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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 Ag+ concentration is 6.84 x 104 M and the Zn2+ concentration is 1.12 M? 2Ag+ (aq) +Zn(s) 2Ag(s) + Zn2+ (aq) Ecell Ag (aq) + e Ag(s) E Zn2+ (aq) + 2eZn(s) E red = 0.799 V red = -0.763 V V The cell reaction as written above is spontaneous for the concentrations given: true false

What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Ag+ concentration is 6.84 x 104 M and the Zn2+ concentration is 1.12 M? 2Ag+ (aq) +Zn(s) 2Ag(s) + Zn2+ (aq) Ecell Ag (aq) + e Ag(s) E Zn2+ (aq) + 2eZn(s) E red = 0.799 V red = -0.763 V V The cell reaction as written above is spontaneous for the concentrations given: true false

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 50QRT
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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 Ag+ concentration is 6.84 x 104 M and the Zn2+ concentration is 1.12 M? 2Ag+ (aq) +Zn(s) 2Ag(s) + Zn2+ (aq) Ecell Ag (aq) + e Ag(s) E Zn2+ (aq) + 2eZn(s) E red = 0.799 V red = -0.763 V V The cell reaction as written above is spontaneous for the concentrations given: true false
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 Ag+ concentration is 6.84 x 104 M and the Zn2+ concentration is 1.12 M? 2Ag+ (aq) +Zn(s) 2Ag(s) + Zn2+ (aq) Ecell Ag (aq) + e Ag(s) E Zn2+ (aq) + 2eZn(s) E red = 0.799 V red = -0.763 V V The cell reaction as written above is spontaneous for the concentrations given: true false
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