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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A solution contains 0.2 mol/l of the salt ammonium acetate (NH+4CH3COO-). The pH of the solution has been adjusted to 8.0 via addition of NaOH. The equilibrium constants for the deprotonation of acetic acid and the ammonium ion are: NH+4(aq)+H2O(l) = NH3(aq)+H3O+(aq) pKa1=9.25 CH3COOH(aq)+H2O(1)= CH3COO-(aq)+H3O+(aq) pKa2=4.75 1. Calculate the concentration of ammonia (NH3NH3) in the solution. 2. Calculate the concentration of acetate ions (CH3COO-CH3COO-) in the solution. 3. Calculate the concentration of non-dissociated acetic acid (CH3COOHCH3COOH) in the solution. 4. Calculate the concentration of sodium ions in the solution. 5. Calculate the pH of a solution containing the same amount of NaOH in absence of ammonium acetate. 6. Calculate the pH of a 0.2 mol/l ammonium acetate solution, if no NaOH is added.
With the information provided below, calculate the enthalpy of reduction, AredHº, for the reaction: Sr2*(aq) → Sr(s), and comment on the sign of the obtained magnitude given the properties of the alkaline-earth elements (i.e.: metallic character, reduction potentials, etc.). (hint: Hess' law should come in handy) Show your work AatH® (kJ/mol) AnyaH® (kJ/mol) IE: (kJ/mol) IE2 (kJ/mol) Element Sr 164 -1456 549.5 1064 AatHº: enthalpy of atomization; AnyaH®: enthalpy of hydration; IE1: first ionization energy; IE2: second ionization energy 2.
How many grams of silver can be plated onto an object in 7.46 minutes at 3.07 A of current? Ag+ (aq) +e → ► Ag(s) Your Answer: Answer units
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ezto.mheducation.com/ext/map/index.html?_con3con&external_browser=0&launchUrl=https%25 pter 19 Sa Enter your answer in the provided box. Given the following data, ts 2H9²*(aq) + 2e→ Hg,“(aq) E = 0.92 V eBook Hg,"(aq) + 2e¯ → 2Hg(l) E = 0.85 V ferences calculate AG for the following process at 25°C: Hg,"(aq) → Hg²*(aq) + Hg(1) kJ / mol raw < Prev e here to search 2.
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