scholarly journals Kinetics of Oxidation of L-Leucine by Mono- and Bimetallic Gold and Silver Nanoparticles in Hydrogen Peroxide Solution

2012 ◽  
Vol 33 (7-8) ◽  
pp. 1306-1311 ◽  
Author(s):  
P. VENKATESAN ◽  
J. SANTHANALAKSHMI
Keyword(s):  
Hydrogen Peroxide ◽  
Silver Nanoparticles ◽  
Hydrogen Peroxide Solution ◽  
Gold And Silver Nanoparticles ◽  
Kinetics Of Oxidation ◽  
Kinetics Of

Chemical Modification of Surfaces and the Kinetics of Oxidation of Aqueous Salts of Silver Nanoparticles

2021 ◽  
Vol 95 (1) ◽  
pp. 177-182
Author(s):  
A. Yu. Olenin ◽  
A. S. Korotkov ◽  
V. V. Yagov ◽  
G. V. Lisichkin
Keyword(s):  
Silver Nanoparticles ◽  
Chemical Modification ◽  
Kinetics Of Oxidation ◽  
Kinetics Of

Porphyrin macrocycle-stabilized gold and silver nanoparticles and their application in catalysis of hydrogen peroxide

2015 ◽  
Vol 120 ◽  
pp. 155-160 ◽  
Author(s):  
Koodlur Sannegowda Lokesh ◽  
Aralekallu Shambhulinga ◽  
Nemakal Manjunatha ◽  
Mohammed Imadadulla ◽  
Mirabbos Hojamberdiev
Keyword(s):  
Hydrogen Peroxide ◽  
Silver Nanoparticles ◽  
Gold And Silver Nanoparticles ◽  
Porphyrin Macrocycle

Kinetics and mechanism of oxidation of iodide ion by the molybdenum (VI) – hydrogen peroxide system

1990 ◽  
Vol 68 (9) ◽  
pp. 1499-1503 ◽  
Author(s):  
Conchita Arias ◽  
Fernando Mata ◽  
Joaquin F. Perez-Benito
Keyword(s):  
Hydrogen Peroxide ◽  
Rate Constants ◽  
Reaction Rate ◽  
Sodium Molybdate ◽  
Initial Reaction Rate ◽  
Initial Reaction ◽  
Kinetics Of Oxidation ◽  
Iodide Ion ◽  
Aqueous Perchloric Acid ◽  
Kinetics Of

The kinetics of oxidation of potassium iodide by hydrogen peroxide in aqueous perchloric acid has been studied both in the absence and in the presence of sodium molybdate by means of the initial-rates method. The law found for the total initial reaction rate is[Formula: see text]The activation energies associated with rate constants k1, k2, and k3 are 52 ± 1, 49 ± 1, and 42 ± 3 kJ mol−1, respectively. A mechanism in agreement with the experimental kinetic data is proposed, according to which rate constants k1, k2, and k3 correspond to the oxidations of iodide ion by H2O2, H3O2+ and H2MoO5, respectively. Keywords: catalysis, hydrogen peroxide, iodide ion, kinetics, molybdate ion.

Kinetics of oxidation of o-dianisidine by hydrogen peroxide in the presence of antibody complexes of iron(III) coproporphyrin

1994 ◽  
Vol 47 (2-3) ◽  
pp. 317-327 ◽  
Author(s):  
Alexander P. Savitsky ◽  
Mary I. Nelen ◽  
Anatoly K. Yatsmirsky ◽  
Mary V. Demcheva ◽  
Gely V. Ponomarev ◽  
...  
Keyword(s):  
Hydrogen Peroxide ◽  
Kinetics Of Oxidation ◽  
Kinetics Of

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

2008 ◽  
Vol 5 (1) ◽  
pp. 43-51 ◽  
Author(s):  
Mansur Ahmed ◽  
K. Subramani
Keyword(s):  
Hydrogen Peroxide ◽  
Electron Transfer ◽  
Bond Cleavage ◽  
Micellar Medium ◽  
Hydroxy Acids ◽  
Peroxide Oxidation ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
First Order Kinetics ◽  
Kinetics Of

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.

Oxywater-oxenoid conception of mechanisms of benzylpenicillin oxidation and oxidant decomposition in aqueous hydrogen peroxide solution

1970 ◽  
Author(s):  
Anton A. Chumakov ◽  
Oleg A. Kotelnikov ◽  
Yurij G. Slizhov ◽  
Tamara S. Minakova
Keyword(s):  
Hydrogen Peroxide ◽  
Oxygen Atom ◽  
Singlet Oxygen ◽  
Aromatic Ring ◽  
Hydrogen Peroxide Solution ◽  
Colloid Solution ◽  
Spin Moment ◽  
Aqueous Hydrogen Peroxide ◽  
True Nature ◽  
Kinetics Of

There are actuality and importance of confirmation or at least reasoned argumentation of molecular kinetics of hydrogen peroxide oxidation reactions because of currently unidentified true nature of oxygen intermediates, at one side, and widespread of these processes in natural biological and artificial anthropogenic systems, from other side. The building of common theory of hydrogen peroxide oxidative activity and dismutation decomposition can be based on determination of structure of individual model reactions products. The benzylpenicillin molecule has a heterofunctional structure. Its sodium salt was dissolved in aqueous hydrogen peroxide solution without Fenton catalysts addition. The system was protected from thermal and photochemical activation. As result, we observed a colloid solution formation, a water-insoluble sediment accumulation, and a hydrogen peroxide disproportionation with gas-phase molecular oxygen liberation. The NMR-spectroscopy data evidenced in favor of S-oxidation of sulfide fragment, N-oxidation of nitrogen atoms with amide groups dissociation, and aromatic ring hydroxylation and electrophilic carbonylation. The precipitate is a mixture of several substances, some of which have presumably an oligomeric structure due to neighboring molecules coupling in carbonylation and hydroxylamine fragments O-acylation reactions. The molecular kinetics of model organic molecule oxidative modifications and hydrogen peroxide dismutation is interpreted by oxywater-oxenoid conception. In accordance with one, there are different associates between water HOH and hydrogen peroxide HOOH molecules in solution system due to hydrogen bonds. These molecules are simultaneously Brønsted acids and bases. The rate of proton accepting and donation depends on temperature and concentration parameters. The hydronium H3O+ and hydroperoxonium H3O2+ cations, and the hydroxide HO− and hydroperoxide HO2− anions are generated. For hydrogen peroxide molecule H2O2, there is possibility for isomeric bipolar ion oxywater H2O+O− formation. The zwitter-ion heterolytically dissociates with water molecule liberation and singlet oxygen atom generation. The 1D-oxene (2p[↑↓][↑↓][_]) oxidizes sulfur and nitrogen heteroatoms through accepting their unshared electron pairs by own vacant atomic orbital. In addition, singlet oxygen atom hydroxylates an aromatic ring by hydride transfer and mediates decomposition of hydrogen peroxide. The dioxygen liberated during hydrogen peroxide dismutation is generated at first in singlet 1∆g-quantum state, the quenching of which, presumably, includes a dimerization of 1O2 antipodes by orbital moment. Inside the associate (1O2)2, the electron exchange interaction occurs. As result, two molecules of triplet dioxygen are generated, and they are antipodes by spin moment: first molecule has spin +1 and second molecule has spin −1.

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