Suppose the galvanic cell sketched below is powered by the following reaction: Mg(s) + Zn (NO3)₂(aq) Mg(NO3)₂(aq) + Zn(s) E1 S1 - Write a balanced equation for the half-reaction that happens at the cathode of this cell. E2 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? S2 0 0 0 0 0-0 Do X 0,0,... e lo 4 c.

Suppose the galvanic cell sketched below is powered by the following reaction: Mg(s) + Zn (NO3)₂(aq) Mg(NO3)₂(aq) + Zn(s) E1 S1 - Write a balanced equation for the half-reaction that happens at the cathode of this cell. E2 Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2? S2 0 0 0 0 0-0 Do X 0,0,... e lo 4 c.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 97AP

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Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.
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