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Excess volume of the mixture of ethanol and water (volume contraction) Heat of mixing of the mixture of ethanol and water Vapor–liquid equilibrium of the mixture of ethanol and water (including azeotrope) Solid–liquid equilibrium of the mixture of ethanol and water (including eutecticum) Miscibility gap in the mixture of dodecane and ethanol
Boiling point (°C) K b (°C⋅kg/mol) Freezing point (°C) ... Ethanol: 0.78 78.4 1.22 –114.6 –1.99 ... Water: 100.00 0.512 0.00
This page contains tables of azeotrope data for various binary and ternary mixtures of solvents. The data include the composition of a mixture by weight (in binary azeotropes, when only one fraction is given, it is the fraction of the second component), the boiling point (b.p.) of a component, the boiling point of a mixture, and the specific gravity of the mixture.
At atmospheric pressure, mixtures of ethanol and water form an azeotrope at about 89.4 mol% ethanol (95.6% ethanol by mass, [83] 97% alcohol by volume), with a boiling point of 351.3 K (78.1 °C). [84] At lower pressure, the composition of the ethanol-water azeotrope shifts to more ethanol-rich mixtures. [85]
Old thermometer in a pharmacy in Vienna, showing room temperature by Reaumur scale. Réaumur and Celsius scale on thermometer. Private collection, central Europe. The Réaumur scale (French pronunciation: [ʁeomy(ː)ʁ]; °Ré, °Re, °r), also known as the "octogesimal division", [1] is a temperature scale for which the melting and boiling points of water are defined as 0 and 80 degrees ...
Ethanol-filled thermometer are used in preference to mercury for meteorological measurements of minimum temperatures and can be used down to −70 °C (−94 °F). [2] The physical limitation of the ability of a thermometer to measure low temperature is the freezing point of the liquid used. Ethanol freezes at −114.9 °C (−174.82 °F).
Owing to the presence of the polar OH alcohols are more water-soluble than simple hydrocarbons. Methanol, ethanol, and propanol are miscible in water. 1-Butanol, with a four-carbon chain, is moderately soluble. Because of hydrogen bonding, alcohols tend to have higher boiling points than comparable hydrocarbons and ethers.
It competitively inhibits alcohol dehydrogenase for example. [5] TFE forms complexes with Lewis bases such as THF or pyridine through hydrogen bonding, yielding 1:1 adducts. [6] It is classified as a hard Lewis acid and its acceptor properties are discussed in the ECW model yielding E A = 2.07 and C A = 1.06.