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Boiling point (°C) K b (°C⋅kg/mol) Freezing point (°C) K f (°C⋅kg/mol) Data source; Aniline: 184.3 3.69 –5.96 –5.87 K b & K f [1] Lauric acid: 298.9 44 –3.9 Acetic acid: 1.04 117.9 3.14 16.6 –3.90 K b [1] K f [2] Acetone: 0.78 56.2 1.67 –94.8 K b [3] Benzene: 0.87 80.1 2.65 5.5 –5.12 K b & K f [2] Bromobenzene: 1.49 156.0 6. ...
Flaxseed oil: Unrefined: 107 °C: 225 °F [3] Grape seed oil: 216 °C: 421 °F Lard: 190 °C: 374 °F [5] Mustard oil: 250 °C: 480 °F [11] Olive oil: Refined: 199–243 °C: 390–470 °F [12] Olive oil: Virgin: 210 °C: 410 °F Olive oil: Extra virgin, low acidity, high quality: 207 °C: 405 °F [3] [13] Olive oil: Extra virgin: 190 °C: 374 ...
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.
This is a list of the various reported boiling points for the elements, with recommended values to be used elsewhere on Wikipedia. ... Kelvin Celsius Fahrenheit; 1 H ...
The difference of temperatures between the freezing- and boiling-points of water under standard atmospheric pressure shall be called 100 degrees. (The same increment as the Celsius scale) Thomson's best estimates at the time were that the temperature of freezing water was 273.7 K and the temperature of boiling water was 373.7 K. [33]
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.
The natural temperature range of Kelvin; 0: N/A: ... Freezing/melting point of fresh water (at 1 atm pressure) ... Melting/freezing point of palm oil [30] 309.5 K:
Boiling-point elevation is the phenomenon whereby the boiling point of a liquid (a solvent) will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent. This happens whenever a non-volatile solute, such as a salt, is added to a pure solvent, such as water.