Kinetics of the Oxidation of Ethylene Diamine Tetra Acetic Acid by Chloramine-T

1973 ◽  
Vol 28 (7-8) ◽  
pp. 483-485 ◽  
Author(s):  
Ram Sanehi ◽  
R. M. Mehrotra ◽  
S. P. Mushran
Keyword(s):  
Acetic Acid ◽  
Activation Parameters ◽  
Hydrogen Ion ◽  
Ethylene Diamine ◽  
Acidic Media ◽  
First Order ◽  
Order Dependence ◽  
Plausible Mechanism ◽  
Chloramine T ◽  
Kinetics Of

The kinetics of the oxidation of ethylene diamine tetra acetic acid (EDTA) by chloramine-T in acidic media has been investigated. The reaction shows first order dependence in chloramine-T and the order in hydrogen ion and substrate is fractional. On the basis of kinetic results a plausible mechanism is suggested. Activation parameters have also been calculated.

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 Reactivity of Phenol and Aniline towards Quinolinium Chloro Chromate: A Comparative Oxidation Kinetic Study

2015 ◽  
Vol 59 ◽  
pp. 81-92
Author(s):  
Seplapatty Kalimuthu Periyasamy ◽  
H. Satham Hussain ◽  
R. Manikandan
Keyword(s):  
Oxidation Kinetic ◽  
Activation Parameters ◽  
Dipole Interaction ◽  
Reaction Rates ◽  
Hydrogen Ion ◽  
Aqueous Acetic Acid ◽  
Acetic Acid Medium ◽  
First Order ◽  
Different Temperatures ◽  
Kinetics Of

The kinetics of Oxidation of Phenol and aniline by quinolinium Chlorochromate (QCC) in aqueous acetic acid medium leads to the formation of quinone and azobenzene respectively. The reactions are first order with respect to both Phenol and aniline. The reaction is first order with respect to quinolinium chlorochromate (QCC) and is catalyzed by hydrogen ion. The hydrogen-ion dependence has the form: kobs = a+b [H+]. The rate of oxidation decreases with increasing dielectric constant of solvent, indicating the presence of an ion-dipole interaction. The reaction does not induced the polymerization of acrylonitrile. The retardation of the rate by the addition of Mn2+ ions confirms that a two electron transfer process is involved in the reaction. The reaction rates have been determined at different temperatures and the activation parameters have been calculated. From the above observations kinetic results a probable mechanism have been proposed.

scholarly journals Kinetics of the Oxidation of methyl n-propyl ketone by manganese(III) sulphate

1971 ◽  
Vol 26 (1) ◽  
pp. 30-31 ◽  
Author(s):  
K. K. Banerji ◽  
P. Nath ◽  
G. V. Bakore
Keyword(s):  
Acetic Acid ◽  
Activation Parameters ◽  
Solvent Composition ◽  
Keto Form ◽  
First Order ◽  
Propyl Ketone ◽  
Kinetics Of

The oxidation of methyl n-propyl ketone by Mn (III) sulphate in aq. acetic acid is first order with respect to the ketone and Mn (III). The rate is independent of acidity and solvent composition. The activation parameters for oxidation and enolisation were evaluated. Oxidation is faster than enolisation under similar conditions. A mechanism involving an attack on the keto-form by Mn (III) is proposed.

scholarly journals Oxidation of Some Aliphatic Alcohols by Pyridinium Chlorochromate -Kinetics and Mechanism

2009 ◽  
Vol 6 (1) ◽  
pp. 237-246 ◽  
Author(s):  
Sapana Jain ◽  
B. L. Hiran ◽  
C. V. Bhatt
Keyword(s):  
Dielectric Constant ◽  
Carbonyl Compounds ◽  
Activation Parameters ◽  
Dipole Interaction ◽  
Hydrogen Ion ◽  
Pyridinium Chlorochromate ◽  
Secondary Alcohols ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Kinetics Of

Kinetics of oxidation of some aliphatic primary and secondary alcoholsviz.,ethanol, propan-1-ol, propan-2-ol, butan-1-ol, butan-2-ol and 2-methyl butanol by pyridinium chlorochromate (PCC) have been studied in water- perchloric acid medium. The reaction shows first order dependence with respect to pyridinium chlorochromate [PCC] and hydrogen ion [H+]. The rate of oxidation decreases with increase in dielectric constant of solvent suggests ion-dipole interaction. Activation parameters have been evaluated. Products are carbonyl compounds and free radical absence was proved. A tentative mechanism has been proposed.

scholarly journals Kinetics and Mechanism of Oxidation ofL-Cystine by Hexacyanoferrate(III) in Alkaline Medium

2009 ◽  
Vol 6 (1) ◽  
pp. 93-98 ◽  
Author(s):  
Annapurna Nowduri ◽  
Kalyan Kumar Adari ◽  
Nageswara Rao Gollapalli ◽  
Vani Parvataneni
Keyword(s):  
Alkaline Medium ◽  
Oxidation Product ◽  
Experimental Results ◽  
Cysteic Acid ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Order Dependence ◽  
Plausible Mechanism ◽  
Mechanism Of Oxidation ◽  
Kinetics Of

Kinetics of oxidation ofL-cystine by hexacyanoferrate(III) was studied in alkaline medium at 30 °C. The reaction was followed spectrophotometrically at λmax = 420 nm. The reaction was found to be first order dependence each on [HCF(III)] and [cystine]. It was found that the rate of the reaction increases with increase in [OH-]. The oxidation product of the reaction was found to be cysteic acid. A plausible mechanism has been proposed to account for the experimental results.

scholarly journals Kinetics of Oxidation of Cychlohexanol by N-Chloronicotinamide in Aqueous Acetic Acid Medium

2004 ◽  
Vol 3 (1) ◽  
pp. 1-6
Author(s):  
R. Sridharan ◽  
N. Mathiyalagan
Keyword(s):  
Acetic Acid ◽  
Acid Medium ◽  
Activation Parameters ◽  
Acid Mixture ◽  
Aqueous Acetic Acid ◽  
Acetic Acid Medium ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Retarding Effect ◽  
Kinetics Of

Kinetics of oxidation o Cyclohexanol by N-Chloronicotinamide(NCN) in 50% V/V aqueous acetic acid mixture has been investigated in the presence of HCIO4 and NaCl. The observed rate of oxidation is first-order with respect to oxidation (NCN) and fractional-order with respect to cyclohexanol. A decrease in dielectric constant of the medium increases the rate. Addition of nicotinamide (NA), the reduction product of NCN, has a retarding effect an the rate of oxidation. Arrhenius and activation parameters are calculated. Kinetics of bromination1 and oxidation2,3 of saturated organic compounds by N-bromosuccinimide(NBS) have been received considerable attention. Kinetics and mechanism of oxidation of amino acids by NCN has been reported in aqueous acetic acid medium, we report herein the result of similar studies on the oxidation of cyclohexanol with NCN in aqueous acetic acid medium.

scholarly journals Kinetics of Oxidation of 3-Benzoylpropionic Acid byN-Chlorobenzamide in Aqueous Acetic Acid Medium

2011 ◽  
Vol 8 (2) ◽  
pp. 561-564 ◽  
Author(s):  
N. A. Mohamed Farook ◽  
G. A. Seyed Dameem
Keyword(s):  
Acetic Acid ◽  
Acid Medium ◽  
Reaction Medium ◽  
Activation Parameters ◽  
Slow Step ◽  
Aqueous Acetic Acid ◽  
Acetic Acid Medium ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Kinetics Of

The kinetics of oxidation of 3-benzoylpropionic acid(KA)byN-chlorobenzamide(NCB)in aqueous acetic acid medium in the presence of perchloric acid have been investigated. The observed rate of oxidation is first order dependence each in[KA],[NCB]and [H+]. The main product of the oxidation is the corresponding carboxylic acid. The rate decreases with the addition of benzamide, one of the products of the reaction. Variation in ionic strength of the reaction medium has no significant effect on the rate of oxidation. But the rate of the reaction is enhanced by lowering the dielectric constant of the reaction medium. Hypochlorous acidium ion (H2O+Cl), has been postulated as the reactive oxidizing species. A mechanism consistent with observed results have been proposed and the related rate law deduced. The activation parameters have been computed with respect to slow step of the mechanism.

scholarly journals Non enzymatic NADH-dependent reduction of Cis-[Co(en)2(H2O)2]3+ in aqueous medium

2018 ◽  
Vol 6 (2) ◽  
pp. 163
Author(s):  
Bharati Behera ◽  
Jashoda Behera
Keyword(s):  
Electron Transfer ◽  
Aqueous Medium ◽  
Transfer Reaction ◽  
Activation Parameters ◽  
Electron Transfer Reaction ◽  
Transfer Reactions ◽  
Electron Transfer Reactions ◽  
First Order ◽  
Order Dependence ◽  
Kinetics Of

The kinetics of the electron transfer reaction of NADH with Cis-[Co(en)2(H2O)2]3+ has been studied over the range 1.0 ≤ 102 [NADH] ≤ 3.0 mol dm-3, 7.0 ≤ pH ≤ 8.0 and 200C ≤ t ≤ 350C in aqueous medium. The rate of electron transfer reaction was found to be first-order dependence each in [NADH]T and Cis-[Co(en)2(H2O)2]3+T. The products of the reaction were found to be NAD+ and Co(II). The corresponding activation parameters of the electron transfer reactions were found to be as ΔH#=27.55 kJ mol-1 and  ΔS#= -189.35 JK-1mol-1. 

Kinetics of the Oxidation of Aliphatic Aldehydes by Chromic Acid

1971 ◽  
Vol 26 (5) ◽  
pp. 383-385 ◽  
Author(s):  
C. Goswami ◽  
K. K. Banerji
Keyword(s):  
Acetic Acid ◽  
Chromic Acid ◽  
Activation Parameters ◽  
Acid Oxidation ◽  
First Order ◽  
Chromic Acid Oxidation ◽  
Rate Determining Step ◽  
Reversible Formation ◽  
Kinetics Of ◽  
Chromate Ion

The kinetics of chromic acid oxidation of propanaldehyde, butyraldehyde and isobutyraldehyde in aq. acetic acid have been studied. The product of the oxidation is the corresponding carboxylic acid. The reaction is of first order with respect to each the acid chromate ion, HCrO4⊖, and the aldehyde but of second order to hydrogen ion. The rate increases with proportion of acetic acid in the solution. The activation parameters for the oxidation and enolisation reactions have been evaluated. The rate of enolisation under similar condition is less than that of oxidation. A mechanism in which the first step is the rapid reversible formation of a chromate ester followed by a hydrideion transfer in the rate determining step has been suggested.

Kinetics and Mechanism of Oxidation of Tin(II) by Hexachloroiridate(IV) in Aqueous Perchlorate Solutions

1992 ◽  
Vol 57 (2) ◽  
pp. 326-331 ◽  
Author(s):  
Refat M. Hassan
Keyword(s):  
Reaction Mechanism ◽  
Reaction Rate ◽  
Activation Parameters ◽  
Hydrogen Ion ◽  
Ion Concentration ◽  
Hydrogen Ion Concentration ◽  
First Order ◽  
Mechanism Of Oxidation ◽  
Kinetics Of ◽  
Overall Kinetics

The kinetics of hexachloroiridate(IV) oxidation of tin(II) in aqueous perchlorate media at a constant ionic strength of 2.0 mol dm-3 have been studied spectrophotometrically. The reaction was found to follow second-order overall kinetics and first order with respect to each of the reactants. The results showed hydrogen ion dependence where the reaction rate increased with increasing hydrogen ion concentration. The activation parameters were evaluated and a tentative reaction mechanism has been discussed.

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