The Kinetics of the Reduction, in Acid Solution, of Hydrogen Peroxide by Iodide Ion

Liebhafsky, H. A.; Mohammad, Ali

doi:10.1021/ja01337a010

Cited by 71 publications

(60 citation statements)

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“…The mechanism proposed for the uncatalyzed reaction (reactions [4], [7], [8], and [lo]) is consistent with the ones proposed by other authors for..the same reaction (5,7,27,28). As far as the catalyzed reaction is concerned, albeit the mechanism given in reactions [5], [6], and [9] differs notably from previous proposals (16,17), it is in better agreement with the experimental rate law (eq.…”

Section: Discussionsupporting

confidence: 87%

“…As far as the catalyzed reaction is concerned, albeit the mechanism given in reactions [5], [6], and [9] differs notably from previous proposals (16,17), it is in better agreement with the experimental rate law (eq. [3]) found in this work.…”

Section: Discussionsupporting

confidence: 60%

“…According to the kinetic data obtained in this work, the overall mechanism that can be proposed for the oxidation of iodide ion by the molybdenum(V1) -hydrogen peroxide system is as follows: First, we have considered in reaction [4] the equilibrium of H202 in reaction [5] to form H2Mo05; actually, the existence of protonation of hydrogen peroxide to enhance its oxidizing power, peroxymolybdic acid, as well as that of other peroxyderivatives due to the fact that the electron density of H302+ is lower than of molybdenum(VI), is already known (25,26). The equilibrium that of H202; i.e., H302+ is a better oxidant than H202.…”

Section: Discussionmentioning

confidence: 99%

“…The reaction between iodide ion and hydrogen peroxide in aqueous solution (overall stoichiometry: 31-+ H202 + 2H+ + 13-+ 2H20) has been the subject of kinetic study for over a century (1)(2)(3)(4)(5)(6)(7)(8)(9)(10). In particular, it has been established that several oxyanions, such as molybdate ion, have a catalytic effect on that reaction, what has been shown to be useful for the analytical determination of microquantities of those oxyanions (1 1-14).…”

Section: Introductionmentioning

confidence: 99%

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

Arias¹,

Mata²,

Perez‐Benito³

1990

Can. J. Chem.

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). The kinetics of oxidation of potassium iodide by hydrogen peroxide in aqueous perchloric acid has been studied both in the The activation energies associated with rate constants kl, k2, and k3 are 52 ? 1, 49 t 1, and 42 ? 3 kJ mol-', respectively.A mechanism in agreement with the experimental kinetic data is proposed, according to which rate constants k, , k2, and k3 correspond to the oxidations of iodide ion by H202. H302+ and H2Mo05, respectively.

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Section: Discussionsupporting

confidence: 87%

Section: Discussionsupporting

confidence: 60%

Section: Discussionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

See 2 more Smart Citations

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

Arias¹,

Mata²,

Perez‐Benito³

1990

Can. J. Chem.

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“…Iodide is known to decompose hydrogen peroxide (Eq. 1) with iodide consumed at a molar ratio of 3:1 (I -: HP); bromide was known to react similarly [36,37] darken after a few months storage, but the inhibiting effect of iodide was not diminished.…”

Section: Adulterated Reactionsmentioning

confidence: 99%

Factors Influencing Triacetone Triperoxide (TATP) and Diacetone Diperoxide (DADP) Formation: Part I

Oxley

Smith

Bowden

et al. 2013

Propellants Explo Pyrotec

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Conditions which result in the formation of triacetone triperoxide (TATP) or diacetone diperoxide (DADP) from acetone and hydrogen peroxide (HP) have been studied for the purposes of inhibiting the reaction. Reaction of HP with acetone precipitates either DADP or TATP, but the overall yield and amount of each was found to depend on (1) reaction temperature; (2) the molar ratio of acid to HP/acetone; (3) initial concentrations of reactants, and (4) length of reaction. Controlling molar ratios and concentrations of starting materials was complicated because both sulfuric acid and hydrogen peroxide were aqueous solutions.Temperature exercised great control over the reaction outcome. Holding all molar concentrations constant and raising the temperature from 5 to 25°C showed an increase of DADP over TATP formation and a decrease in overall yield. At 25°C a good yield of TATP was obtained if the HP to acetone ratio was kept between 0.5-to-1 and 2-to-1. At constant temperature and HP-toacetone held at one-to-one ratio, acid-to-HP molar ratios between 0.10:1 and 1.2:1 produced good yield of TATP. Plotting the molality of HP versus that of sulfuric acid revealed regions in which relatively pure DADP or pure TATP could be obtained. In addition to varying reaction conditions, adulterants placed into acetone were tested to inhibit the formation of TATP. 2Because there is much speculation of the relative stability, sensitivity, including solvent wetting of crystals, and performance of DADP and TATP, standard tests (i.e. DSC, drop weight impact, and SSED) were performed.

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The Temperature‐Dependence of E _a

Perlmutter-Hayman

1976

Progress in Inorganic Chemistry

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The Kinetics of the Reduction, in Acid Solution, of Hydrogen Peroxide by Iodide Ion

Cited by 71 publications

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

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

Factors Influencing Triacetone Triperoxide (TATP) and Diacetone Diperoxide (DADP) Formation: Part I

The Temperature‐Dependence of E _a

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The Kinetics of the Reduction, in Acid Solution, of Hydrogen Peroxide by Iodide Ion

Cited by 71 publications

References 0 publications

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

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

Factors Influencing Triacetone Triperoxide (TATP) and Diacetone Diperoxide (DADP) Formation: Part I

The Temperature‐Dependence of E a

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The Temperature‐Dependence of E _a