34. A key step in the formation of sulfuric acid from dissolvedSO, in acid precipitation is the oxidation of hydrogensulfite ion by hydrogen peroxide:HSO5 (aq) + H2O2 (aq) -The mechanism involves peroxymonosulfurous acid,SO,0OH:HSO, (aq) + H20(e)kiHSO3 (аg) + H02(aq) — SO20OH (аg)+ H:0(€)k-1k2SO20OH¯(aq) + H3O* (aq)→ HSO, (aq) + H3O* (aq)By making a steady-state approximation for the reactiveintermediate concentration, [SO2OOH¯(aq)], express therate of formation of HSO, (aq) in terms of the concentra-tions of HSO3 (aq), H,O2(aq), and H;O*(aq).

Given that, the mechanism of formation of sulfuric acid from the dissolved SO2 in acid precipitation…

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 for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....

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The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the average rate of disappearance of I- between 400.0 s and 800.0 s in M/s. Determine the average rate of disappearance of I- in the initial 400.0 s in M/s. Determine the average rate of disappearance of I- between 1200.0 s and 1600.0 s in M/s. Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.
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