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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

Chemistry
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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The two half reactions are: OH + HS →S+ + H20 + 2 e Previous Next 3 H20 + Cl03" + 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 H20 + CI" + 6 OH Are there species that appear on both sides of the equation? yes O no 3 OH" +3 HS + 3 H,0 + ClO3 - 3S+ 3 H20 + Cl¯ + 6 OH Subtracting 3 OH" and 3 H20 from each side gives : 3 HS" + Cl03 - 3 S + Cl¯ + 3 OH¯ Is this equation balanced with respect to both mass and charge? yes no
Transcribed Image Text:The two half reactions are: OH + HS →S+ + H20 + 2 e Previous Next 3 H20 + Cl03" + 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 H20 + CI" + 6 OH Are there species that appear on both sides of the equation? yes O no 3 OH" +3 HS + 3 H,0 + ClO3 - 3S+ 3 H20 + Cl¯ + 6 OH Subtracting 3 OH" and 3 H20 from each side gives : 3 HS" + Cl03 - 3 S + Cl¯ + 3 OH¯ Is this equation balanced with respect to both mass and charge? yes no
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