User:Andarisekar/sandbox

Molecular Formula = C2H6O Displayed formula =

Dots and Cross diagrams showing the covalent bonds The homologous series it belongs to = Alcohol Physical properties such appearance, melting point, boiling point and solubility Appearance Pure ethanol is a flammable, colorless liquid. Its density is 789 g/l about 20% less than that of water. '''Boiling Point  78.5° C. Melting Point  -114.5° C Solubility''' Because of the strength of the attraction of the OH group, first three alcohols (methanol, ethanol and propanol) are completely miscible. They dissolve in water in any amount.

Structure and Bonding

'''USES : ''' Ethanol is a good fuel for use in spark-ignition engines. It has high octane number, making it attractive as an antiknock additive in gasoline. It can be used as an additive for diesel (biodiesel). Ethanol is also an important feedstock for the chemical industry. ( https://extension.illinois.edu/ethanol/ )

'''HOW IT IS MADE: ''' -reactions (equation) >FROM ETHENE AND STEAM ethene + steam → ethanol C2H4 + H2O → C2H5OH The process is continuous – as long as ethene and steam are fed into one end of the reaction vessel, ethanol will be produced. These features make it an efficient process, but there is a problem. Ethene is made from crude oil, which is a non-renewable resource. It cannot be replaced once it is used up and it will run out one day.

>BY FERMENTATION Sugar from plant material is converted into ethanol and carbon dioxide by fermentation. The enzymes found in single-celled fungi (yeast) are the natural catalysts that can make this process happen. C66H12O6 → 2C2H5OH + 2CO2 Unlike ethene, sugar from plant material is a renewable resource. ( http://www.bbc.co.uk/schools/gcsebitesize/science/aqa/substancesfromcrudeoil/polymersandethanolrev4.shtml )

'''REACTIONS: ''' --Ester formation-- In the presence of acid catalysts, ethanol reacts with carboxylic acids to produce ethyl esters and water: RCOOH + HOCH2CH3 → RCOOCH2CH3 + H2O

--Dehydration-- 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. 2 CH3CH2OH → CH3CH2OCH2CH3 + H2O (ca. 120 °C) CH3CH2OH → H2C=CH2 + H2O (above 160 °C)

--Combustion-- Complete combustion of ethanol forms carbon dioxide and water: C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (l); −ΔHc = 1371 kJ/mol[95] = 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[96] Specific heat = 2.44 kJ/(kg·K)

--Acid-base chemistry-- 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:[55] 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-- 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.[78] HBr requires refluxing with a sulfuric acid catalyst.[78] Ethyl halides can, in principle, also be produced by treating ethanol with more specialized halogenating agents, such as thionyl chloride or phosphorus tribromide.[55][78] 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.[97] " An intermediate in the reaction with chlorine is the aldehyde called chloral, which forms chloral hydrate upon reaction with water:[98] 4 Cl2 + CH3CH2OH → CCl3CHO + 5 HCl CCl3CHO + H2O → CCl3C(OH)2H --Oxidation-- Ethanol can be oxidized to acetaldehyde and further oxidized to acetic acid, depending on the reagents and conditions.[78] 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. ( https://en.wikipedia.org/wiki/Ethanol#Etymology )