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The epoxidation can take place either in a homogeneous reaction by peracids [2] or heterogeneous catalysis (e.g. silver and molecular oxygen). [ 3 ] [ 4 ] [ 5 ] In industrial production the heterogeneously catalyzed synthesis is preferred because of better atom economy , a simpler separation of the product and easier recycling of catalyst.
Aliquat 336 is used as a phase transfer catalyst, [2] including in the catalytic oxidation of cyclohexene to 1,6-hexanedioic acid. [3] This reaction is an example of green chemistry, as it is more environmentally friendly than the traditional method of oxidizing cyclohexanol or cyclohexanone with nitric acid or potassium permanganate, which produce hazardous wastes.
3 K 2 MnO 4 + 4 HCl → 2 KMnO 4 + MnO 2 + 2 H 2 O + 4 KCl. A weak acid such as carbonic acid is sufficient for this reaction: 3 K 2 MnO 4 + 2 CO 2 → 2 KMnO 4 + 2 K 2 CO 3 + MnO 2. Permanganate salts may also be generated by treating a solution of Mn 2+ ions with strong oxidants such as lead dioxide (PbO 2), sodium bismuthate (NaBiO 3), or ...
Cyclohexene is produced by the partial hydrogenation of benzene, a process developed by the Asahi Chemical company. [4] The main product of the process is cyclohexane because cyclohexene is more easily hydrogenated than benzene. In the laboratory, it can be prepared by dehydration of cyclohexanol. [5] C 6 H 11 OH → C 6 H 10 + H 2 O
Oxidation of 1-methylcyclohexene catalyzed by cytochrome P450 yields a 2:1 mixture of hydroxylation to epoxidation products. [4] The stereochemistry of hydroformylation has been examined using 1-methylcyclohexene. The main product has the formyl group on the less substituted alkene-carbon, trans with respect to the methyl substituent. [5]
A catalyst is a substance that alters the rate of a chemical reaction but it remains chemically unchanged afterwards. The catalyst increases the rate of the reaction by providing a new reaction mechanism to occur with in a lower activation energy. In autocatalysis a reaction product is itself a catalyst for that reaction leading to positive ...
The turnover-limiting step of the reaction is the hydrolysis step; therefore, sulfuric acid is added to increase the rate of this step. [ 17 ] [ 18 ] Manganese is also used in dihydroxylation and is often chosen when osmium tetroxide methods yield poor results. [ 18 ]
Both the oxidation and reduction steps are pH dependent. Figure 1 shows the standard potentials at pH 0 (strongly acidic) as referenced to the normal hydrogen electrode (NHE). 2 half reactions (at pH = 0) Oxidation 2H 2 O → 4H + + 4e − + O 2 E° = +1.23 V vs. NHE Reduction 4H + + 4e − → 2H 2 E° = 0.00 V vs. NHE