A clock reaction is commonly used to demonstrate principles of chemical kinetics. In a clock reaction, an initially colorless solution changes color at a precise time during the course of the reaction. One such clock reaction is based on a reaction between S2O82– and I–. The rate law was determined to be rate = k [ S2O82–] [I–]. The following mechanism has been proposed for the reaction. Predict whether the steps are fast or slow based on the overall rate law.

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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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A clock reaction is commonly used to demonstrate principles of chemical kinetics. In a clock reaction, an initially colorless solution changes color at a precise time during the course of the reaction. One such clock reaction is based on a reaction between S2O82– and I. The rate law was determined to be rate = k [ S2O82–] [I]. The following mechanism has been proposed for the reaction. Predict whether the steps are fast or slow based on the overall rate law.

S2O82–+ Iyield  IS2O83–  fast or slow

IS2O83– yield 2 SO42– + Ifast or slow

I++ I yield I2                          fast or slow

I2+ I yield I3–                         fast or slow

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