Cinétique d'oxydation des oximes du benzaldéhyde et de l'acétophénone par l'ion thallique

1980 ◽  
Vol 58 (13) ◽  
pp. 1305-1310 ◽  
Author(s):  
Robert Lortie ◽  
Miklos Zador
Keyword(s):  
Reaction Mechanism ◽  
Aqueous Medium ◽  
Rate Equation ◽  
Chloride Ions ◽  
Kinetics Of Oxidation ◽  
Kinetics Of

The kinetics of oxidation of benzaldehyde and acetophenone oximes by Tl(III) in aqueous medium has been studied. The reaction occurs in two consecutive steps: formation of a nitroso intermediate and its decomposition. The oxime forms a complex with Tl(III) leading to the rate equation: −d[oxime]/dt = K1/k2[oxime][Tl(III)]/(1 + K1[Tl(III)]). The formation of the final carbonyl product is inhibited by Tl(III), a resuit of the formation of a complex resistant to decomposition. Coordination of Tl(III) by chloride ions affects the rate of the above two steps. The reaction mechanism is discussed. [Journal translation]

THE REDUCTION OF CYTOCHROMEcBY HYDROQUINONE

1963 ◽  
Vol 41 (1) ◽  
pp. 231-237 ◽  
Author(s):  
G. R. Williams
Keyword(s):  
Reaction Mechanism ◽  
Ionic Strength ◽  
Rate Equation ◽  
Second Order ◽  
Order Rate ◽  
Ferricytochrome C ◽  
Kinetics Of ◽  
Kinetics Of Reduction ◽  
Order Rate Equation

The kinetics of reduction of ferricytochrome c by hydroquinone have been studied. The reaction does not conform to a simple second-order rate equation and it is demonstrated that the deviations are brought about by the presence of p-quinone, one of the products of the reaction. The accelerating effect of p-quinone is explained tentatively on the basis of an involvement of the semi-quinone. The effects on the reaction of pH, ionic strength, and temperature are reported and used to suggest features of the reaction mechanism.

Kinetics of oxidation of reduced cytochrome c by aquacopper(II) and chlorocopper(II) complexes in the presence of oxygen

1981 ◽  
Vol 34 (1) ◽  
pp. 99 ◽  
Author(s):  
JK Yandell
Keyword(s):  
Reaction Mechanism ◽  
Ionic Strength ◽  
Cytochrome C ◽  
Rate Constants ◽  
Kinetics Of Oxidation ◽  
Ferrocytochrome C ◽  
Kinetics Of

The rate constants for the oxidation of reduced cytochrome c by aquacopper(II) ion, aquachloro- copper(II) ion and aquadichlorocopper(II) were found to be 5.7�0.3 1. mol-1 s-1, 2.3×102 1. mol-1 s-1 and 5.6xl031. mol-1 s-1 respectively at 25�C, ionic strength 0.1 and pH 4.0. At low ratios of aquacopper(II) ion to ferrocytochrome c, when oxygen is required to completely oxidize the cytochrome, the reaction mechanism was found to be complex. No evidence for the involvement of copper bound to the cytochrome was found.

THE REDUCTION OF CYTOCHROMEcBY HYDROQUINONE

1963 ◽  
Vol 41 (1) ◽  
pp. 231-237 ◽  
Author(s):  
G. R. Williams
Keyword(s):  
Reaction Mechanism ◽  
Ionic Strength ◽  
Rate Equation ◽  
Second Order ◽  
Order Rate ◽  
Ferricytochrome C ◽  
Kinetics Of ◽  
Kinetics Of Reduction ◽  
Order Rate Equation

The kinetics of reduction of ferricytochrome c by hydroquinone have been studied. The reaction does not conform to a simple second-order rate equation and it is demonstrated that the deviations are brought about by the presence of p-quinone, one of the products of the reaction. The accelerating effect of p-quinone is explained tentatively on the basis of an involvement of the semi-quinone. The effects on the reaction of pH, ionic strength, and temperature are reported and used to suggest features of the reaction mechanism.

scholarly journals Kinetics of Oxidation of Tryptophan by Sodium Hypochlorite

1981 ◽  
Vol 36 (3) ◽  
pp. 359-361 ◽  
Author(s):  
Thomas Rausch ◽  
Frieder Hofmann ◽  
Willy Hilgenberg
Keyword(s):  
Activation Energy ◽  
Reaction Mechanism ◽  
Sodium Hypochlorite ◽  
Arrhenius Plot ◽  
Ph Dependence ◽  
Order Conditions ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Pseudo First Order ◽  
Kinetics Of

AbstractThe oxidation of tryptophan to 3-indoleacetaldehyde with sodium hypochlorite was investigated with 14C labelled DL-tryptophan. The reaction was performed under pseudo first order conditions. From the pH dependence of the reaction it was concluded that only the unprotonated tryptophan is converted to the aldehyde. The activation energy is 35 ± 2.2 (SE) kJ x mol-1 as derived from the Arrhenius plot. Variing the pH between 8.5 and 11.0 and the temperature in the range from 298 K to 318 K did not alter the selectivity of the reaction as confirmed by TLC of the product (purity ≧ 90%). A possible reaction mechanism is proposed.

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

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.

Kinetics of oxidation of bivalent iron by chlorate

1979 ◽  
Vol 44 (9) ◽  
pp. 2760-2768 ◽  
Author(s):  
Karel Mádlo
Keyword(s):  
Rate Equation ◽  
Heterogeneous Systems ◽  
Time Interval ◽  
Kinetics Of Oxidation ◽  
Homogeneous Systems ◽  
Spontaneous Change ◽  
Hydrolysis Products ◽  
Constant Ph ◽  
Bivalent Iron ◽  
Kinetics Of

Kinetics of Fe(II) oxidation by chlorate was studied in homogeneous systems (pH 1, HCLO4 and in heterogeneous systems involving precipitate of Fe(III) hydrolysis products (pH 1 to 5.5). The stoichiometry ( 6 Fe2+ : 1 ClO-3 : 6H+) as well as the rate equation (-d[Fe2+]/dt = kexp/.[Fe2+][ClO-3]) is the same in the two cases. Also the differences in the experimental activation energies and entropies for the two pH regions are insignificant. The [OH-]/[Fe3+] ratio passes a maximum during the spontaneous change of pH (pH0 5), whereas if the pH is maintained constant (pH 5) the ratio increases monotonically throughout the whole time interval followed. The balance of the Fe2+ and Fe3+ showed that part of the Fe2+ ( 10-3 mol l-1) was present during the reaction in the precipitate of the Fe(III) hydrolysis products, while part of the Fe3+ (5 . 10-3 mol l-1) existed outside this precipitate; the latter dropped by approximately two orders of magnitude only several tens of hours after the finishing of the Fe(II) oxidation.

Kinetics of oxidation of an arabinogalactan from larch (Larix sibirica L.) in an aqueous medium in the presence of hydrogen peroxide

2004 ◽  
Vol 53 (2) ◽  
pp. 318-324 ◽  
Author(s):  
I. M. Borisov ◽  
E. N. Shirokova ◽  
R. Kh. Mudarisova ◽  
R. R. Muslukhov ◽  
Yu. S. Zimin ◽  
...  
Keyword(s):  
Hydrogen Peroxide ◽  
Aqueous Medium ◽  
Larix Sibirica ◽  
Kinetics Of Oxidation ◽  
Kinetics Of

Kinetics of oxidation of trimethylamine by hexacyanoferrate(III) in aqueous medium

1983 ◽  
Vol 23 (3-4) ◽  
pp. 393-395 ◽  
Author(s):  
Gopa Dasgupta ◽  
M. K. Mahanti
Keyword(s):  
Aqueous Medium ◽  
Kinetics Of Oxidation ◽  
Kinetics Of
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