I included the directions in the picture below To write Spontaneous Redox Reactions:1. Reverse one of the half-rxns into an oxidation step such that the sum of the two 1/2 reactions E°give a positive E cell2. Add the two half-rxns to obtained an overall redox reaction in such a way that the number of electrons cancelfrom both sides of the equation.*NOTE: Changing the "balancing" coefficients of a half-rxn does NOT change the E° value. An electrode potential, Eis an intensive property, one that does not depend on the amount of substance present. The potential is the ratioof energy to charge, when the coefficients are changed (increasing the amount of substance) both the energy andcharge increases proportionally and therefore: the energy to charge ratio does not change: The potential, E°, doesnot change.Examples:1. Hg,Cl2 + 2 e 5 2 Hg + 2 CIE° = + 0.27PBSO, + 2 e 5 Pb + So,?E° = + 0.362. A3* + 3 e 5AlE = - 1.67Br2 + 2 e5 2 BrE° = + 1.09

Cell potential[E°(cell)] is the difference of potential which results in current flow from higher to…

Answered: 1. Reverse one of the half-rxns into an…

1. Reverse one of the half-rxns into an oxidation step such that the sum of the two 1/2 reactions E° give a positive E° cll

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 125AE

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