Balance the following oxidation-reduction reactions that occur in basic solution. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Add H,O or OH to any side of the reaction if it is needed.) a. Fe(s) + MnO4 (ag) → MnO2(s) + Fe(OH)4 (ag) Fe(s) + MnO4 (aq) + MnO2 (s) + Fe(OH)4 (aq) + b. Br2 (1) → Br (aq) + OBr (aq) Br2 (1) + Br (aq) ОВг (aд) + NO2 (ag) + Al(s) NH3 (g) + AlO2 (aq) NO2 (aq) + Al(s) + NH3 (s) + AlO2 (aq) +
Balance the following oxidation-reduction reactions that occur in basic solution. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Add H,O or OH to any side of the reaction if it is needed.) a. Fe(s) + MnO4 (ag) → MnO2(s) + Fe(OH)4 (ag) Fe(s) + MnO4 (aq) + MnO2 (s) + Fe(OH)4 (aq) + b. Br2 (1) → Br (aq) + OBr (aq) Br2 (1) + Br (aq) ОВг (aд) + NO2 (ag) + Al(s) NH3 (g) + AlO2 (aq) NO2 (aq) + Al(s) + NH3 (s) + AlO2 (aq) +
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section: Chapter Questions
Problem 1PS: Write balanced equations for the following half-reactions. Specify whether each is an oxidation or...
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Transcribed Image Text:Balance the following oxidation-reduction reactions that occur in basic solution.
(Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. Add H,O or OH" to any side of the reaction if it is needed.)
a.
Fe(s) + MnO4¯(ag) → MnO2(s) + Fe(OH)4¯(ag)
Fe(s) +
MnO4 (aq) +
MnO2 (s) +
Fe(OH)4 (aq) +
b.
Br2 (1) → Br (aq) + OB1¯(aq)
Br2 (1) +
+
Br (aq)
OBr (ag) +
NO2 (ag) + Al(s) → NH3 (g) + AlO2 (ag)
NO2 (aq) +
Al(s) +
NH3(s) +
A1O2 (aq) +
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