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: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section17.3: Voltaic Cells
Problem 17.3PSP
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