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Isopropyl alcohol (IUPAC name propan-2-ol and also called isopropanol or 2-propanol) is a colorless, flammable, organic compound with a pungent alcoholic odor. [9]Isopropyl alcohol, an organic polar molecule, is miscible in water, ethanol, and chloroform, demonstrating its ability to dissolve a wide range of substances including ethyl cellulose, polyvinyl butyral, oils, alkaloids, and natural ...
Isobutanol (IUPAC nomenclature: 2-methylpropan-1-ol) is an organic compound with the formula (CH 3) 2 CHCH 2 OH (sometimes represented as i-BuOH).This colorless, flammable liquid with a characteristic smell is mainly used as a solvent either directly or as its esters.
The attractive force draws molecules closer together and gives a real gas a tendency to occupy a smaller volume than an ideal gas. Which interaction is more important depends on temperature and pressure (see compressibility factor). In a gas, the distances between molecules are generally large, so intermolecular forces have only a small effect.
Three of these alcohols, 2-methyl-1-butanol, 2-pentanol, and 3-methyl-2-butanol (methyl isopropyl carbinol), contain stereocenters, and are therefore chiral and optically active. The most important amyl alcohol is isoamyl alcohol , the chief one generated by fermentation in the production of alcoholic beverages and a constituent of fusel oil .
Nitrogen trifluoride [2] 3.58 0.0545 Nitrous oxide: 3.832 0.04415 Octane [2] 37.88 0.2374 1-Octanol [2] 44.71 0.2442 Oxygen: 1.382 0.03186 Ozone [2] 3.570 0.0487 Pentane: 19.26 0.146 1-Pentanol [2] 25.88 0.1568 Phenol [2] 22.93 0.1177 Phosphine: 4.692 0.05156 Propane: 8.779 0.08445 1-Propanol [2] 16.26 0.1079 2-Propanol [2] 15.82 0.1109 Propene ...
Enthalpy of mixing can often be ignored in calculations for mixtures where other heat terms exist, or in cases where the mixture is ideal. [2] The sign convention is the same as for enthalpy of reaction: when the enthalpy of mixing is positive, mixing is endothermic, while negative enthalpy of mixing signifies exothermic mixing. In ideal ...
For example, ethane (C 2 H 6), has a higher boiling point than methane (CH 4). This is because the London dispersion forces between ethane molecules are higher than that between methane molecules, resulting in stronger forces of intermolecular attraction, raising the boiling point.
2.3703 mPa·s at 20°C 1.3311 mPa·s at 40°C Thermodynamic properties. Phase behavior Triple point: 184.9 K (−88.2 °C), ? Pa Critical point: