Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+FeCl,(aq) - - ZnCl,(aq)+Fe(s) E1 E2 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is El made? Of what substance is E2 made? what are the chemical species in solution SI? What are the chemical species in solution S2?

Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+FeCl,(aq) - - ZnCl,(aq)+Fe(s) E1 E2 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is El made? Of what substance is E2 made? what are the chemical species in solution SI? What are the chemical species in solution S2?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 89QAP: An electrolysis experiment is performed to determine the value of the Faraday constant (number of...

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Question

Suppose the galvanic cell sketched below is powered by the following reaction:
Zn(s)+FeCl,(aq) -
- ZnCl,(aq)+Fe(s)
E1
E2
S1
S2
Write a balanced equation for the half-reaction
that happens at the cathode of this cell.
Write a balanced equation for the half-reaction
that happens at the anode of this cell.
Of what substance is El made?
Of what substance is E2 made?
what are the chemical species in solution SI?
What are the chemical species in solution S2?

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An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
Consider a galvanic cell based on the following half-reactions: a. What is the standard potential for this cell? b. A nonstandard cell is set up at 25C with [Mg2+] = 1.00 105 M. The cell potential is observed to be 4.01 V. Calculate [Au3+] in this cell.
An electrode is prepared by dipping a silver strip into a solution saturated with silver thiocyanate, AgSCN, and containing 0.10 M SCN . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.45 V. What is the solubility product of silver thiocyanate?
Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)
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