scholarly journals Kinetics and Mechanism of the Oxidation of Naphthol Green B by Peroxydisulphate Ion in Aqueous Acidic Medium

2014 ◽  
Vol 2014 ◽  
pp. 1-4
Author(s):  
B. Myek ◽  
S. O. Idris ◽  
J. F. Iyun
Keyword(s):  
Acidic Medium ◽  
Reaction Medium ◽  
Intermediate Complex ◽  
Kinetic Investigation ◽  
Hydrogen Ions ◽  
First Order ◽  
Order Dependence ◽  
Naphthol Green B ◽  
Kinetics Of ◽  
Aqueous Acidic Medium

The kinetics of the oxidation of naphthol green B (NGB3−) by peroxydisulphate ion has been carried out in aqueous acidic medium at λmax of 700 nm, T=23±1°C, and I=0.50 mol dm−3 (NaCl). The reaction shows a first-order dependence on oxidant and reductant concentration, respectively. The stoichiometry of the NGB—S2O82- reaction is 1 : 2. Change in hydrogen ions concentration of the reaction medium has no effect on the rate of the reaction. Added cations and anions decreased the rate of the reaction. The results of spectroscopic and kinetic investigation indicate that no intermediate complex is probably formed in the course of this reaction.

scholarly journals Kinetics and Mechanism of Oxidation of Glutamic Acid byN-Bromophthalimide in Aqueous Acidic Medium

2011 ◽  
Vol 8 (4) ◽  
pp. 1472-1477
Author(s):  
N. M. I. Alhaji ◽  
S. Sofiya Lawrence Mary
Keyword(s):  
Dielectric Constant ◽  
Ionic Strength ◽  
Glutamic Acid ◽  
Acidic Medium ◽  
Reaction Medium ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Mechanism Of Oxidation ◽  
Kinetics Of ◽  
Aqueous Acidic Medium

The kinetics of oxidation of glutamic acid (Glu) withN-bromophthalimide (NBP) was studied in perchloric acid medium at 30°C by potentiometric method. The reaction is first order each in NBP and glutamic acid and is negative fractional order in [H+]. Addition of KBr or the reaction product, phthalimide had no effect on the rate. Similarly variation of ionic strength of the medium did not affect the rate of the reaction. Also the rate increased with decrease in dielectric constant of the reaction medium. The thermodynamic parameters were computed from Arrhenius and Eyring plots. A suitable mechanism consistent with the kinetic results has been proposed.

scholarly journals Kinetics of Electron Exchange between Bromopyrogallol Red and Periodate Ion in Aqueous Acidic Medium

2015 ◽  
Vol 2 (2) ◽  
pp. 108-116
Author(s):  
Bako Myek ◽  
S. O Idris ◽  
G.B Adeyemo ◽  
J. F Iyun
Keyword(s):  
Transfer Reaction ◽  
Acidic Solution ◽  
Reaction Medium ◽  
Electron Transfer Reaction ◽  
First Order ◽  
Bromopyrogallol Red ◽  
Mechanistic Pathway ◽  
Oxidant Concentration ◽  
Kinetics Of ◽  
Aqueous Acidic Medium

The kinetics of the electron transfer reaction between Bromopyrogallol (BPR2-) and periodate ion in aqueous acidic solution has been studied in the acid range 0.1 — 10-4 ≤ [H+] ≤ 2 — 10-4 mol dm-3, ionic strength 0.01 ≤ [I] ≤ 0.18 mol dm-3 (NaCl) and T = 29 ± 1.ºC. The reaction shows a first order dependence on reductant and half order on oxidant concentration respectively. It displayed an inverse dependence on the acid concentration of the reaction medium. The reaction conforms to the rate law: -d[BPR2-]/dt = k2[BPR2-][IO4-]1/2[H+]-1/2 The stoichiometry of the reaction is 1:1. Added anions had no effect on the rate of the reaction. Spectroscopic investigation indicates that an intermediate complex is probably formed in the course of this reaction. The reaction is believed to proceed via the innersphere mechanistic pathway.

Entropy-Controlled Cu(II)-Catalyzed Oxidation of N-Acetyl-L-Cysteine by Methylene Blue in Acidic Medium

2017 ◽  
Vol 231 (6) ◽  
Author(s):  
Ranjana Sharma ◽  
Mahender Pal ◽  
K.K. Mishra
Keyword(s):  
Methylene Blue ◽  
Acidic Medium ◽  
Hydrogen Ions ◽  
First Order ◽  
First Order Kinetics ◽  
Rate Of Reaction ◽  
Entropy Of Activation ◽  
Size And Morphology ◽  
Kinetics Of ◽  
Catalyzed Oxidation

AbstractKinetics of the oxidation of N-acetyl-L-cysteine (NAC) by methylene blue (MB) catalyzed by Cu(II) have been investigated in presence of HCl. The reaction follows a first order kinetics in MB while the concentration order in NAC is zero. Hydrogen ions retard the rate of reaction. The reaction involves the participation of nanoparticles as revealed by SEM, XRD and FTIR techniques and a gel-like Cu-NAC network acts like the effective catalyst. The reaction conforms to Eley-Rideal mechanism at lower [NAC] while at higher [NAC], the kinetics are explained by extended Eley-Rideal mechanism. The reaction is regulated by the size and morphology of the nanoparticles and is controlled by the entropy of activation.

Kinetics and Mechanism of Hexachloroiridate(IV) Oxidation of Arsenic(III) in Acidic Perchlorate Solutions

1992 ◽  
Vol 57 (7) ◽  
pp. 1451-1458 ◽  
Author(s):  
Refat M. Hassan
Keyword(s):  
Ionic Strength ◽  
Fractional Order ◽  
Activation Parameters ◽  
Order Reaction ◽  
First Order Reaction ◽  
Intermediate Complex ◽  
Constant Ionic Strength ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Kinetics Of

The kinetics of oxidation of arsenic(III) by hexachloroiridate(IV) at lower acid concentrations and at constant ionic strength of 1.0 mol dm-3 have been investigated spectrophotometrically. A first-order reaction in [IrCl62-] and fractional order with respect to arsenic(III) have been observed. A kinetic evidence for the formation of an intermediate complex between the hydrolyzed arsenic(III) species and the oxidant was presented. The results showed that decreasing the [H+] is accompanied by an appreciable acceleration of the rate of oxidation. The activation parameters have been evaluated and a mechanism consistent with the kinetic results was suggested.

Osmium(VIII) Catalyzed Oxidation of Acetone and Ethylmethyl Ketone by Chloramine-T

1972 ◽  
Vol 27 (10) ◽  
pp. 1161-1163 ◽  
Author(s):  
S. P. Mushran ◽  
R. Sanehi ◽  
M. C. Agraval
Keyword(s):  
Acidic Medium ◽  
Present Note ◽  
Alkaline Media ◽  
Alkaline Solutions ◽  
Slow Step ◽  
First Order ◽  
Chloramine T ◽  
Kinetics Of ◽  
Catalyzed Oxidation ◽  
High Redox Potential

The Osmium (VIII) catalyzed oxidation of acetone and ethylmethyl ketone by chloramine-T, in highly alkaline solutions showed first order dependence to chloramine-T and osmium (VIII). The order of the reactions with respect to alkali and ketone were found to be fractional, being ~-0.82 and 0.3 respectively. No effects of ionic strength were evident. The mechanism has been proposed on the basis of the formation of a complex between N-chlorotoluene-p-sulfonamide and osmium (VIII) in the slow step, which in turn oxidizes the enol anion of the reducing substrate in the fast step.During the study of the mechanism of oxidations by chloramine-T, the kinetics of the oxidation of α-hydroxy acids 1 in presence of osmium (VIII) as catalyst, glycerol2 in neutral and alkaline media, p-cresol3 in an acidic medium, hexacyanoferrate (II)4 in a feebly acidic medium (pH 6-7) and aliphatic aldehydes 5 in alkaline media have been investigated.Despite the high redox potential6 of the chloramine-T/toluene sulfonamide system (1.138 V at pH 12), the oxidation of acetone does not take place in absence of catalyst and that of ethylmethyl ketone proceeds only in highly alkaline solutions7 (NaOH>0.01 M). In the present note the kinetics of the osmium (VIII) catalyzed oxidation of acetone and ethylmethyl ketone have been recorded.

The Decomposition of Sodium Nitrite Solutions in Aqueous Sulphuric and Perchloric Acids

1963 ◽  
Vol 16 (6) ◽  
pp. 927 ◽  
Author(s):  
NS Bayliss ◽  
DW Watts
Keyword(s):  
Aqueous Solutions ◽  
Acid Composition ◽  
Sodium Nitrite ◽  
Decomposition Rate ◽  
Rate Constants ◽  
First Order ◽  
Order Dependence ◽  
Gaseous Products ◽  
Kinetics Of

The kinetics of the decomposition of aqueous solutions of sulphuric and perchloric acids containing sodium nitrite have been investigated at a number of temperatures. The technique involved flushing the decomposing solutions with dry nitrogen to remove the gaseous products. A first-order dependence of decomposition rate on "analytical nitrite" was found, the rate constants being dependent on the solvent acid composition.

scholarly journals Kinetics and Mechanism of Oxidation of Diethanolamine and Triethanolamine by Potassium Ferrate

2011 ◽  
Vol 8 (2) ◽  
pp. 903-909 ◽  
Author(s):  
Shan Jinhuan ◽  
Zhang Jiying
Keyword(s):  
Activation Parameters ◽  
Rate Equations ◽  
Potassium Ferrate ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Order Dependence ◽  
Rate Determining Step ◽  
Thermodynamic Activation Parameters ◽  
Plausible Mechanism ◽  
Kinetics Of

The kinetics of oxidation of diethanolamine and triethanolamine by potassium ferrate(VI)in alkaline liquids at a constant ionic strength has been studied spectrophotometrically in the temperature range of 278.2K-293.2K. The reaction shows first order dependence on potassium ferrate(VI), first order dependence on each reductant, The observed rate constant (kobs) decreases with the increase in [OH-], the reaction is negative fraction order with respect to [OH-]. A plausible mechanism is proposed and the rate equations derived from the mechanism can explain all the experimental results. The rate constants of the rate-determining step and the thermodynamic activation parameters are calculated.

scholarly journals Kinetic Approach to the Reduction of Ethylenediaminetetraacetatoferrate(III) Complex by Iodide Ion in Aqueous Acidic Medium

2019 ◽  
pp. 1-8
Author(s):  
I. U. Nkole ◽  
C. R. Osunkwo
Keyword(s):  
Acidic Medium ◽  
Salt Effect ◽  
Outer Sphere ◽  
Ion Concentration ◽  
Kinetic Approach ◽  
Edta Complex ◽  
Electron Transfer Mechanism ◽  
First Order ◽  
Iodide Ion ◽  
Aqueous Acidic Medium

The kinetic approach to the reduction of ethylenediaminetetraacetatoferrate(III) complex (hereafter [Fe(III)EDTA]-) by iodide ion has been studied spectrophotometrically in an aqueous acidic medium. The study was carried out under pseudo-first order conditions of an excess of iodide ion concentration at 28 ± 1, ionic strength (I) = 0.43 coulomb2 mol dm-3 (KNO3) and [H+] = 5.0  10-2 mol dm-3. The [Fe(III)EDTA]- complex was reduced according to the reaction; 2[Fe(III)EDTA]- + 2I-  → 2[Fe(II)EDTA]2- + I2 The rate law is - d[Fe(III)EDTA-]/dt = (a + b[H+])[Fe(III)EDTA-][I-] The rate of the reaction is first order in oxidant and reductant concentrations, and displayed positive Brønsted-Debye salt effect. On the basis of catalysis by added cation, Michaelis-Menten plots and the absence of intermediates, the outer-sphere electron transfer mechanism is proposed for the reaction.

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