Balance the following oxidation-reduction reactions that occur in acidic solution using the half-reaction method. (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 H₂O or H* to any side of the reaction if it is needed. Fe²+ (aq) + MnO4 (aq) → Fe³+ (aq) + Mn²+ (aq) a. b. - → Fe²+ (aq) + MnO4 (aq) + Fe³+ (aq) + Mn²+ (aq) + As2O3 (8) + NO3(aq) → H3 AsO4 (aq) + NO(g) As₂O3 (8) + NO3(aq) + H3 AsO4 (aq) + + NO(g) + + + +

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Balance the following oxidation-reduction reactions that occur in acidic solution using the half-reaction method.
(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 H₂O or H+ to any side of the reaction if it is needed.)
a.
b.
2+
3+
Fe²+ (aq) + MnO4¯¯ (aq) → Fe³+ (aq) + Mn²+ (aq)
Fe²+ (aq) +
MnO4 (aq) +
2+
Fe³+ (aq) +
Mn²+ (aq) +
As2O3 (s) + NO3¯¯ (aq) → H3 AsO4 (aq) + NO(g)
As2O3(s) +
NO3(aq) +
H3 AsO4 (aq) +
+
NO(g) +
+
Transcribed Image Text:Balance the following oxidation-reduction reactions that occur in acidic solution using the half-reaction method. (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 H₂O or H+ to any side of the reaction if it is needed.) a. b. 2+ 3+ Fe²+ (aq) + MnO4¯¯ (aq) → Fe³+ (aq) + Mn²+ (aq) Fe²+ (aq) + MnO4 (aq) + 2+ Fe³+ (aq) + Mn²+ (aq) + As2O3 (s) + NO3¯¯ (aq) → H3 AsO4 (aq) + NO(g) As2O3(s) + NO3(aq) + H3 AsO4 (aq) + + NO(g) + +
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