Identification of the product from the reduction of permanganate ion by trimethylamine in aqueous phosphate buffers

Mata-Pérez, Fernando; Perez‐Benito, Joaquin F.

doi:10.1139/v85-165

Cited by 65 publications

(42 citation statements)

References 16 publications

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“…The integral form of eq. [2] is This equation was successfully used for the kinetic study of the permanganate ion oxidation of dimethylamine (3) and trimethylamine (2) and was also proposed for the acid-catalyzed hydrolysis of esters (44).…”

Section: Resultsmentioning

confidence: 99%

“…[ l ] and [2] The values of the rate constants corresponding to different methylammonium ion concentrations have been determined. We can see in Fig.…”

Section: Resultsmentioning

confidence: 99%

“…Although some kinetic studies on the permanganate ion oxidation of tertiary (1,2) and secondary (3)amines have been reported, little attention has been paid to the kinetic aspects of the oxidation of primary amines by permanganate ion, save for the case of benzylamine (4). On the other hand, the products from the oxidation of a wide variety of amines by permanganate ion are known (5)(6)(7).…”

Section: Introductionmentioning

confidence: 99%

“…Autocatalysis seems to be a rather general phenomenon for the oxidation of amines by permanganate ion (2)(3)(4)8), but is by no means limited to amines, for many permanganate reactions have been found to be autocatalytic (9)(10)(11)(12)(13)(14)(15)(16)(17)(18)(19)(20)(21)(22)(23)(24)(25)(26)(27).…”

Section: Introductionmentioning

confidence: 99%

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Kinetics and mechanisms of oxidation of methylamine by permanganate ion

Mata-Pérez¹,

Perez‐Benito²

1987

Can. J. Chem.

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. Can. J. Chem. 65, 2373 (1987). The oxidation of methylamine by permanganate ion in aqueous phosphate buffers is autocatalyzed by a soluble form of colloidal manganese dioxide temporarily stabilized in solution by adsorption of phosphate ions on its surface. The dependence of the rate constants of both the noncatalytic and catalytic mechanisms on the concentrations of both methylammonium and hydroxyl ions and on temperature has been determined. The activation parameters have been obtained. Mechanisms in agreement with the experimental data are proposed.FERNANDO MATA-PEREZ et JOAQUIN F. PEREZ-BENITO. Can. J. Chem. 65, 2373 (1987). L'oxydation de la mithylamine par l'ion permanganate, en solution dans des tampons de phosphates, est autocatalyste par une forme soluble du bioxyde de manganese colloidal qui est temporairement stabiliste en solution par adsorption des ions phosphates sur sa surface. On a dttermini les relations qui existent entre les constantes de vitesse, tant des micanismes catalysis que ceux des mtcanismes non-catalysts, et soit les concentrations tant des ions mithylammonium que des ions hydroxyles soit la temptrature. On a obtenu les paramttres d'activation. On propose des micanismes qui sont en accord avec les donntes expirimentales.[Traduit par la revue]

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Section: Resultsmentioning

confidence: 99%

“…[ l ] and [2] The values of the rate constants corresponding to different methylammonium ion concentrations have been determined. We can see in Fig.…”

Section: Resultsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

See 2 more Smart Citations

Kinetics and mechanisms of oxidation of methylamine by permanganate ion

Mata-Pérez¹,

Perez‐Benito²

1987

Can. J. Chem.

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“…This has given rise to the use of stabilization aids. Mata-Perez and PerezBenito [28] found that the conversion rate of soluble Mn(IV) to MnO 2 (s) could be delayed when phosphate was present. Kao et al [29] found that ~82% of MnO 2 production could be inhibited by including Na 2 HPO 4 with MnO 4 − without affecting TCE loss.…”

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confidence: 99%

Improving the treatment of non-aqueous phase TCE in low permeability zones with permanganate

Chokejaroenrat

Comfort²,

Sakulthaew

et al. 2014

Journal of Hazardous Materials

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A kinetic study of the enhancement of solution chemiluminescence of glyoxylic acid oxidation by manganese species

et al. 2014

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In order to study the mechanism of the enhancement of solution chemiluminescence, the kinetics of the decay of the oxidant and the chemiluminescence emission were followed for oxidations by permanganate, manganese dioxide sol and Mn(3+) (aq) of glyoxylic acid, using stopped-flow spectrophotometry. Results are reported for the glyoxylic acid oxidized under pseudo first-order conditions and in an acidic medium at 25 °C. For permanganate under these conditions, the decay is sigmoidal, consistent with autocatalysis, and for manganese dioxide sol and Mn(3+) it is pseudo first order. The effects of the presence of aqueous formaldehyde and Mn(2+) were observed and a fit to a simple mechanism is discussed. It is concluded that chemiluminescent enhancement in these systems is best explained by reaction kinetics.

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Identification of the product from the reduction of permanganate ion by trimethylamine in aqueous phosphate buffers

Cited by 65 publications

References 16 publications

Kinetics and mechanisms of oxidation of methylamine by permanganate ion

Kinetics and mechanisms of oxidation of methylamine by permanganate ion

Improving the treatment of non-aqueous phase TCE in low permeability zones with permanganate

A kinetic study of the enhancement of solution chemiluminescence of glyoxylic acid oxidation by manganese species

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