Balance the following oxidation-reduction equation. The reactions occur in acidic or basic aqueous solution, as indicated.a. Co+ + H2S → Co+ S§ (acidic)O Co2+ + 8H2S → 2Co + Sg + 16H+O Co2+ + 8H2S → 2Co + S§O8C02+ + 8H2S → 8Co + Sg + 16H+b. S? + Cl2 → SOQ² + Cl¯ (basic)S- + 4C12 + 8OH¯ → 8C1¯ + SO4 + 4H20S2-+ 4C12 + 4H2 0 → 8C1¯ + SO4² + 8H+O s + 4C12 + 4H2O → 8C1¯ + SO,²-c. Cr + NO3¯ → Cr(OH)4¯+NH3 (basic)O Cr + 3NO3 + 50H¯ → Cr(OH)4¯+3NH3O8Cr + 3NO3¯ + 23H2O → 8Cr(OH)4¯+3NH3 + 5H+O 8Cr + 3NO3¯+50H¯ + 18H2O → 8Cr(OH)4 + 3NH3d. TcO4 + C20,2 → TcO2 + CO2 (basic)O 2TCO4 + 30C204²- + 8H+ → 2TCO2 + 6CO2 + 4H2OO 2TCO4 +3C204² → 2TCO2 + 6CO2O 2TCO4 +3C204² +4H20 → 2TCO2 + 6CO2 + 80H¯

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Balance the following oxidation-reduction equation. The reactions occur in acidic or basic aqueous solution, as indicated. a. Co+ + H2S → Co+ S§ (acidic) O Co2+ + 8H2S → 2Co + Sg + 16H+ O Co2+ + 8H2S → 2Co+ S8 O8C02+ + 8H2S → 8Co + S8 + 16H+ b. S + Cl2 → SO,² + Cl¯ (basic) S- + 4C12 + 80H¯ → 8C1¯ + SO42 + 4H20 S + 4C12 + 4H2O → 8C1¯ + SO,² + 8H† Os + 4C12 + 4H2O → 8C1 + SO,²- c. Cr + NO3¯ → Cr(OH)4¯ +NH3 (ba O Cr + 3NO3 +50H → Cr(OH)4¯ +3NH3 O8Cr + 3NO3¯ + 23H2O → 8Cr(OH)4¯+3NH3 + 5H+ O 8Cr + 3NO3 +50H¯ +18H2O → 8Cr(OH)4 + 3NH3

Balance the following oxidation-reduction equation. The reactions occur in acidic or basic aqueous solution, as indicated. a. Co+ + H2S → Co+ S§ (acidic) O Co2+ + 8H2S → 2Co + Sg + 16H+ O Co2+ + 8H2S → 2Co+ S8 O8C02+ + 8H2S → 8Co + S8 + 16H+ b. S + Cl2 → SO,² + Cl¯ (basic) S- + 4C12 + 80H¯ → 8C1¯ + SO42 + 4H20 S + 4C12 + 4H2O → 8C1¯ + SO,² + 8H† Os + 4C12 + 4H2O → 8C1 + SO,²- c. Cr + NO3¯ → Cr(OH)4¯ +NH3 (ba O Cr + 3NO3 +50H → Cr(OH)4¯ +3NH3 O8Cr + 3NO3¯ + 23H2O → 8Cr(OH)4¯+3NH3 + 5H+ O 8Cr + 3NO3 +50H¯ +18H2O → 8Cr(OH)4 + 3NH3

Chemistry

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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

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Balance the following oxidation-reduction equation. The reactions occur in acidic or basic aqueous solution, as indicated.
a. Co+ + H2S → Co+ S§ (acidic)
O Co2+ + 8H2S → 2Co + Sg + 16H+
O Co2+ + 8H2S → 2Co + S§
O8C02+ + 8H2S → 8Co + Sg + 16H+
b. S? + Cl2 → SOQ² + Cl¯ (basic)
S- + 4C12 + 8OH¯ → 8C1¯ + SO4 + 4H20
S2-
+ 4C12 + 4H2 0 → 8C1¯ + SO4² + 8H+
O s + 4C12 + 4H2O → 8C1¯ + SO,²-
c. Cr + NO3¯ → Cr(OH)4¯+NH3 (basic)
O Cr + 3NO3 + 50H¯ → Cr(OH)4¯+3NH3
O8Cr + 3NO3¯ + 23H2O → 8Cr(OH)4¯+3NH3 + 5H+
O 8Cr + 3NO3¯+50H¯ + 18H2O → 8Cr(OH)4 + 3NH3
d. TcO4 + C20,2 → TcO2 + CO2 (basic)
O 2TCO4 + 30C204²- + 8H+ → 2TCO2 + 6CO2 + 4H2O
O 2TCO4 +3C204² → 2TCO2 + 6CO2
O 2TCO4 +3C204² +4H20 → 2TCO2 + 6CO2 + 80H¯

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