The two half reactions are: OH + HS¯ → S+ H2O + 2 e Previous Next 3 H20 + ClO3 + 6 e" → Cl¯ + 6 OH¯ The oxidation half-reaction needs to be multiplied by a constant so that the two can be added to cancel the overall charge. By what factor must the oxidation half-reaction be multiplied? Factor = | Multiplying the oxidation half reaction by 3, adding the two together and cancelling the electrons gives: 3 OH + 3 HS + 3 H,0 + Cl03 -3S+3 H,0 + Cl¯ + 6 OH Are there species that appear on both sides of the equation? O yes no 3 OH" + 3 HS" + 3 H20 + C1O3¯ → 3S+ 3 H2O + Cl¯ + 6 OH Subtracting 3 OH and 3 H20 from each side gives : 3 HS + ClO3 - 3S + Cl¯ + 3 OH¯ Is this equation balanced with respect to both mass and charge? O yes O no
The two half reactions are: OH + HS¯ → S+ H2O + 2 e Previous Next 3 H20 + ClO3 + 6 e" → Cl¯ + 6 OH¯ The oxidation half-reaction needs to be multiplied by a constant so that the two can be added to cancel the overall charge. By what factor must the oxidation half-reaction be multiplied? Factor = | Multiplying the oxidation half reaction by 3, adding the two together and cancelling the electrons gives: 3 OH + 3 HS + 3 H,0 + Cl03 -3S+3 H,0 + Cl¯ + 6 OH Are there species that appear on both sides of the equation? O yes no 3 OH" + 3 HS" + 3 H20 + C1O3¯ → 3S+ 3 H2O + Cl¯ + 6 OH Subtracting 3 OH and 3 H20 from each side gives : 3 HS + ClO3 - 3S + Cl¯ + 3 OH¯ Is this equation balanced with respect to both mass and charge? O yes O no
Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Mark S. Cracolice, Ed Peters
Chapter19: Oxidation-reduction(electron Transfer) Reactions
Section: Chapter Questions
Problem 11E
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