A key step in the formation of sulfuric acid from dissolved SO, in acid precipitation is the oxidation of hydrogen sulfite ion by hydrogen peroxide: HSO5 (aq) + H2O2(aq) → HSO (aq) + H2O(€) The mechanism involves peroxymonosulfurous acid, SO,OOH¯: ki HSO (aq) + H2O2(aq) SO20OH¯(aq) + H2O(€) k-1 2 SO,OOH"(aq) + H;O* (aq) HSO, (aq) + H;O* (aq) By making a steady-state approximation for the reactive intermediate concentration, [SO,OOH (aq)], express the rate of formation of HSO, (aq) in terms of the concentra- tions of HSO, (aq), H2O2(aq), and H;0*(aq).

A key step in the formation of sulfuric acid from dissolved SO, in acid precipitation is the oxidation of hydrogen sulfite ion by hydrogen peroxide: HSO5 (aq) + H2O2(aq) → HSO (aq) + H2O(€) The mechanism involves peroxymonosulfurous acid, SO,OOH¯: ki HSO (aq) + H2O2(aq) SO20OH¯(aq) + H2O(€) k-1 2 SO,OOH"(aq) + H;O* (aq) HSO, (aq) + H;O* (aq) By making a steady-state approximation for the reactive intermediate concentration, [SO,OOH (aq)], express the rate of formation of HSO, (aq) in terms of the concentra- tions of HSO, (aq), H2O2(aq), and H;0*(aq).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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