The kinetics of the reduction of tetraoxoiodate(VII) by n-(2-hydroxylethyl)ethylenediaminetriacetatocobaltate(II) ion in aqueous perchloric acid

Onu, A. D.; Iyun, J. F.; Idris, S. O.

doi:10.1007/s11243-009-9273-1

Cited by 9 publications

(14 citation statements)

References 16 publications

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“…The electronic spectrum of the complex gave λmax at 520 nm which was in agreement with literature value (Onu et al, 2009(Onu et al, , 2015.The result of spectrophotometric titration showed that two moles of the reductant were consumed by one mole of the oxidant. The plots of the titration from which the stoichiometry was determined is presented in Figure 1.…”

Section: Resultssupporting

confidence: 89%

“…The stoichiometry of the reaction was determined by spectrophotometric titration using the mole ratio method (Onu et al, 2009 and. The concentration of [Co(II)EDTA] 2was kept constant at 5.0 × 10 -3 mol dm −3 while that of S2O8 2was varied 4 folds below and above that of S2O8 2-.…”

Section: Methodsmentioning

confidence: 99%

“…Thus, the study of oxidation of these complexes has continued to receive wide attention. Electron transfer reactions of these complexes with some oxyanions have been reported (Onu et al, 2008(Onu et al, , 2009(Onu et al, , 2015(Onu et al, & 2016Naik et al, 2007& Mansour, 2003. In these studies both the inner-sphere and outer-sphere mechanisms were reported.…”

Section: Introductionmentioning

confidence: 97%

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Kinetics of oxidation of ethylenediammine-N,N,N’,N’-tetraacetatocobaltate(II)complex by silver-activated persulphate ion in aqueous acidic medium

Onu¹,

Idris²,

Yaraghi³

2019

Nig J Bas App Sci

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The kinetics of oxidation of Ethylenediammine-N,N,N',N'-tetraacetatocobaltate(II) complex (()) by silver-activated persulphate ion in a ueous nitric acid medium was studied at I = 0.5 mol dm-3 (NaNO3), [H + ] = 1 × 10-2 mol dm-3 , [Ag + ] = 1 × 10-2 mol dm-3 , T = 299 ± 1 K and λmax = 520 nm. Stoichiometric study showed 2:1 (Reductant: Oxidant) mole ratio. The reaction exhibited first order with respect to the [Co(II)EDTA 2-] and [  2 8 2 O S ] and the rate constant, (5.90 × 10-2 dm 3 mol-1 s-1) was independent of the acid concentration, but varied linearly with catalyst concentration, [Ag + ]. The overall rate law is represented as: () () The reaction displayed zero salt effect suggesting an activated complex composed of either a neutralcharged, neutral-neutral reactant species or ion-pair. The reaction was catalysed by addition of formate ion, HCOOand the Michaelis-Menten's type plot gave zero intercept indicating the absence of intermediate complex. Also, the activation enthalpy (= +39.27 kJ mol-1) and entropy (=-136.73 J K-1 mol-1) were determined. The entropy of activation shows a more ordered activated complex relative to the reactants species. Evaluating the experimental data, an outer-sphere mechanistic pathway via ion pair activated complex is proposed for the reaction.

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Section: Resultssupporting

confidence: 89%

Section: Methodsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 97%

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Kinetics of oxidation of ethylenediammine-N,N,N’,N’-tetraacetatocobaltate(II)complex by silver-activated persulphate ion in aqueous acidic medium

Onu¹,

Idris²,

Yaraghi³

2019

Nig J Bas App Sci

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“…Although the equilibrium in Equation 2has been established for hydrogen peroxide reactions, the nature of acid dependent obtained in this study coupled with the insensitivity of the reaction to change in ionic strength; envisaging an activated complex composed of anions ([CoHEDTAOH 2 ] − and 2 HO − ) is not supported by experimental result in this study. The mechanistic scheme below which involves a deprotonation of the complex specie [32]…”

Section: ) Catalysis Of Reaction By Added Anionmentioning

confidence: 99%

Kinetics and Stoichiometry of the Reduction of Hydrogen Peroxide by an Aminocarboxylactocobaltate(II) Complex in Aqueous Medium

Onu¹,

Iyun²,

Idris³

2015

OJIC

Self Cite

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The kinetics and stoichiometry of the reduction of H2O2 by an aminocaboxylactocobaltate(II) complex (hereafter[CoHEDTAOH2] −) in aqueous medium have been studied under the following conditions: T = 29˚C ± 1˚C, Ionic Strength, I = 0.50 mol dm −3 (NaClO4), [H + ] = 1 × 10 −3 mol dm −3. The ratio from the stoichiometric study conforms to the equation 2[CoHEDTAOH2] − + H2O2 + 2H + → 2 [Co-HEDTAOH2] + 2H2O. The rate of reaction varied linearly to the first power of the concentrations of the reductant and oxidant and displayed inverse dependence on acid concentration. The plot of acid dependent rate constant versus [H + ] −1 was linear with zero intercept. The [CoHEDTAOH2] −-H2O2 reaction was insensitive to the change in ionic strength of the medium suggesting interaction of charged and uncharged species at the activated complex. The Michaelis-Menten plot of [ ] 1 1 1 versus k oxidant was linear without intercept which suggested absence of intermediate complex. Evidences in this paper showed that the reaction occurred through the outer-sphere mechanism.

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“…The stoichiometry of the reaction was control by spectrophotometric titration utilizing the mole ratio technique. The stoichiometry was assessed from a graph of absorbance against the mole ratio ( Onu et al., 2009 ).…”

Section: Methodsmentioning

confidence: 99%

A kinetic study and mechanisms of reduction of N, N′-phenylenebis(salicyalideneiminato)cobalt(III) by L-ascorbic acid in DMSO-water medium

Abdulsalam

Idris

Shallangwa

et al. 2020

Heliyon

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The kinetics of reduction of N, N 1 -phenylene bis -(salicylideneiminato)cobalt (III), referred to as [Co(Salophen)] + by L-ascorbic acid (H 2 A) was studied in mixed aqueous medium (DMSO:H 2 O; 1:4 v/v) under pseudo-first-order conditions at 33 ± 1 °C, μ = 0.1 mol dm −3 (NaCl) and λ max = 470 nm. L-ascorbic acid was oxidized to dehydroascorbic acid with kinetics that was first order in both the [H 2 A] and [Co(Salophen) + ] and second-order overall. The reaction involves two parallel reaction pathways; an acid-dependent and the inverse acid-dependent pathways. The inverse acid pathway shows that there is a pre-equilibrium step before the rate determining-step in which a proton is lost. The kinetics followed negative Brønsted–Debye salt effect. Evidence was obtained for the presence of free radicals but none to support the formation of an intermediate complex of significant stability during the reaction. Overall, the data obtained suggest an outer-sphere mechanism for the reaction. A plausible mechanism is proposed.

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The kinetics of the reduction of tetraoxoiodate(VII) by n-(2-hydroxylethyl)ethylenediaminetriacetatocobaltate(II) ion in aqueous perchloric acid

Cited by 9 publications

References 16 publications

Kinetics of oxidation of ethylenediammine-N,N,N’,N’-tetraacetatocobaltate(II)complex by silver-activated persulphate ion in aqueous acidic medium

Kinetics of oxidation of ethylenediammine-N,N,N’,N’-tetraacetatocobaltate(II)complex by silver-activated persulphate ion in aqueous acidic medium

Kinetics and Stoichiometry of the Reduction of Hydrogen Peroxide by an Aminocarboxylactocobaltate(II) Complex in Aqueous Medium

A kinetic study and mechanisms of reduction of N, N′-phenylenebis(salicyalideneiminato)cobalt(III) by L-ascorbic acid in DMSO-water medium

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