Thermometric determination and analytical application of the landolt effect

Gaál, Ferenc F.; Sörös, V.I.; Vajgand, Vilim J.

doi:10.1016/s0003-2670(01)82846-4

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1990

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Cited by 6 publications

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“…[13] stands for the total concentration of hydrogen peroxide (H202 + H3O2+) present in the experiments, whereas in eq. [14] stands for the total concentration of catalyst (H2Mo04 + H2Mo05 + HMo05-), that is, the initial concentration of sodium molybdate used to prepare the solutions.…”

Section: Discussionmentioning

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: Discussionmentioning

confidence: 99%

“…This means that the free form of hydrogen peroxide (H202) was predominant in the experiments and, therefore, the total concentration of hydrogen peroxide [H2O2lT can also be approximately written in eq. [13] as [H202]. Moreover, it is well-known (25) that molybdenum(V1) is easily peroxidized (i.e., K5 is very high).…”

Section: Discussionmentioning

confidence: 99%