4. Lead-acid batteries are used in automobiles. The oxidation and reduction half-reactions are: Pb(s) + HSO4 → PbSO4(s) + H* + 2 e PbO2(s) + 3 H* + HSO4 + 2 e → PBSO4(s) + 2 H2O(1) E° = +0.356 V E° = +1.685 V %3D a. Write out the complete balanced redox equation and calculate its standard potential (E°). b. Write out the reaction quotient expression (Q) for this system.

4. Lead-acid batteries are used in automobiles. The oxidation and reduction half-reactions are: Pb(s) + HSO4 → PbSO4(s) + H* + 2 e PbO2(s) + 3 H* + HSO4 + 2 e → PBSO4(s) + 2 H2O(1) E° = +0.356 V E° = +1.685 V %3D a. Write out the complete balanced redox equation and calculate its standard potential (E°). b. Write out the reaction quotient expression (Q) for this system.

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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