Why is the below reaction split into two independentrate stages.The overall reaction between hydrogen peroxide and iodide ion in acid solution is:H2O2 + 2H* + 31-2H,O + I;I, + IThe kinetics of this reaction has been interpreted as consisting of two independent ratedetermining stages:H2O2 + IH20 + IO-(1)k1H2O2 + H* + IН.О + HIO

The rate of a reaction is the rate of decrease of concentration of of reactants or the rate o…

Why is the below reaction split into two independent rate stages. The overall reaction between hydrogen peroxide and iodide ion in acid solution is: H2O2 + 2H* + 3I- 2H,O + Iz I2 + I The kinetics of this reaction has been interpreted as consisting of two independent rate determining stages: k,° H2O2 + I H2O + IO¯ (1) k1 H2O2 + H* + I H20 + HIO (2)

Why is the below reaction split into two independent rate stages. The overall reaction between hydrogen peroxide and iodide ion in acid solution is: H2O2 + 2H* + 3I- 2H,O + Iz I2 + I The kinetics of this reaction has been interpreted as consisting of two independent rate determining stages: k,° H2O2 + I H2O + IO¯ (1) k1 H2O2 + H* + I H20 + HIO (2)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 68QAP: For the decomposition of a peroxide, the activation energy is 17.4 kJ/mol. The rate constant at 25C...

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