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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
The minimum-pressure azeotrope has an ethanol fraction of 100% [86] and a boiling point of 306 K (33 °C), [85] corresponding to a pressure of roughly 70 torr (9.333 kPa). [87] Below this pressure, there is no azeotrope, and it is possible to distill absolute ethanol from an ethanol-water mixture.
8 Boiling points of aqueous solutions. 9 Charts. 10 References. Toggle the table of contents. ... Solid–liquid equilibrium of the mixture of ethanol and water ...
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.
The rule, however, has some exceptions. For example, the entropies of vaporization of water, ethanol, formic acid and hydrogen fluoride are far from the predicted values. The entropy of vaporization of XeF 6 at its boiling point has the extraordinarily high value of 136.9 J/(K·mol). [4]
Values are in kelvin K and degrees Celsius °C, rounded For the equivalent in degrees Fahrenheit °F, see: Boiling points of the elements (data page) Some values are predictions
T b is boiling point of the pure solvent in kelvin. ΔH vap is the molar enthalpy of vaporization of the solvent. Through the procedure called ebullioscopy, a known constant can be used to calculate an unknown molar mass. The term ebullioscopy means "boiling measurement" in Latin.
Water boiling at 99.3 °C (210.8 °F) at 215 m (705 ft) elevation. The boiling point of a substance is the temperature at which the vapor pressure of a liquid equals the pressure surrounding the liquid [1] [2] and the liquid changes into a vapor. The boiling point of a liquid varies depending upon the surrounding environmental pressure.