Oxidative study of gabapentin by alkaline hexacyanoferrate(III) in room temperature in presence of catalytic amount of Ru(III) – a mechanistic approach

Jose, Timy P.; Angadi, Mahantesh A.; Salunke, Manjalee S.; Tuwar, Suresh M.

doi:10.1016/j.molstruc.2008.05.006

Cited by 15 publications

(9 citation statements)

References 13 publications

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“…Ruthenium(III) chloride has been extensively used as a catalyst in many redox reactions involving one or two equivalent oxidants [11][12][13][14] . The existence of Ru(III) in its chloride complexes are possible only when on heating [21] or aging in presence of higher concentration of HCl.…”

Section: Discussionmentioning

confidence: 99%

“…The redox potentials of Ru(IV)/Ru(III) is +1.3 V which is unexpectedly higher than that of Os(VIII)/Os(VI) of + 0.85 V. This suggests that the ruthenium is a good catalyst in +3 state. Apart from this and the fact that the substrates are oxidized by two equivalent change in the form of hydride ion [12,13,14] abstraction in Ru(III) catalysis, irrespective of one equivalent or two equivalent oxidants used. Hence, to understand the reaction path of L-proline in the formation of L-glutamic acid, a single equivalent oxidant, HCF and Ru(III) as a catalyst are used.…”

Section: Introductionmentioning

confidence: 99%

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Kinetics and Mechanism of Ruthenium(III) Catalyzed Oxidation of LProline by Hexacyanoferrate(III) in Aqueous Alkali

Sharanabasamma¹

2011

TOCATJ

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Kinetics of ruthenium(III) catalyzed oxidation of L-proline by hexacyanoferrate(III)(HCF) in alkali was studied spectrophotometrically at 30 0 C. A reaction was found to be independent upon [L-proline]. The reaction was occurred without intervening free radical. Since unit order each in [Ru(III)] and [HCF], the oxidation follows an outer-sphere mechanism. A suitable mechanism was proposed and rate law was derived asThe rate constant, 'k' and equilibrium constant 'K 1 ' of the prior equilibrium step of reaction,were calculated. The oxidative product of L-proline was analyzed quantitatively as L-glutamic acid. Activation parameters were evaluated.

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Section: Discussionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Kinetics and Mechanism of Ruthenium(III) Catalyzed Oxidation of LProline by Hexacyanoferrate(III) in Aqueous Alkali

Sharanabasamma¹

2011

TOCATJ

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“…Hexacyanoferrate (III) (HCF(III)) ion in alkaline medium known to oxidise inorganic and organic compounds [17][18][19][20][21][22][23][24][25][26][27][28][29] HCF(III)/ HCF(II) is a one electron oxidant with a redox potential of +0.36 V [30]. It is a moderate oxidizing agent and therefore, is used as electron or proton abstracting agent and results in the formation of a free radical intermediate during the oxidation of organic compounds [31].…”

Section: Introductionmentioning

confidence: 99%

Mechanistic investigation of the oxidation of Cefuroxime by hexacyanoferrate(III) in alkaline conditions

Khan

Asiri

Azum

et al. 2013

Journal of Industrial and Engineering Chemistry

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“…It is also known that it exists [9] in various forms, viz. [OsO 3 (OH) 3 ] À , [OsO 4 (OH) 2 ] 2 À and [OsO 5 (OH)] 3 À in alkali. Hence, to determine the active form of osmium(VIII), and the path followed during catalysis, it has been selected as a catalyst in the HCF oxidations of organic substrates.…”

Section: Introductionmentioning

confidence: 99%

Mechanism of the Osmium(Viii)-Catalysed Oxidation of Fursemide by Alkaline Hexacyanoferrate(Iii) and Analysis of Fursemide by a Kinetic and Catalytic Method

Billalli

Sharanabasamma

Tuwar

2010

Progress in Reaction Kinetics and Mechanism

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The kinetics of the title reaction showed first-order behaviour both in hexacyanoferrate(III) and osmium(VIII) and fractional order each in fursemide and alkali concentrations. The added product, [Fe(CN) 6 ] 4 À , retarded the rate of reaction. The active species of osmium(VIII) in alkali appears to be [OsO 5 (OH)] 3 À . A mechanism involving a complex formed between osmium(VIII) and fursemide, followed by its oxidation with hexacyanoferrate(III) in a rate-determining step is proposed. A rate law for the mechanism was derived and verified. The formation constant, K 2 for [OsO 5 (OH)] 3 À , K 3 for the complex, and the rate constant of the slow step, k, were evaluated. The activation parameters E a , DH # , DS # , DG # and log A were calculated as 55.2 + 2 kJ mol À 1 , 52.7 + 2 kJ mol À 1 , À 52.0 + 2 J K À 1 mol À 1 , 69.8 + 2.5 kJ mol À 1 and 6.5 + 0.1 respectively.Fursemide is used in the pharmacotherapy for various diseases and it is also considered as a doping agent in sports. A simple and specific procedure for its analysis was developed being based on its oxidation by alkaline hexacyanoferrate(III) in the presence of trace amount of osmium(VIII) catalyst. Three different methods have been recommended, namely, the rate constant method, fixed time method and fixed change in optical density method. Of these, the latter two were found to be fast, simple, and accurate. From these methods, fursemide could be analysed from a few micrograms to milligrams per cm 3 . The interference by binders of tablets, and other possible substances like proteins and amino acids, have also been studied.

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Oxidative study of gabapentin by alkaline hexacyanoferrate(III) in room temperature in presence of catalytic amount of Ru(III) – a mechanistic approach

Cited by 15 publications

References 13 publications

Kinetics and Mechanism of Ruthenium(III) Catalyzed Oxidation of LProline by Hexacyanoferrate(III) in Aqueous Alkali

Kinetics and Mechanism of Ruthenium(III) Catalyzed Oxidation of LProline by Hexacyanoferrate(III) in Aqueous Alkali

Mechanistic investigation of the oxidation of Cefuroxime by hexacyanoferrate(III) in alkaline conditions

Mechanism of the Osmium(Viii)-Catalysed Oxidation of Fursemide by Alkaline Hexacyanoferrate(Iii) and Analysis of Fursemide by a Kinetic and Catalytic Method

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