Heterogeneous catalysis in solution. Part 24.—Kinetics of a redox system exhibiting three separate diffusion-controlled regions: the iron(<scp>III</scp>)+ iodide reaction at a rotating platinum disc catalyst

Creeth, Andrew; Spiro, M.

doi:10.1039/ft9918700977

Cited by 7 publications

(1 citation statement)

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“…The typical results of linear regression analysis of the collected data are given in Figure and by prefix− ln nobreak0em.25em⁡ normalΔ t = 37.2 − 12.0 × 10 3 ( 1 / T ) From Figure and eqs and , it follows that A = 5.1 × 10 18 L 2 mol –2 s –1 and E a = 99.7 kJ mol –1 . The value of the activation energy is in excellent agreement with the literature values, for example, 100 kJ mol –1 and 102 kJ mol –1 …”

Section: Resultssupporting

confidence: 89%

The Effect of Temperature and Ionic Strength on the Oxidation of Iodide by Iron(III): A Clock Reaction Kinetic Study

Bauer

Tomišić

Vrkljan³

2012

J. Chem. Educ.

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A laboratory exercise has recently been reported in which the students use the initial rates method based on the clock reaction approach to deduce the rate law and propose a reaction mechanism for the oxidation of iodide by iron(III) ions. The same approach is used in the exercise proposed herein; the students determine the dependence of the reaction rate on ionic strength and temperature in a straightforward manner. The previously proposed mechanism is further supported by the results, the rate-determining step is identified, and the activation parameters E a , Δ ⧧ H, and Δ ⧧ S are determined for the overall reaction of the first two steps of the mechanism. The significance of such kinetic studies in elaborating reaction mechanisms is clearly demonstrated to the students.

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