34. 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: HSO3 (aq) + H2O2(aq) → HSO, (aq) + H2O(e) The mechanism involves peroxymonosulfurous acid, SO,OOH: ki HSO5 (aq) + H2O2(aq) = k-1 SO2OOH¯(aq) + H2O(€) k2 SO20OH (aq) + H:0" (аg) HSO, (aq) + H30* (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), H¿O2(aq), and H3O*(aq).
34. 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: HSO3 (aq) + H2O2(aq) → HSO, (aq) + H2O(e) The mechanism involves peroxymonosulfurous acid, SO,OOH: ki HSO5 (aq) + H2O2(aq) = k-1 SO2OOH¯(aq) + H2O(€) k2 SO20OH (aq) + H:0" (аg) HSO, (aq) + H30* (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), H¿O2(aq), and H3O*(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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Question
![34. 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) -
The mechanism involves peroxymonosulfurous acid,
SO,0OH:
HSO, (aq) + H20(e)
ki
HSO3 (аg) + H02(aq) — SO20OH (аg)+ H:0(€)
k-1
k2
SO20OH¯(aq) + H3O* (aq)
→ HSO, (aq) + H3O* (aq)
By making a steady-state approximation for the reactive
intermediate concentration, [SO2OOH¯(aq)], express the
rate of formation of HSO, (aq) in terms of the concentra-
tions of HSO3 (aq), H,O2(aq), and H;O*(aq).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8b661251-6f9a-4090-a1f5-56e54f1837ca%2F3bb86a01-6fd9-486f-b596-ffa2baabdbd4%2Flaldr29_processed.png&w=3840&q=75)
Transcribed Image Text:34. 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) -
The mechanism involves peroxymonosulfurous acid,
SO,0OH:
HSO, (aq) + H20(e)
ki
HSO3 (аg) + H02(aq) — SO20OH (аg)+ H:0(€)
k-1
k2
SO20OH¯(aq) + H3O* (aq)
→ HSO, (aq) + H3O* (aq)
By making a steady-state approximation for the reactive
intermediate concentration, [SO2OOH¯(aq)], express the
rate of formation of HSO, (aq) in terms of the concentra-
tions of HSO3 (aq), H,O2(aq), and H;O*(aq).
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