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What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Agt concentration is 1.09 M and the Zn² concentration is 7.69 x 10-4 M? 2Ag+ (aq) + Zn(s) → 2Ag(s) + Zn²+ (aq) 0.799 V Ag (aq) + e → Ag(s) E Zn²+ red (aq) + 2e → Zn(s) E red -0.763 V Ecell = The cell reaction as written above is spontaneous for the concentrations given: O true O false V

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Agt concentration is 1.09 M and the Zn² concentration is 7.69 x 10-4 M? 2Ag+ (aq) + Zn(s) → 2Ag(s) + Zn²+ (aq) 0.799 V Ag (aq) + e → Ag(s) E Zn²+ red (aq) + 2e → Zn(s) E red -0.763 V Ecell = The cell reaction as written above is spontaneous for the concentrations given: O true O false V

Fundamentals Of Analytical Chemistry
Fundamentals Of Analytical Chemistry
9th Edition
ISBN:9781285640686
Author:Skoog
Publisher:Skoog
Chapter19: Applications Of Standard Electrode Potentials
Section: Chapter Questions
Problem 19.8QAP
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What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Agt concentration is 1.09 M and the Zn² concentration is 7.69 x 10-4 M? 2Ag+ (aq) + Zn(s) → 2Ag(s) + Zn²+ (aq) 0.799 V Ag (aq) + e → Ag(s) E Zn²+ red (aq) + 2e → Zn(s) E red = Ecell The cell reaction as written above is spontaneous for the concentrations given: O true O false -0.763 V V
Transcribed Image Text:What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Agt concentration is 1.09 M and the Zn² concentration is 7.69 x 10-4 M? 2Ag+ (aq) + Zn(s) → 2Ag(s) + Zn²+ (aq) 0.799 V Ag (aq) + e → Ag(s) E Zn²+ red (aq) + 2e → Zn(s) E red = Ecell The cell reaction as written above is spontaneous for the concentrations given: O true O false -0.763 V V
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