A. Using the following standard reduction potentials: Ag* (aq) +e = Ag (s) Pb2* (aq) + 2e= Pb (s) E° = +0.80 V E° = -0.13 V Write a balanced redox reaction that represents the overall cell reaction for the feasible galvanic cell. i. ii. Calculate the standard cell potential. iii. Draw a fully labelled galvanic cell for this redox system. Your labels should show (but not limited to): the electron and ion flow; the anode and cathode, the half cells where oxidation and reduction take place.

A. Using the following standard reduction potentials: Ag* (aq) +e = Ag (s) Pb2* (aq) + 2e= Pb (s) E° = +0.80 V E° = -0.13 V Write a balanced redox reaction that represents the overall cell reaction for the feasible galvanic cell. i. ii. Calculate the standard cell potential. iii. Draw a fully labelled galvanic cell for this redox system. Your labels should show (but not limited to): the electron and ion flow; the anode and cathode, the half cells where oxidation and reduction take place.

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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