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2.79 6.55 –20.2 Diethyl ether: 0.713 34.5 2.16 –116.3 –1.79 K b & K f [1] Methanol [4] 0.79 64.7 Ethanol: 0.78 78.4 1.22 –114.6 –1.99 K b [2] Ethylene bromide: 2.18 133 6.43 9.974 –12.5 K b & K f [1] Ethylene glycol: 1.11 197.3 2.26 −12.9 –3.11 K b & K f [1] Formic acid: 101.0 2.4 8.0 –2.77 K b & K f [1] Naphthalene: 217.9 78. ...
log 10 of Acetonitrile vapor pressure. Uses formula log e P m m H g = {\displaystyle \scriptstyle \log _{e}P_{mmHg}=} log e ( 760 101.325 ) − 3.881710 log e ( T + 273.15 ) − 4999.618 T + 273.15 + 41.05901 + 3.515956 × 10 − 06 ( T + 273.15 ) 2 {\displaystyle \scriptstyle \log _{e}({\frac {760}{101.325}})-3.881710\log _{e}(T+ ...
methanol: 67-56-1 CH 3 N(C 2 H 4 OH) 2: methyl diethanolamine: 105-59-9 CH 3 NC: methyl isocyanide: 593-75-9 C 5 H 9 NO: N-Methyl-2-pyrrolidone: 872-50-4 CH 3 CH 2 CH 2 OH: 1-Propanol: 71-23-8 CH 2 (CH 2 OH) 2: 1,3-Propanediol: 504-63-2 HOCH 2 CH 2 CH 2 CH 2 CH 2 OH: 1,5-Pentanediol: 111-29-5 (CH 3) 2 CHOH: 2-Propanol: 67-63-0 CH 3 CH 2 COOH ...
A solvent is usually a liquid but can also be a solid, a gas, or a supercritical fluid. Water is a solvent for polar molecules, and the most common solvent used by living things; all the ions and proteins in a cell are dissolved in water within the cell. Major uses of solvents are in paints, paint removers, inks, and dry cleaning. [2]
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.
Acetonitrile is used mainly as a solvent in the purification of butadiene in refineries. Specifically, acetonitrile is fed into the top of a distillation column filled with hydrocarbons including butadiene, and as the acetonitrile falls down through the column, it absorbs the butadiene which is then sent from the bottom of the tower to a second separating tower.
The following table lists the Van der Waals constants (from the Van der Waals equation) for a number of common gases and volatile liquids. [ 1 ] To convert from L 2 b a r / m o l 2 {\displaystyle \mathrm {L^{2}bar/mol^{2}} } to L 2 k P a / m o l 2 {\displaystyle \mathrm {L^{2}kPa/mol^{2}} } , multiply by 100.
Here is a similar formula from the 67th edition of the CRC handbook. Note that the form of this formula as given is a fit to the Clausius–Clapeyron equation, which is a good theoretical starting point for calculating saturation vapor pressures: