azeotrope, leaving anhydrous ethanol at the bottom.[citation needed] Molecular sieves
Molecular sieves
and desiccants[edit]

This section needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. (December 2015) (Learn how and when to remove this template message)

Apart from distillation, ethanol may be dried by addition of a desiccant, such as molecular sieves, cellulose, and cornmeal. The desiccants can be dried and reused.[70] Molecular sieves
Molecular sieves
can be used to selectively absorb the water from the 95.6% ethanol solution.[82] Synthetic zeolite in pellet form can be used, as well as a variety of plant-derived absorbents, including cornmeal, straw, and sawdust. The zeolite bed can be regenerated essentially an unlimited number of times by drying it with a blast of hot carbon dioxide. Cornmeal
and other plant-derived absorbents cannot readily be regenerated, but where ethanol is made from grain, they are often available at low cost. Absolute ethanol produced this way has no residual benzene, and can be used to fortify port and sherry in traditional winery operations. 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 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:[70]

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;[83] Extraction of ethanol from grain mash by supercritical carbon dioxide; Pervaporation; Fractional freezing
Fractional freezing
is also used to concentrate fermented alcoholic solutions, such as traditionally made Applejack (beverage); Pressure swing adsorption.[84]

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.[85][86] 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) levels. If azeotropic distillation is used to remove water, it will contain trace amounts of the material separation agent (e.g. benzene).[87] 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.[88] Pure ethanol is classed as 200 proof in the U.S., equivalent to 175 degrees proof in the UK system.[89] Rectified spirits[edit] Rectified spirit, an azeotropic composition of 96% ethanol containing 4% water, is used instead of anhydrous ethanol for various purposes. Wine spirits are about 94% ethanol (188 proof). The impurities are different from those in 95% (190 proof) laboratory ethanol.[90] Reactions[edit] Further information: Alcohol Ethanol
is classified as a primary alcohol, meaning that the carbon 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:


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
Diethyl sulfate
and triethyl phosphate are prepared by treating ethanol with sulfur trioxide and phosphorus pentoxide respectively. Diethyl sulfate
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] Strong acid desiccants cause the partial dehydration of ethanol to form diethyl ether and other byproducts. If the dehydration temperature exceeds around 160 °C (320 °F), full dehydration will occur and ethylene will be the main product.

(ca. 120 °C)    CH3CH2OH → H2C=CH2 + H2O
(above 160 °C)

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[91] = 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[92]

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:[52]

2 CH3CH2OH + 2 Na → 2 CH3CH2ONa + H2

or a very strong base such as sodium hydride:

CH3CH2OH + NaH → CH3CH2ONa + H2

The acidity 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:


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

These reactions require a catalyst such as zinc chloride.[75] HBr requires refluxing with a sulfuric acid catalyst.[75] Ethyl halides can, in principle, also be produced by treating ethanol with more specialized halogenating agents, such as thionyl chloride or phosphorus tribromide.[52][75]

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.[93] " An intermediate in the reaction with chlorine is the aldehyde called chloral, which forms chloral hydrate upon reaction with water:[94]

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.[75] 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. Safety[edit] See also: Alcohol
§ Toxicity Pure ethanol will irritate the skin and eyes.[95] Nausea, vomiting, and intoxication are symptoms of ingestion. Long-term use by ingestion can result in serious liver damage.[96] Atmospheric concentrations above one in a thousand are above the European Union occupational exposure limits.[96] History[edit] Further information: Distilled beverage The fermentation of sugar into ethanol is one of the earliest biotechnologies employed by humans. The intoxicating effects of ethanol 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.[97] The medieval Muslims used the distillation process extensively, and applied it to the distillation of alcohol. The Arab chemist Al-Kindi unambiguously described the distillation of wine in the 9th century.[98][99][100] The process later spread from the Middle East
Middle East
to Italy.[98][101] Production of alcohol from distilled wine was later recorded by the School of Salerno alchemists in the 12th century.[102] Mention of absolute alcohol, in contrast with alcohol-water mixtures, was later made by Raymond Lull in the 14th century.[102] In China, archaeological evidence indicates that the true distillation of alcohol began during the 12th century Jin or Southern Song dynasties.[103] A still has been found at an archaeological site in Qinglong, Hebei, dating to the 12th century.[103] In India, the true distillation of alcohol was introduced from the Middle East, and was in wide use in the Delhi Sultanate
Delhi Sultanate
by the 14th century.[101] 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.[104] French chemist Antoine Lavoisier
Antoine Lavoisier
described ethanol as a compound of carbon, hydrogen, and oxygen, and in 1807 Nicolas-Théodore de Saussure
Nicolas-Théodore de Saussure
determined ethanol's chemical formula.[105][106] Fifty years later, Archibald Scott Couper
Archibald Scott Couper
published the structural formula of ethanol. It was one of the first structural formulas determined.[107] Ethanol
was first prepared synthetically in 1825 by Michael Faraday. He found that sulfuric acid could absorb large volumes of coal gas.[108] He gave the resulting solution to Henry Hennell, a British chemist, who found in 1826 that it contained "sulphovinic acid" (ethyl hydrogen sulfate).[109] In 1828, Hennell and the French chemist Georges-Simon Serullas
Georges-Simon Serullas
independently discovered that sulphovinic acid could be decomposed into ethanol.[110][111] 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.[112] Ethanol
was used as lamp fuel in the United States 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.[113] Use as an automotive fuel dates back to 1908, with the Ford Model T
Ford Model T
able to run on petrol (gasoline) or ethanol.[114] It fuels some spirit lamps. Ethanol
intended for industrial use is often produced from ethylene.[115] 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]

1-Propanol Butanol fuel Cellulosic ethanol
Cellulosic ethanol
commercialization Ethanol-induced non-lamellar phases in phospholipids Ethenol Ethynol Isopropyl alcohol Methanol Rubbing alcohol tert-Butyl alcohol Timeline of alcohol fuel


^ a b " Ethanol
– Compound Summary". The PubChem Project. USA: National Center for Biotechnology
Information.  ^ a b c d Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 3.246. ISBN 1439855110.  ^ Ballinger P, Long FA (1960). " Acid
Ionization Constants of Alcohols. II. Acidities of Some Substituted Methanols and Related Compounds1,2". Journal of the American Chemical Society. 82 (4): 795–798. doi:10.1021/ja01489a008.  ^ Arnett EM, Venkatasubramaniam KG (1983). "Thermochemical acidities in three superbase systems". J. Org. Chem. 48 (10): 1569–1578. doi:10.1021/jo00158a001.  ^ Lide DR, ed. (2012). CRC Handbook of Chemistry
and Physics (92 ed.). Boca Raton, FL.: CRC Press/Taylor and Francis. pp. 6–232.  ^ Lide DR, ed. (2008). CRC Handbook of Chemistry
and Physics (89 ed.). Boca Raton: CRC Press. pp. 9–55.  ^ Liebig J (1834). "Ueber die Constitution des Aethers und seiner Verbindungen" [On the constitution of ether and its compounds]. Annalen der Pharmacie (in German). 9: 1–39. doi:10.1002/andp.18341072202. From page 18: "Bezeichnen wir die Kohlenwasserstoffverbindung 4C + 10H als das Radikal des Aethers mit E2 und nennen es Ethyl, ..." (Let us designate the hydrocarbon compound 4C + 10H as the radical of ether with E2 and name it ethyl ...).  ^ Harper, Douglas. "ethyl". Online Etymology Dictionary.  ^ For a report on the 1892 International Conference on Chemical Nomenclature, see:

Armstrong H (1892). "The International Conference on Chemical Nomenclature". Nature. 46 (1177): 56–59. Bibcode:1892Natur..46...56A. doi:10.1038/046056c0.  Armstrong's report is reprinted with the resolutions in English in: Armstrong H (1892). "The International Conference on Chemical Nomenclature". The Journal of Analytical and Applied Chemistry. 6: 390–400 (398). The alcohols and the phenols will be called after the name of the hydrocarbon from which they are derived, terminated with the suffix ol (ex. pentanol, pentenol, etc.) 

^ OED; etymonline.com ^ McDonnell G, Russell AD (January 1999). "Antiseptics and disinfectants: activity, action, and resistance". Clinical Microbiology Reviews. 12 (1): 147–79. PMC 88911 . PMID 9880479.  ^ "Chemical Disinfectants Disinfection & Sterilization Guidelines Guidelines Library Infection Control CDC". www.cdc.gov. Retrieved 2018-01-29.  ^ "Why is 70% ethanol used for wiping microbiological working areas?". ResearchGate. Retrieved 2018-01-29.  ^ " Methanol
poisoning". MedlinePlus. National Institute of Health. 30 January 2013. Retrieved 6 April 2015.  ^ Scalley R (September 2002). "Treatment of Ethylene
Glycol Poisoning". American Family Physician. 66 (5): 807–813. Retrieved 15 January 2018.  ^ Adams KE, Rans TS (December 2013). "Adverse reactions to alcohol and alcoholic beverages". Annals of Allergy, Asthma & Immunology. 111 (6): 439–45. doi:10.1016/j.anai.2013.09.016. PMID 24267355.  ^ Zuccotti GV, Fabiano V (July 2011). "Safety issues with ethanol as an excipient in drugs intended for pediatric use". Expert Opinion on Drug Safety. 10 (4): 499–502. doi:10.1517/14740338.2011.565328. PMID 21417862.  ^ a b Harger RN (1958). "The pharmacology and toxicology of alcohol". Journal of the American Medical Association. 167 (18): 2199–202. doi:10.1001/jama.1958.72990350014007. PMID 13563225.  ^ Wallner M, Olsen RW (2008). "Physiology and pharmacology of alcohol: the imidazobenzodiazepine alcohol antagonist site on subtypes of GABAA receptors as an opportunity for drug development?". British Journal of Pharmacology. 154 (2): 288–98. doi:10.1038/bjp.2008.32. PMC 2442438 . PMID 18278063.  ^ Alcohol
use and safe drinking. US National Institutes of Health. ^ "Appendix B – Transportation Energy Data Book". Center for Transportation Analysis of the Oak Ridge National Laboratory.  ^ a b Eyidogan M, Ozsezen AN, Canakci M, Turkcan A (2010). "Impact of alcohol–gasoline fuel blends on the performance and combustion characteristics of an SI engine". Fuel. 89 (10): 2713–2720. doi:10.1016/j.fuel.2010.01.032.  ^ a b Thomas, George: "Overview of Storage Development DOE Hydrogen Program" (PDF). Archived from the original (PDF) on 21 February 2007.  (99.6 KB). Livermore, CA. Sandia National Laboratories. 2000. ^ Thomas G (2000). "Overview of Storage Development DOE Hydrogen Program" (PDF). Sandia National Laboratories. Retrieved 1 August 2009.  ^ "Availability of Sources of E85". Clean Air Trust. Retrieved 27 July 2015.  ^ Reel M (19 August 2006). "Brazil's Road to Energy Independence". The Washington Post.  ^ Chow D (26 April 2010). " Rocket
Racing League Unveils New Flying Hot Rod". Space.com. Retrieved 27 April 2010.  ^ Green R. "Model T Ford Club Australia (Inc.)". Archived from the original on 14 January 2014. Retrieved 24 June 2011.  ^ " Ethanol
101". American Coalition for Ethanol.  ^ Energy Future Coalition. "The Biofuels FAQs". The Biofuels Source Book. United Nations Foundation. Archived from the original on 19 February 2011.  ^ California Air Resources Board
California Air Resources Board
(October 1989). "Definition of a Low Emission Motor Vehicle in Compliance with the Mandates of Health and Safety Code Section 39037.05, second release,".  ^ Lowi A, Carter WP (March 1990). A Method for Evaluating the Atmospheric Ozone
Impact of Actual Vehicle emissions. S.A.E. Technical Paper. Warrendale, PA.  ^ Jones TT (2008). "The Clean Fuels Report: A Quantitative Comparison Of Motor (engine) Fuels, Related Pollution and Technologies". researchandmarkets.com. Archived from the original on 18 May 2016.  ^ Tao R (16–20 August 2010). Electro-rheological Fluids and Magneto-rheological Suspensions. Proceedings of the 12th International Conference. Philadelphia, USA: World Scientific. ISBN 9789814340229.  ^ Biello D. "Want to Reduce Air Pollution? Don't Rely on Ethanol Necessarily". Scientific American. Retrieved 11 July 2017.  ^ "Adoption of the Airborne Toxic Control Measure to Reduce Formaldehyde
Emissions from Composite Wood Products". USA: Window and Door Manufacturers Association. 30 July 2008. Archived from the original on 9 March 2010.  ^ "2008 World Fuel
Production". U.S.: Renewable Fuels Association.  ^ "Tecnologia flex atrai estrangeiros". Agência Estado.  ^ "First Commercial U.S. Cellulosic Ethanol
Biorefinery Announced". Renewable Fuels Association. 20 November 2006. Retrieved 31 May 2011.  ^ Sweet sorghum
Sweet sorghum
for food, feed and fuel New Agriculturalist, January 2008. ^ Developing a sweet sorghum ethanol value chain ICRISAT, 2013 ^ Horn M, Krupp F (16 March 2009). Earth: The Sequel: The Race to Reinvent Energy and Stop Global Warming. W. W. Norton. p. 85. ISBN 978-0-393-06810-8.  ^ Mechanics see ethanol damaging small engines, Msnbc.com, 8 January 2008 ^ Darling D. "The Internet Encyclopedia of Science: V-2".  ^ a b Braeunig, Robert A. " Rocket
Propellants." (Website). Rocket & Space Technology, 2006. Retrieved 23 August 2007. ^ "A Brief History of Rocketry." NASA Historical Archive, via science.ksc.nasa.gov. ^ Badwal SP, Giddey S, Kulkarni A, Goel J, Basu S (May 2015). "Direct ethanol fuel cells for transport and stationary applications – A comprehensive review". Applied Energy. 145: 80–103. doi:10.1016/j.apenergy.2015.02.002.  ^ "Can Ethanol
Fireplaces Be Cozy?". Wall Street Journal. Retrieved 2 March 2016.  ^ a b c Lide DR, ed. (2000). CRC Handbook of Chemistry
and Physics 81st edition. CRC press. ISBN 0-8493-0481-4.  ^ "What is the triple point of alcohol?". Webanswers.com. 31 December 2010. Archived from the original on 14 May 2013. [scientific citation needed] ^ a b c d Windholz M (1976). The Merck index: an encyclopedia of chemicals and drugs (9th ed.). Rahway, N.J., U.S.A: Merck. ISBN 0-911910-26-3. [page needed] ^ a b c Morrison RT, Boyd RN (1972). Organic Chemistry
(2nd ed.). Allyn and Bacon, inc. ISBN 0-205-08452-4. [page needed] ^ Dahlmann U, Schneider GM (1989). "(Liquid + liquid) phase equilibria and critical curves of (ethanol + dodecane or tetradecane or hexadecane or 2,2,4,4,6,8,8-heptamethylnonane) from 0.1 MPa to 120.0 MPa". J Chem Thermodyn. 21 (9): 997–1004. doi:10.1016/0021-9614(89)90160-2.  ^ "Ethanol". Encyclopedia of chemical technology. 9. 1991. p. 813.  ^ Costigan MJ, Hodges LJ, Marsh KN, Stokes RH, Tuxford CW (1980). "The Isothermal Displacement Calorimeter: Design Modifications for Measuring Exothermic
Enthalpies of Mixing". Aust. J. Chem. 33 (10): 2103. doi:10.1071/CH9802103.  ^ Lei Z, Wang H, Zhou R, Duan Z (2002). "Influence of salt added to solvent on extractive distillation". Chem Eng J. 87 (2): 149–156. doi:10.1016/S1385-8947(01)00211-X.  ^ Pemberton RC, Mash CJ (1978). "Thermodynamic properties of aqueous non-electrolyte mixtures II. Vapour pressures and excess Gibbs energies for water + ethanol at 303.15 to 363.15 K determined by an accurate static method". J Chem Thermodyn. 10 (9): 867–888. doi:10.1016/0021-9614(78)90160-X.  ^ Merck Index of Chemicals and Drugs, 9th ed.; monographs 6575 through 6669 ^ "Flash Point and Fire Point". Nttworldwide.com. Archived from the original on 14 December 2010.  ^ "Flash points of ethanol-based water solutions". Engineeringtoolbox.com. Retrieved 23 June 2011.  ^ Dudley R (August 2004). "Ethanol, fruit ripening, and the historical origins of human alcoholism in primate frugivory". Integrative and Comparative Biology. 44 (4): 315–23. doi:10.1093/icb/44.4.315. PMID 21676715.  ^ Graber C (2008). "Fact or Fiction?: Animals Like to Get Drunk". Scientific American. Retrieved 23 July 2010.  ^ Leblová S, Sinecká E, Vaníčková V (1974). "Pyruvate metabolism in germinating seeds during natural anaerobiosis". Biologia Plantarum. 16 (6): 406–411. doi:10.1007/BF02922229.  ^ Schriver A, Schriver-Mazzuoli L, Ehrenfreund P, d'Hendecourt L (2007). "One possible origin of ethanol in interstellar medium: Photochemistry of mixed CO2–C2H6 films at 11 K. A FTIR study". Chemical Physics. 334 (1–3): 128–137. Bibcode:2007CP....334..128S. doi:10.1016/j.chemphys.2007.02.018.  ^ Turner C, Spanel P, Smith D (2006). "A longitudinal study of ethanol and acetaldehyde in the exhaled breath of healthy volunteers using selected-ion flow-tube mass spectrometry". Rapid Communications in Mass Spectrometry. 20 (1): 61–8. doi:10.1002/rcm.2275. PMID 16312013.  ^ Doucleff M (17 September 2013). "Auto-Brewery Syndrome: Apparently, You Can Make Beer
In Your Gut". NPR.  ^ Mills GA, Ecklund EE (1987). "Alcohols as Components of Transportation Fuels". Annual Review of Energy. 12: 47–80. doi:10.1146/annurev.eg.12.110187.000403.  ^ Wittcoff HA, Reuben BG, Plotkin JS (2004). Industrial Organic Chemicals. John Wiley & Sons. pp. 136–. ISBN 978-0-471-44385-8.  ^ Roberts JD, Caserio MC (1977). Basic Principles of Organic Chemistry. W. A. Benjamin, Inc. ISBN 0-8053-8329-8. [page needed] ^ a b c d Kosaric N, Duvnjak Z, Farkas A, Sahm H, Bringer-Meyer S, Goebel O, Mayer D (2011). "Ethanol". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a09_587.pub2. (subscription required) ^ "Ethanol". Encyclopedia of chemical technology. 9. 1991. p. 82.  ^ Ethanol. essentialchemicalindustry.org ^ Harrison, Tim (May 2014) Catalysis
Web Pages for Pre-University Students V1_0. Bristol ChemLabS, School of Chemistry, University of Bristol ^ Lodgsdon JE (1991). "Ethanol". In Howe-Grant, Mary, Kirk, Raymond E., Othmer, Donald F., Kroschwitz, Jacqueline I. Encyclopedia of chemical technology. 9 (4th ed.). New York: Wiley. p. 817. ISBN 0-471-52669-X.  ^ a b c d e Streitwieser A, Heathcock CH (1976). I ntroduction to Organic Chemistry. MacMillan. ISBN 0-02-418010-6.  ^ Biological production of ethanol from CO2 produced by a fossil-fueled power plant. ^ Liew F, Henstra AM, Köpke M, Winzer K, Simpson SD, Minton NP (March 2017). "Metabolic engineering of Clostridium autoethanogenum for selective alcohol production". Metabolic Engineering. 40: 104–114. doi:10.1016/j.ymben.2017.01.007. PMC 5367853 . PMID 28111249.  ^ "Solar-to- Fuel
System Recycles CO2 for Ethanol
and Ethylene". News Center. 18 September 2017. Retrieved 19 September 2017.  ^ "TU Delft researcher makes alcohol out of thin air". TU Delft. Retrieved 19 September 2017.  ^ Menetrez MY (July 2012). "An overview of algae biofuel production and potential environmental impact" (PDF). Environmental Science & Technology. 46 (13): 7073–85. Bibcode:2012EnST...46.7073M. doi:10.1021/es300917r. PMID 22681590.  ^ Clines T (July 2006). "Brew Better Ethanol". Popular Science Online. Archived from the original on 3 November 2007.  ^ Chemists, American Association of Cereal (1986). Advances in Cereal Science and Technology. American Association of Cereal Chemists, Incorporated. ISBN 9780913250457.  ^ Song Y, Peng R, Hensley DK, Bonnesen PV, Liang L, Wu Z, Meyer HM, Chi M, Ma C, Sumpter BG, Rondinone AJ (2016). "High-Selectivity Electrochemical
Conversion of CO2 to Ethanol
using a Copper Nanoparticle/N-Doped Graphene
Electrode". ChemistrySelect. 1 (Preprint): 6055–6061. doi:10.1002/slct.201601169.  ^ Jeong J, Jeon H, Ko K, Chung B, Choi G (2012). "Production of anhydrous ethanol using various PSA (Pressure Swing Adsorption) processes in pilot plant". Renewable Energy. 42: 41–45. doi:10.1016/j.renene.2011.09.027.  ^ "U-M Program to Reduce the Consumption of Tax-free Alcohol; Denatured Alcohol
a Safer, Less Expensive Alternative" (PDF). University of Michigan. Archived from the original (PDF) on 27 November 2007. Retrieved 29 September 2007.  ^ Great Britain (2005). The Denatured Alcohol
Regulations 2005. Statutory Instrument 2005 No. 1524. ^ Bansal RK, Bernthsen A (2003). A Textbook of Organic Chemistry. New Age International Limited. pp. 402–. ISBN 978-81-224-1459-2.  ^ Christian GD (2004). "Solvents for Spectrometry". Analytical chemistry. 1 (6th ed.). Hoboken, N.J.: John Wiley & Sons. p. 473. ISBN 978-0471214724.  ^ Andrews S (1 August 2007). Textbook Of Food & Bevrge Mgmt. Tata McGraw-Hill Education. pp. 268–. ISBN 978-0-07-065573-7.  ^ Kunkee RE, Amerine MA (July 1968). " Sugar
and alcohol stabilization of yeast in sweet wine". Applied Microbiology. 16 (7): 1067–75. PMC 547590 . PMID 5664123.  ^ Rossini FD (1937). "Heats of Formation of Simple Organic Molecules". Ind. Eng. Chem. 29 (12): 1424–1430. doi:10.1021/ie50336a024.  ^ Calculated from heats of formation from CRC Handbook of Chemistry and Physics, 49th Edition, 1968–1969. ^ Chakrabartty SK (1978). Trahanovsky WS, ed. Oxidation in Organic Chemistry. New York: Academic Press. pp. 343–370.  ^ Reinhard J, Kopp E, McKusick BC, Röderer G, Bosch A, Fleischmann G (2007). "Chloroacetaldehydes". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a06_527.pub2.  ^ Minutes of Meeting. Technical Committee on Classification and Properties of Hazardous Chemical Data ( 12–13 January 2010). ^ a b "Safety data for ethyl alcohol". University of Oxford. 9 May 2008. Retrieved 3 January 2011.  ^ Roach J (18 July 2005). "9,000-Year-Old Beer
Re-Created From Chinese Recipe". National Geographic News. Retrieved 3 September 2007.  ^ a b al-Hassan AY (2001). Science and Technology in Islam: Technology and applied sciences. UNESCO. pp. 65–69.  ^ Hassan AY. " Alcohol
and the Distillation
of Wine in Arabic Sources". History of Science and Technology in Islam. Retrieved 19 April 2014.  ^ "Liquid fire – The Arabs discovered how to distil alcohol. They still do it best, say some". The Economist. 18 December 2003.  ^ a b Habib, Irfan (2011). Economic History of Medieval India, 1200-1500. Pearson Education India. pp. 55–. ISBN 978-81-317-2791-1.  ^ a b Forbes RJ (1948). A short history of the art of distillation. Brill. p. 89. ISBN 9004006176.  ^ 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  ^ 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 für die Freunde der Naturlehre, Aerznengelartheit, Haushaltungskunde und Manufakturen (in German). Lorenz Von Crell. 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". Encyclopædia Britannica. 1 (11th ed.). Cambridge University Press. pp. 525–527.  ^ de Saussure T (1807). "Mémoire sur la composition de l'alcohol et de l'éther sulfurique". Journal de physique, de chimie, d'histoire naturelle et des arts. Fuchs. 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, Théodore (1814). "Nouvelles observations sur la composition de l'alcool et de l'éther sulfurique". Annales de chimie et de physique. Masson. 89: 273–305.  ^ Couper AS (1858). "On a new chemical theory" (online reprint). Philosophical Magazine. 16 (104–16). 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. Royal Society (London). 116: 240–249. doi:10.1098/rstl.1826.0021.  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.  On page 368, Hennell produces ethanol from "sulfovinic acid" (ethyl hydrogen sulfate). ^ Sérullas G (1828). Guyton de Morveau L, Gay-Lussac JL, Arago F, Michel Eugène Chevreul, Marcellin Berthelot, Éleuthère Élie Nicolas Mascart, Albin Haller, eds. "De l'action de l'acide sulfurique sur l'alcool, et des produits qui en résultent". Annales de chimie et de physique. Masson. 39: 152–186.  On page 158, Sérullas mentions the production of alcohol from "sulfate acid d'hydrogène carboné" (hydrocarbon acid sulfate). ^ In 1855, the French chemist Marcellin Berthelot
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'hydrogène (On the formation of alcohol by means of ethylene)". Annales de chimie et de physique. Chez Crochard. 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, Conn.: Greenwood Press. p. 122. ISBN 0-313-33758-6. 

Further reading[edit]

Boyce JM, Pittet D (2003). "Hand Hygiene in Healthcare Settings". Atlanta, Georgia, United States: 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. 

External links[edit]

Look up alcohol or ethanol in Wiktionary, the free dictionary.

Wikimedia Commons has media related to Ethanol.

(Ethanol) at The Periodic Table of Videos
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

v t e


Straight-chain primary alcohols (1°)

(C 1) Ethanol
(C 2) 1-Propanol
(C 3) n-Butanol (C 4) 1-Pentanol
(C 5) 1-Hexanol
(C 6) 1-Heptanol
(C 7) 1-Octanol
(C 8) 1-Nonanol
(C 9) 1-Decanol
(C 10) Undecanol
(C 11) Dodecanol
(C 12) Tridecan-1-ol (C 13) 1-Tetradecanol
(C 14) Pentadecan-1-ol (C 15) Cetyl alcohol
Cetyl alcohol
(C 16) Heptadecan-1-ol (C 17) Stearyl alcohol
Stearyl alcohol
(C 18) Nonadecan-1-ol (C 19) Arachidyl alcohol
Arachidyl alcohol
(C 20) Heneicosan-1-ol (C 21) Docosanol
(C 22) Tricosan-1-ol (C 23) 1-Tetracosanol
(C 24) Pentacosan-1-ol (C 25) 1-Hexacosanol
(C 26) 1-Heptacosanol
(C 27) 1-Octacosanol
(C 28) 1-Nonacosanol
(C 29) Triacontanol
(C 30)

Other primary alcohols

(C 4) Isoamyl alcohol
Isoamyl alcohol
(C 5) 2-Methyl-1-butanol
(C 5) Phenethyl alcohol
Phenethyl alcohol
(C 8) Tryptophol
(C 10)

Secondary alcohols (2°)

Isopropanol (C 3) 2-Butanol
(C 4) 2-Pentanol
(C 5) 2-Hexanol
(C 6) 2-Heptanol
(C 7) Cyclohexanol
(C 6) 2-Octanol
(C 8)

Tertiary alcohols (3°)

tert-Butyl alcohol (C 4) tert-Amyl alcohol (C 5) 2-Methyl-2-pentanol
(C 6) 2-Methylhexan-2-ol (C 7) 2-Methylheptan-2-ol (C 8) 3-Methyl-3-pentanol
(C 6) 3-Methyloctan-3-ol (C 9)

v t e

Motor fuels


Gasoline/petrol Diesel Biodiesel Lead Replacement Petrol Kerosene Compressed natural gas Hydrogen Ethanol Butanol fuel Racing fuel (Tetraethyllead)


Butyl rubber Butylated hydroxytoluene 1,2-Dibromoethane 1,2-Dichloroethane Dimethyl methylphosphonate 2,4-Dimethyl-6-tert-butylphenol Dinonylnaphthylsulfonic acid 2,6-Di-tert-butylphenol Ecalene Ethylenediamine Metal deactivator Methyl tert-butyl ether Nitromethane Tetraethyllead Tetranitromethane


Motor oil Antifreeze Automatic transmission fluid Brake fluid Gear oil Windshield washer fluid


card Full service MTBE controversy Pay at the pump

v t e

Molecules detected in outer space



Aluminium monochloride Aluminium monofluoride Aluminium monoxide Argonium Carbon
monophosphide Carbon
monosulfide Carbon
monoxide Carborundum Cyanogen
radical Diatomic carbon Fluoromethylidynium Hydrogen
chloride Hydrogen
fluoride Hydrogen
(molecular) Hydroxyl
radical Iron(II) oxide Magnesium monohydride cation Methylidyne radical Nitric oxide Nitrogen
(molecular) Nitrogen
monohydride Nitrogen
sulfide Oxygen
(molecular) Phosphorus monoxide Phosphorus mononitride Potassium chloride Silicon carbide Silicon mononitride Silicon monoxide Silicon monosulfide Sodium
chloride Sodium
iodide Sulfur monohydride Sulfur monoxide Titanium oxide


Aluminium hydroxide Aluminium isocyanide Amino radical Carbon
dioxide Carbonyl sulfide CCP radical Chloronium Diazenylium Dicarbon monoxide Disilicon carbide Ethynyl radical Formyl radical Hydrogen
cyanide (HCN) Hydrogen
isocyanide (HNC) Hydrogen
sulfide Hydroperoxyl Iron cyanide Isoformyl Magnesium cyanide Magnesium isocyanide Methylene radical N2H+ Nitrous oxide Nitroxyl Ozone Phosphaethyne Potassium cyanide Protonated molecular hydrogen Sodium
cyanide Sodium
hydroxide Silicon carbonitride c-Silicon dicarbide Silicon naphthalocyanine Sulfur dioxide Thioformyl Thioxoethenylidene Titanium dioxide Tricarbon Water

Four atoms

Acetylene Ammonia Cyanic acid Cyanoethynyl Cyclopropynylidyne Formaldehyde Fulminic acid HCCN Hydrogen
peroxide Hydromagnesium isocyanide Isocyanic acid Isothiocyanic acid Ketenyl Methylene amidogen Methyl radical Propynylidyne Protonated carbon dioxide Protonated hydrogen cyanide Silicon tricarbide Thioformaldehyde Tricarbon
monoxide Tricarbon
sulfide Thiocyanic acid

Five atoms

ion Butadiynyl Carbodiimide Cyanamide Cyanoacetylene Cyanoformaldehyde Cyanomethyl Cyclopropenylidene Formic acid Isocyanoacetylene Ketene Methane Methoxy
radical Methylenimine Propadienylidene Protonated formaldehyde Protonated formaldehyde Silane Silicon-carbide cluster

Six atoms

Acetonitrile Cyanobutadiynyl radical E-Cyanomethanimine Cyclopropenone Diacetylene Ethylene Formamide HC4N Ketenimine Methanethiol Methanol Methyl isocyanide Pentynylidyne Propynal Protonated cyanoacetylene

Seven atoms

Acetaldehyde Acrylonitrile

Vinyl cyanide

Cyanodiacetylene Ethylene
oxide Hexatriynyl radical Methylacetylene Methylamine Methyl isocyanate Vinyl alcohol

Eight atoms

Acetic acid Aminoacetonitrile Cyanoallene Ethanimine Glycolaldehyde Heptatrienyl radical Hexapentaenylidene Methylcyanoacetylene Methyl formate Propenal

Nine atoms

Acetamide Cyanohexatriyne Cyanotriacetylene Dimethyl ether Ethanol Methyldiacetylene Octatetraynyl radical Propene Propionitrile

Ten atoms or more

Acetone Benzene Benzonitrile Buckminsterfullerene
(C60 fullerene, buckyball) C70 fullerene Cyanodecapentayne Cyanopentaacetylene Cyanotetra-acetylene Ethylene
glycol Ethyl formate Methyl acetate Methyl-cyano-diacetylene Methyltriacetylene Propanal n-Propyl cyanide Pyrimidine

Deuterated molecules

Ammonia Ammonium
ion Formaldehyde Formyl radical Heavy water Hydrogen
cyanide Hydrogen
deuteride Hydrogen
isocyanide Methylacetylene N2D+ Trihydrogen cation


Anthracene Dihydroxyacetone Ethyl methyl ether Glycine Graphene H2NCO+ Linear C5 Naphthalene
cation Phosphine Pyrene Silylidine


Abiogenesis Astrobiology Astrochemistry Atomic and molecular astrophysics Chemical formula Circumstellar envelope Cosmic dust Cosmic ray Cosmochemistry Diffuse interstellar band Earliest known life forms Extraterrestrial life Extraterrestrial liquid water Forbidden mechanism Helium hydride ion Homochirality Intergalactic dust Interplanetary medium Interstellar medium Photodissociation region Iron–sulfur world theory Kerogen Molecules in stars Nexus for Exoplanet System Science Organic compound Outer space PAH world hypothesis Panspermia Polycyclic aromatic hydrocarbon
Polycyclic aromatic hydrocarbon
world hypothesis Spectroscopy Tholin

Book:Chemistry Category:Astrochemistry Category:Molecules Portal:Astrobiology Portal:Astronomy Portal:Chemistry

Authority control

LCCN: sh2009007801 GND: 41258