Ethanol

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For ethanol as a drug or medicine, see Alcohol (drug) and Alcohol (medicine).
Not to be confused with ethenol, also known as vinyl alcohol, or ethynol.

Ethanol
Full structural formula of ethanol
Skeletal formula of ethanol
Ball-and-stick model of ethanol
Space-filling model of ethanol
Names
Pronunciation /ˈɛθənɒl/
Systematic IUPAC name
ethanol[1]
Other names
Absolute alcohol
alcohol
cologne spirit
drinking alcohol
ethylic alcohol
EtOH
ethyl alcohol
ethyl hydrate
ethyl hydroxide
ethylol
grain alcohol
hydroxyethane
methylcarbinol
Identifiers
3D model (JSmol)
3DMet B01253
1718733
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.000.526
E number E1510 (additional chemicals)
787
UNII
UN number UN 1170
Properties
C2H6O
Molar mass 46.069 g·mol−1
Appearance Colorless liquid
Density 0.7893 g/cm3 (at 20 °C)[2]
Melting point −114.14 ± 0.03[2] °C (−173.45 ± 0.05 °F; 159.01 ± 0.03 K)
Boiling point 78.24 ± 0.09[2] °C (172.83 ± 0.16 °F; 351.39 ± 0.09 K)
miscible
log P −0.18
Vapor pressure 5.95 kPa (at 20 °C)
Acidity (pKa) 15.9 (H2O), 29.8 (DMSO)[3][4]
−33.60·10−6 cm3/mol
1.3611[2]
Viscosity 1.2 mPa·s (at 20 °C), 1.074 mPa·s (at 25 °C)[5]
1.69 D[6]
Hazards
Safety data sheet See: data page
[7]
GHS pictograms The flame pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS) The exclamation-mark pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS)
GHS signal word Danger
H225, H319
P210, P280, P305+351+338
NFPA 704
Flash point 14 °C (Absolute)[citation needed] 
Lethal dose or concentration (LD, LC):
7340 mg/kg (oral, rat)
7300 mg/kg (mouse)
US health exposure limits (NIOSH):
PEL (Permissible)
 TWA 1000 ppm (1900 mg/m3) [8]
REL (Recommended)
 TWA 1000 ppm (1900 mg/m3) [8]
IDLH (Immediate danger)
 N.D.[8]
Related compounds
Related compounds
 Ethane
Methanol
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references

Ethanol (also called ethyl alcohol, grain alcohol, drinking alcohol, or simply alcohol) is a chemical compound, a simple alcohol with the chemical formula C
2H
6O. Its formula can be also written 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 used across many different kinds of manufacturing industries. Ethanol is also used as a clean-burning fuel source.

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”).[10] 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”).[11]

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.[12]

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 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.[13] The use of “alcohol” for ethanol (in full, “alcohol of wine”) is modern, first recorded 1753, and by the later 18th century referred to “any sublimated substance”; “distilled spirit” used for “the spirit of wine” (shortened from a full expression the spirit of alcohol of wine). The systematic use in chemistry dates to 1850.

Uses[edit]

Medical[edit]

Main article: Alcohol (medicine)

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.[14] 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.[15] 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.[16][17] Ethanol can also be used as a disinfectant and antiseptic because it causes cell dehydration by disrupting the osmotic balance across cell membrane, so water leaves the cell leading to cell death.[18]

Antidote[edit]

Ethanol may be administered as an antidote to methanol[19] and ethylene glycol poisoning.[20]

Medicinal solvent[edit]

Ethanol, often in high concentrations, is used to dissolve many water-insoluble medications and related compounds. Liquid preparations of crack cocaine, 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.[21] 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.[22]

Pharmacology[edit]

If ingested orally, ethanol is extensively metabolized by the liver, particularly via the enzyme CYP450.[23] Ethyl Alcohol increases the secretion of acids in the stomach.[23] The metabolite acetaldehyde is responsible for much of the short term, and long term effects of ethyl alcohol toxicity.[24]

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.[25]

Fuel[edit]

Engine fuel[edit]

Main article: Ethanol fuel
Energy content of some fuels compared with ethanol:[26]
Fuel type MJ/L MJ/kg Research
octane
number
Dry wood (20% moisture) ~19.5
Methanol 17.9 19.9 108.7[27]
Ethanol 21.2[28] 26.8[28] 108.6[27]
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[29] 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.[30] 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.[31] 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.

Ethanol has been used as rocket fuel and is currently in lightweight rocket-powered racing aircraft.[32]

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.[33]

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.[34] 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.[35]

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.[36] This leads to a significantly larger photochemical reactivity and more ground level ozone.[37] These data have been assembled into The Clean Fuels Report comparison of fuel emissions[38] and show that ethanol exhaust generates 2.14 times as much ozone as gasoline exhaust.[39] 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.[40] 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).[41]

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.[42] More than 20% of Brazilian cars are able to use 100% ethanol as fuel, which includes ethanol-only engines and flex-fuel engines.[43] 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.[44]

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 sorghum as a source of fuel, food, and animal feed in arid parts of Asia and Africa.[45] 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.[46]

Ethanol's high miscibility with water makes it unsuitable for shipping through modern pipelines like liquid hydrocarbons.[47] 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.[48]

Ethanol pump station
Ethanol pump station in São Paulo, Brazil
Ford Taurus photograph
A Ford Taurus fueled by ethanol in New York City
Postal service photograph
USPS 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 V-2 rocket of World War II, credited with beginning the space age, used ethanol as the main constituent of B-Stoff, under such nomenclature the ethanol was mixed with 25% of water to reduce the combustion chamber temperature.[49][50] 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.[51] Alcohols fell into general disuse as more efficient rocket fuels were developed.[50]

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.[52]

Household heating[edit]

Ethanol fireplaces can be used for home heating or for decoration.[53]

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[54], 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. 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]

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 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).[55] The triple point for ethanol is 150 K at a pressure of 4.3 × 10−4 Pa.[56]

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.[55][57] It is also miscible with light aliphatic hydrocarbons, such as pentane and hexane, and with aliphatic chlorides such as trichloroethane and tetrachloroethylene.[57]

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.[58] 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[59]). 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.[55][60] Mixing ethanol and water is exothermic, with up to 777 J/mol[61] being released at 298 K.

Mixtures of ethanol and water form an azeotrope at about 89 mole-% ethanol and 11 mole-% water[62] 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.[63]

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.[57] Sodium and potassium chlorides are slightly soluble in ethanol.[57] Because the ethanol molecule also has a nonpolar end, it will also dissolve nonpolar substances, including most essential oils[64] 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 mass (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.[65] The flash point of pure ethanol is 13 °C (55 °F),[66] less than average room temperature. Ethanol is considered a flammable liquid (Class 3 Hazardous Material) in concentrations above 2.35% by volume.[67][68][69]

Flash points of ethanol–water mixtures[70][68][71]
Ethanol
mass fraction, % 		Temperature
°C °F
1 84.5 184.1[68]
2 64 147[68]
2.35 60 140[68][67]
3 51.5 124.7[68]
5 43 109[70]
6 39.5 103.1[68]
10 31 88[70]
20 25 77[68]
30 24 75[70]
40 26 79[citation needed][71]
50 20 68[70][68]
60 22 72[citation needed][71]
70 16 61[70]
80 15.8 60.4[68]
90 14 57[70]
100 12.5 54.5[70][68][66]

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.[72] 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.[73] Ethanol is also produced during the germination of many plants as a result of natural anerobiosis.[74] Ethanol has been detected in outer space, forming an icy coating around dust grains in interstellar clouds.[75] Minute quantity amounts (average 196 ppb) of endogenous ethanol and acetaldehyde were found in the exhaled breath of healthy volunteers.[76] 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.[77]

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.[78] 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.[79]

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,[80][81] 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.[82] 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.[83][84] In the U.S., this process was used on an industrial scale by 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,[85] 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:[86]

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 reduced by hydrogen to produce ethanol, acetic acid, and smaller amounts of 2,3-butanediol and lactic acid using Clostridium ljungdahlii, Clostridium autoethanogenum or Moorella sp. HUC22-1.[87][88]

CO2 can be converted using electrochemical reactions at room temperature and pressure.[89][90] In a system developed at Delft University of Technology, a copper nanowire array used as a cathode adsorbs molecules of carbon dioxide and reduced intermediate species such as CO and COH. However, even in the best results about half the current went into producing hydrogen and only a small amount of ethanol was produced. Other products, produced in larger quantities, were (in decreasing order) formic acid, ethylene, CO, and n-propanol.[91]

From lipids[edit]

Lipids can also be used to make ethanol and can be found in such raw materials such as algae.[92]

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

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 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.[93]

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.[81]

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 and desiccants[edit]

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.[81] Molecular sieves can be used to selectively absorb the water from the 95.6% ethanol solution.[94] 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:[81]

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.[97][98]

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).[99] 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.[100]

Pure ethanol is classed as 200 proof in the U.S., equivalent to 175 degrees proof in the UK system.[101]

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.[102]

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:

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, ethanol converts to ethylene. Typically solid acids such as silica are used:[103]

   CH3CH2OH → H2C=CH2 + H2O

Ethylene produced in this way competes with ethylene from oil refineries and fracking.

Under alternative conditions, diethyl ether results:

2 CH3CH2OH → CH3CH2OCH2CH3 + H2O

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[104] = 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[105]

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:[58]

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:

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

These reactions require a catalyst such as zinc chloride.[86] HBr requires refluxing with a sulfuric acid catalyst.[86] Ethyl halides can, in principle, also be produced by treating ethanol with more specialized halogenating agents, such as thionyl chloride or phosphorus tribromide.[58][86]

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.[106] " An intermediate in the reaction with chlorine is the aldehyde called chloral, which forms chloral hydrate upon reaction with water:[107]

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.[86] 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.[108] Nausea, vomiting, and intoxication are symptoms of ingestion. Long-term use by ingestion can result in serious liver damage.[109] Atmospheric concentrations above one in a thousand are above the European Union occupational exposure limits.[109]

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.[110]

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.[111][112][113] The process later spread from the Middle East to Italy.[111][114] Production of alcohol from distilled wine was later recorded by the School of Salerno alchemists in the 12th century.[115] Mention of absolute alcohol, in contrast with alcohol-water mixtures, was later made by Raymond Lull in the 14th century.[115]

In China, archaeological evidence indicates that the true distillation of alcohol began during the 12th century Jin or Southern Song dynasties.[116] A still has been found at an archaeological site in Qinglong, Hebei, dating to the 12th century.[116] 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.[114]

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.[117] 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.[118][119] Fifty years later, Archibald Scott Couper published the structural formula of ethanol. It was one of the first structural formulas determined.[120]

Ethanol was first prepared synthetically in 1825 by Michael Faraday. He found that sulfuric acid could absorb large volumes of coal gas.[121] He gave the resulting solution to Henry Hennell, a British chemist, who found in 1826 that it contained "sulphovinic acid" (ethyl hydrogen sulfate).[122] In 1828, Hennell and the French chemist Georges-Simon Serullas independently discovered that sulphovinic acid could be decomposed into ethanol.[123][124] 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.[125]

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.[126] Use as an automotive fuel dates back to 1908, with the Ford Model T able to run on petrol (gasoline) or ethanol.[127] It fuels some spirit lamps.

Ethanol intended for industrial use is often produced from ethylene.[128] 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]

References[edit]

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  121. ^ 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."
  122. ^ 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. 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).
  123. ^ 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).
  124. ^ 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. 39: 152–186. On page 158, Sérullas mentions the production of alcohol from "sulfate acid d'hydrogène carboné" (hydrocarbon acid sulfate).
  125. ^ 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'hydrogène (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.)
  126. ^ Siegel R (15 February 2007). "Ethanol, Once Bypassed, Now Surging Ahead". NPR. Retrieved 22 September 2007.
  127. ^ 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.
  128. ^ Myers RL, Myers RL (2007). The 100 most important chemical compounds: a reference guide. Westport, Conn.: Greenwood Press. p. 122. ISBN 978-0-313-33758-1.

Further reading[edit]

External links[edit]

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