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Density (g cm-3) Boiling point (°C) K b (°C⋅kg/mol) Freezing point (°C) ... K f [2] K b [1] Water: 100.00 0.512 0.00 –1.86 K b & K f [2] Ethyl Acetate: 77.1 [5 ...
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. ... 211.5 K: −61.7 °C: −79.1 ...
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.
1.199 g mL −1 [2] Melting point: −105.5 °C; −157.8 °F; 167.7 K Boiling point: 105–106 °C; 221–223 °F; 378–379 K ... 1-Bromo-2,2-dimethylpropane, ...
N 1,N 1-Dimethylpropane-1,3-diamine. ... 812 mg mL −1: Boiling point: 132.1 °C; 269.7 °F; 405.2 K log P: ... 1.87 g kg −1 (oral, rat)
N 1,N 3-Dimethylpropane-1,3-diamine. Other names N,N ... Boiling point: 145 °C (293 °F; 418 K) [1] Hazards Flash point: 20 °C (68 °F; 293 K)
The boiling point elevation happens both when the solute is an electrolyte, such as various salts, and a nonelectrolyte. In thermodynamic terms, the origin of the boiling point elevation is entropic and can be explained in terms of the vapor pressure or chemical potential of the solvent. In both cases, the explanation depends on the fact that ...