Propan-2-ol oxidation

The formulation [Ag radical] can be considered as existing in a solvent cage. Oxidation then proceeds when the radical diffuses out of the cage to be further oxidized to acetone by a second mole of Ag . The rate data show that the oxidative reactivity of AgOH+ towards propan-2-ol is much less than that of Ag +. Comparison of activation parameters with those for propan-2-ol oxidations by other oxidants reveals no relation to the standard redox potential. 

Due to atmospheric oxidation it is common for commercial propan-2-ol to contain a small amount of acetone. 

V sol in acetic acid, ethanol and w. Prepn is by dehydration of propan-2-ol over Al oxide at 330°. It is also obtd as a pyrolysis product of propane and as a fraction of petr well head gases Propene has a Qc of 460.47kcal/mole the expln limits with air are 2.0 to 11.1% (Ref 2) it has an autoign temp of 927°F. Under unusual conditions, such as 955 atms press and... 

A similar system based on rhodium has been studied (123) and was found to be less active than the equivalent iridium catalysts. Selective hydrogenation of acetylenes to olefins and dienes to monoolefins can be performed using the rhodium system, and the authors note that although propan-2-ol is an effective source of hydrogen (via oxidation to acetone), mild pressures of hydrogen gas can also be employed. 

Hafifad, D. Chambellan, A. Lavalley, J.C. Propan-2-ol transformation on simple metal oxides Ti02, Zr02 and Ce02. J. Mol. Catal. A Chem. 2001,168,153-164. 

The reaction medium was extracted with an equal volume of diethyl ether (1 mL), evaporated, diluted to original volume with propan-2-ol (1 mL) and analysed by chiral HPLC (Chiralcel OD column rate flow 1 mL min 2 254 nm for ( )-l n-hexane/ propan-2-ol, 90/10 for ( )-2 -hexane/propan-2-ol, 95/5 for ( )-3 n-hexane/propan-2-ol, 90/10) in order to evaluate the degree of oxidation and the enantiomeric excess. 

Tu. C. H., Hsian. H. Y., Chou. Y. T., and Wang, W.-F. Vapor-liquid equilibria of methanol, ethanol, propan-2-ol, and 2-methylpropan-2-ol with a five-component hydrocarbon mixtrue at 101.3 kPa,/. Chem. Eng. Data, 46(5) 1239-1243, 2001. Tu. C.M. Influence of pesticides and some of the oxidized analogues on microbial populations, nitrification and respiration activities in soil. Bull Environ. Contam. Toxicol, 24(1) 13-19, 1980. 

Table 8 Representative kinetic data for the oxidation of propan-2-ol by ruthenium oxo complexes.

Following oral administration of 50 mg/kg bw 2,3-dibromopropan-l-ol to male Sprague-Dawley rats, two urinary mercapturic acid metabolites were identified as N-acetyl-5 -(2,3-dihydroxypropyl)cysteine and A, W-bis-acetyl-N<5"-(l,3-bis-cysteinyl)-propan-2-ol, respectively. It was inferred that 3-bromo-l,2-propane epoxide is an intermediate in the metabolism of 2,3-dibromopropan-l-ol. In addition, (3-bromolactate was produced, presumably as a result of hydrolysis to the a-bromohydrin and subsequent oxidation (Jones Fakhouri, 1979). Marsden and Casida (1982) identified small amounts of 2-bromoacrylic acid in the urine of rats injected intraperitoneally with 2,3-dibromopropan-l-ol and suggested that this arose by oxidation and dehydrobromi-nation, with 2-bromoacrolein as an unstable intermediate. 

Chemoselective reduction of conjugated enones to allylic alcohols via hydrogen transfer from propan-2-ol over metal oxides is investigated in vapour phase conditions. The unique ability of Mgo to reduce exclusively carbonyl group is observed. However, because of the high basicity of MgO side reactions are present. It is shown that by doping the Mgo catalyst with HC1 a significant decrease of its basicity occurs and consequently side reactions are minimized. 

Solid sodamide and potassium metal. Both of these substances undergo surface oxidation to give oxide films which may initiate explosions when the samples are handled. In the case of potassium, surface oxidation occurs even when the metal is stored under oil, and the act of paring off the oxide film with a knife may initiate an explosion. Samples of potassium which are heavily encrusted with oxide should not be used but should be carefully destroyed by adding the lumps to a large excess of propan-2-ol. Similarly, old or obviously encrusted (yellow) lumps of sodamide (Section 4.2.67) should not be ground in a pestle and mortar, but should be destroyed by mixing with solid ammonium chloride. 

Sodium residues. Bottles containing sodium wire previously used for solvent drying constitute a fire and explosion hazard. The sodium, sometimes heavily coated with hydroxide or oxide film, should be covered with propan-2-ol and set aside with occasional swirling until all the sodium particles are destroyed (at least 2 hours). The contents of the bottle should then be poured into a large excess of water (water should not be added to the bottle) and the bottle washed out several times with industrial spirit. Only then can the bottle be safely rinsed with water. 

The major products of the photolysis of glycolaldehyde are HCHO and CO, methanol and OH production was also observed. Photolysis of glycolaldehyde was used as the OH source to measure the reaction rate constants of OH with a series of dienes by the relative method and to identify and quantify the oxidation products of the OH-initiated oxidation of propan-2-ol. HCHO is observed to be the major product of the OH-initiated oxidation of glycolaldehyde. The results indicate that the OH reaction and photolysis can compete as tropospheric sinks for glycolaldehyde.218... 

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