Kinetics of Oxidation of Cobalt(III) Complexes ofaAcids by Hydrogen Peroxide in the Presence of Surfactants

Hydrogen peroxide oxidation of pentaamminecobalt(III) complexes ofα-hydroxy acids at 35°C in micellar medium has been attempted. In this reaction the rate of oxidation shows first order kinetics each in [cobalt(III)] and [H2O2]. Hydrogen peroxide induced electron transfer in [(NH3)5CoIII-L]2+complexes ofα-hydroxy acids readily yields 100% of cobalt(II) with nearly 100% of C-C bond cleavage products suggesting that it behaves mainly as one equivalent oxidant in micellar medium. With unbound ligand also it behaves only as C-C cleavage agent rather than C-H cleavage agent. With increasing micellar concentration an increase in the rate is observed.

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Kinetics and mechanism of the oxidation of mercury by peroxidase

Canadian Journal of Chemistry ◽

10.1139/v85-487 ◽

1985 ◽

Vol 63 (11) ◽

pp. 2940-2944 ◽

Cited By ~ 6

Author(s):

Donald C. Wigfield ◽

Season Tse

Keyword(s):

Hydrogen Peroxide ◽

Electron Transfer ◽

Horseradish Peroxidase ◽

Rate Constant ◽

Order Rate Constant ◽

Kinetics And Mechanism ◽

Kinetics Of Oxidation ◽

First Order ◽

Iron Heme ◽

Kinetics Of

The kinetics of oxidation of zero-valent mercury by the horseradish peroxidase system are reported. The reaction is first order in mercury and first order in peroxidase compound 1, and appear to obey these kinetics to completion of the reaction. The second order rate constant is 8.58 × 105 M−1 min−1 at 23 °C. The data are consistent with a simple two-electron transfer from mercury to the iron–heme system of peroxidase with the enzyme acting as a chemical oxidant that is continually being regenerated by reaction with hydrogen peroxide.

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Kinetics of oxidation of hydrogen peroxide and ascorbic acid by a tribridged manganese(IV,IV) dimer in feebly acidic media

Canadian Journal of Chemistry ◽

10.1139/v99-062 ◽

1999 ◽

Vol 77 (4) ◽

pp. 451-458 ◽

Cited By ~ 3

Author(s):

Anup Kumar Bhattacharya ◽

Anath Bondhu Mondal ◽

Anadi C Dash ◽

G S Brahma ◽

Rupendranath Banerjee

Keyword(s):

Hydrogen Peroxide ◽

Ascorbic Acid ◽

Dehydroascorbic Acid ◽

Kinetics Of Oxidation ◽

First Order ◽

Kinetic Activity ◽

First Order Kinetics ◽

Oxidation Of Hydrogen ◽

Kinetics Of ◽

Complex Ion

In weakly acidic, aqueous buffer (MeCO2-+ bipy), the complex ion [Mn2IV(μ-O)2(μ-MeCO2)(bipy)2(H2O)2]3+, 1 (bipy = 2,2prime-bipyridine), coexists in rapid equilibrium with its hydrolytic derivatives, [Mn2IV(μ-O)2(bipy)2(H2O)4]4+, 2, and [Mn2IV(μ-O)2(μ-MeCO2)(bipy)(H2O)4]3+, 3. The solution quantitatively oxidizes hydrogen peroxide to oxygen and ascorbic acid to dehydroascorbic acid, itself being reduced to MnII. In the presence of excess reductant, the reactions follow simple first-order kinetics with no evidence for the accumulation of a significant amount of any intermediate manganese complex. The ascorbate anion shows overwhelming kinetic dominance over ascorbic acid, but no evidence is available for deprotonation of hydrogen peroxide. The preferred intimate mechanism for hydrogen peroxide is inner sphere but that for ascorbic acid is uncertain. For both reductants, increased extent of aquation leads to increased kinetic activity in the order: 1 < 2 < 3.Key words: kinetics, manganese, ascorbic acid, hydrogen peroxide, 2,2prime-bipyridine.

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KINETICS OF OXIDATION WITH HYDROGEN PEROXIDE AND IRON(II) COMPLEX WITH A MACROCYCLIC BINUCLEATING LIGAND

Southern Brazilian Journal of Chemistry - Southern Brazilian Journal of Chemistry, Volume 28, No. 28, 2020 ◽

10.48141/sbjchem.v3.n3.1995.57_1995.pdf ◽

1995 ◽

Vol 3 (3) ◽

pp. 55-62

Author(s):

Lourdes T. Kist ◽

Bruno Szpoganicz ◽

Manuel G. Basallote ◽

Maria J. F. Trujillo ◽

Maria A. Mariez

Keyword(s):

Hydrogen Peroxide ◽

Macrocyclic Ligand ◽

Kinetic Studies ◽

Organic Substrates ◽

Kinetics Of Oxidation ◽

Oxidation Processes ◽

First Order ◽

First Order Kinetics ◽

Kinetics Of ◽

Catalyzed Oxidation

In the present study solutions of a complex of Fe(II) with a macrocyclic ligand were prepared and their oxidation kinetics with hydrogen peroxide examined. The kinetic studies of the oxidation processes lead to values of rate constant of two-step which occur via first-order kinetics. The results are expected to result in a better knowledge of the mechanism of H202 activation in catalyzed oxidation of organic substrates.

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Kinetics and Mechanism of Oxidation of Dimethyl Sulphoxide by Mono- and Di-Substituted N,N-Dichlorobenzenesulphonamides in Aqueous Acetic Acid

Zeitschrift für Naturforschung B ◽

10.1515/znb-2003-0811 ◽

2003 ◽

Vol 58 (8) ◽

pp. 787-794 ◽

Cited By ~ 3

Author(s):

B.Thimme Gowda ◽

K. L. Jayalakshmi ◽

K. Jyothi

Keyword(s):

Acetic Acid ◽

Benzene Ring ◽

Dimethyl Sulphoxide ◽

Aqueous Acetic Acid ◽

Isokinetic Temperature ◽

Free Energies ◽

Kinetics Of Oxidation ◽

First Order ◽

First Order Kinetics ◽

Kinetics Of

In an effort to introduce N,N-dichloroarylsulphonamides of different oxidising strengths, four mono- and five di-substituted N,N-dichlorobenzenesulphonamides are prepared, characterised and employed as oxidants for studying the kinetics of oxidation of dimethyl sulphoxide (DMSO) in 50% aqueous acetic acid. The reactions show first order kinetics in [oxidant], fractional to first order in [DMSO] and nearly zero order in [H+]. Increase in ionic strength of the medium slightly increases the rates, while decrease in dielectric constant of the medium decreases the rates. The results along with those of the oxidation of DMSO by N,N-dichlorobenzenesulphonamide and N,N-dichloro-4- methylbenzenesulphonamide have been analysed. Effective oxidising species of the oxidants employed in the present oxidations is Cl+ in different forms, released from the oxidants. Therefore the introduction of different substituent groups into the benzene ring of the oxidant is expected to affect the ability of the reagent to release Cl+ and hence its capacity to oxidise the substrate. Significant changes in the kinetic and thermodynamic data are observed in the present investigations with change of substituent in the benzene ring. The electron releasing groups such as CH3 inhibit the ease with which Cl+ is released from the oxidant, while electron-withdrawing groups such as Cl enhance this ability. The Hammett equation, log kobs = −3.19 + 1.05 σ , is found to be valid for oxidations by all the p-substituted N,N-dichlorobenzenesulphonamides. The substituent effect on the energy of activation, Ea and log A for the oxidations is also analysed. The enthalpies and free energies of activation correlate with an isokinetic temperature of 320 K.

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Kinetics of oxidation of the chromium(II) acetate dimer by iodine: an example of mixed zero-order/first-order kinetics

Inorganic Chemistry ◽

10.1021/ic00219a033 ◽

1985 ◽

Vol 24 (25) ◽

pp. 4366-4371 ◽

Cited By ~ 3

Author(s):

Ladislav M. Wilson ◽

Roderick D. Cannon

Keyword(s):

Zero Order ◽

Kinetics Of Oxidation ◽

First Order ◽

First Order Kinetics ◽

Kinetics Of

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Investigations into the kinetics and stoichiometry of bacterial oxidation of covellite (CuS) using a polarographic oxygen probe

Canadian Journal of Microbiology ◽

10.1139/m78-164 ◽

1978 ◽

Vol 24 (8) ◽

pp. 998-1003 ◽

Cited By ~ 5

Author(s):

Pamela A. D. Rickard ◽

Donald G. Vanselow

Keyword(s):

Oxygen Uptake Rate ◽

Zero Order ◽

Bacterial Oxidation ◽

Kinetics Of Oxidation ◽

First Order ◽

Cupric Ion ◽

First Order Kinetics ◽

Zero Order Kinetics ◽

Cupric Sulphate ◽

Kinetics Of

"Oxygraph" apparatus was used to measure quantitatively the kinetics of oxidation of synthetic covellite (CuS) in the presence and absence of Thiobacillus species. The expected stoichiometric relationship between oxygen consumed and cupric sulphate produced was verified by atomic absorption assays of cupric ion and sulphate ion. Thiobacillus cultures markedly increased the oxidation rate.The dependence of each oxygen-uptake rate on oxygen concentration was also measured. Sterile controls and some bacterial cultures showed first-order kinetics while other cultures showed zero-order kinetics.Addition of biological inhibitors to reacting slurries revealed that cultures showing first-order kinetics did not oxidize CuS itself but merely oxidized elemental sulphur formed by non-enzymic oxidation of CuS. Cultures showing zero-order kinetics oxidized CuS in a way that resulted in all oxygen reduction being enzymic. This mechanism possibly involves the cyclic oxidation and reduction of soluble iron.

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Acid Hydrolysis of Bis(2,2'; 6',2''–Terpyridyl) Iron(II) Complex in the Water Pools of CTAB/Hexane/Chloroform Reverse Micelles-A Kinetic Study in Confined Medium

BULLETIN OF CHEMICAL REACTION ENGINEERING AND CATALYSIS ◽

10.9767/bcrec.15.3.8425.853-860 ◽

2020 ◽

Vol 15 (3) ◽

pp. 853-860

Author(s):

K. V. Nagalakshmi ◽

P. Shyamala

Keyword(s):

Ionic Strength ◽

Acid Hydrolysis ◽

Reverse Micelles ◽

Order Rate Constant ◽

Micellar Medium ◽

First Order ◽

First Order Kinetics ◽

Rate Of Reaction ◽

Kinetics Of ◽

Hydrolysis Of

The kinetics of acid hydrolysis of bis(2,2';6',2''–terpyridyl) iron(II) complex has been studied in CTAB/Hexane/Chloroform reverse micelles. The reaction obeys first order kinetics with respect to each of the reactants at all values of W, {W= [H2O]/[CTAB]}. In the reverse micellar medium, the reaction is much slower compared to aqueous medium due to low micropolarity of the water pools which does not facilitate a reaction between reactants of same charge. The effect of variation of W {W=[H2O]/[CTAB]} at constant [CTAB] and variation of [CTAB] at fixed W has been studied. The second order rate constant (k2) of the reaction increases as the value of W increases up to W = 8.88 and remains constant thereafter and it is independent of concentration of [CTAB] at constant W. The variation of rate of reaction with W has been explained by considering variation of micropolarity and ionic strength of water pools of reverse micelles with W. Copyright © 2020 BCREC Group. All rights reserved

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Studies on Kinetics and Mechanism of the Oxidation of Cobalt(Iii) Bound And Unbound Alpha - Hydroxy Acids By Tetramethylammonium Chlorochromate

International Journal of Science Technology and Humanities ◽

10.26524/ijsth57 ◽

2015 ◽

Vol 2 (2) ◽

pp. 64-69

Author(s):

Dayanandhan1.R ◽

Subramani.K

Keyword(s):

Electron Transfer ◽

Hydroxy Acid ◽

Transfer Reaction ◽

Bond Cleavage ◽

Electron Transfer Reaction ◽

Kinetics And Mechanism ◽

Hydroxy Acids ◽

Intermediate Radical ◽

Alpha Hydroxy Acids ◽

Kinetics Of

The kinetics of induced electron transfer reaction has been attempted presently with Tetra Methyl Ammonium Chloro Chromate (TMACC) and pentaammine cobalt (III) complexes of α-hydroxy acid in the presence of micelles. The Tetra Methyl Ammonium Chloro Chromate (TMACC) oxidizes cobalt (III) bound and unbound α-hydroxy acids. In Tetra Methyl Ammonium Chloro Chromate (TMACC) induced electron transfer in the complex, the intermediate radical formed dissociates in a nearly synchronous C-C bond cleavage and the rest of it proceeding with C-H fission yielding cobalt (III) complex. With increase in surfactant Sodium Lauryl Ethersulphate (SLES) concentration, an increase in the rate was observed.

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Oxidation of the mercurous ion by peroxidase

Canadian Journal of Chemistry ◽

10.1139/v86-162 ◽

1986 ◽

Vol 64 (5) ◽

pp. 969-972 ◽

Cited By ~ 1

Author(s):

Donald C. Wigfield ◽

Season Tse

Keyword(s):

Elemental Mercury ◽

Order Rate Constant ◽

Kinetics Of Oxidation ◽

First Order ◽

Order Rate ◽

First Order Kinetics ◽

Cold Vapour ◽

Pseudo First Order ◽

Kinetics Of ◽

Mercurous Ion

The kinetics of oxidation of the mercurous ion by peroxidase have been measured by following the disappearance of mercurous ion using cold-vapour atomic absorption spectroscopy. Pseudo-first-order kinetics are observed with respect to mercurous ion, and the pseudo-first-order rate constants are linearly related to peroxidase concentration, showing first-order dependence on peroxidase. This behaviour is identical to oxidation of elemental mercury, and the second-order rate constant, 1.44 × 104 M−1 s−1 at 23 °C, is also, within experimental error, the same as that for elemental mercury oxidation. The data are interpreted in terms of peroxidase-induced disproportionation of the mercurous dimer, followed by two-electron oxidation of zero-valent mercury.

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Kinetics of Oxidation of Hexakis (P-chloroaniline) Cobalt (II) Chloride by Potassium Iodate

Mapana Journal of Sciences ◽

10.12723/mjs.3.3 ◽

2003 ◽

Vol 2 (1) ◽

pp. 34-38

Author(s):

B. Edison ◽

S. Peter

Keyword(s):

Kinetic Parameters ◽

Aqueous Medium ◽

Neutral Salt ◽

Complex Solution ◽

Potassium Iodate ◽

Kinetics Of Oxidation ◽

First Order ◽

First Order Kinetics ◽

Kinetics Of

Vit B12 is an important complex of cobalt3 . The rate of oxidation of the Synthesized complex Hexakis(p-chloral aniline) cobalt((II) chloride follows first order kinetics with respect to the complex and oxidant potassium iodate1,2,4-8 in aqueous medium. Increasing in the concentration of complex solution increases the rate of the oxidation. The rate of the reaction is studied by changing the acid concentrations of the medium , by changing the temperature and by introducing the neutral salt (NaCl) in the Medium. From this study the kinetic parameters Ea, A,∆S#,∆G#,∆H# are found out. From the observed fats it is inferred that the reaction follows three steps.

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