3 3. Given the following reduction half-reactions:Zn2* (ag) + 2 eZn (s)E°red = -0.763 VPb?*(aq) + 2e →Pb(s)E°red = -0.126 Va) Which one is the anode? Which one is cathode?b) Calculate the E°.cell

Given Zn2+(aq) + 2e- → Zn(s) Ered0 = - 0.763 VPb2+(aq) + 2e- → Pb(s) Ered0 = - 0.126 V

Given the following reduction half-reactions: Zn2 (aq) + 2 e - Pb2*(aq) + 2e – Pb(s) E'red = -0.126 V Zn (s) E°red = -0.763 V a) Which one is the anode? Which one is cathode? b) Calculate the Eºcell

Given the following reduction half-reactions: Zn2 (aq) + 2 e - Pb2*(aq) + 2e – Pb(s) E'red = -0.126 V Zn (s) E°red = -0.763 V a) Which one is the anode? Which one is cathode? b) Calculate the Eºcell

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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Stoichiometry

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Question

3. Given the following reduction half-reactions:
Zn2* (ag) + 2 e
Zn (s)
E°red = -0.763 V
Pb?*(aq) + 2e →
Pb(s)
E°red = -0.126 V
a) Which one is the anode? Which one is cathode?
b) Calculate the E°.
cell

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