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When the Ag concentration is 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.078 V. What is the Mn²+ concentration? 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag+ (aq) + e → Ag(s) = 0.799 V Mn2+ (aq) + 2e → Mn(s) [Mn²+] = M 1 Eº red EO red __ -1.180 V

When the Ag concentration is 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.078 V. What is the Mn²+ concentration? 2+ 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag+ (aq) + e → Ag(s) = 0.799 V Mn2+ (aq) + 2e → Mn(s) [Mn²+] = M 1 Eº red EO red __ -1.180 V

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.87QP: Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4]...
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When the Ag concentration is 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.078 V. What is the Mn2+ concentration? 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag+ (aq) + e → Ag(s) = 0.799 V Mn2+ (aq) + 2e → Mn(s) [Mn²+] = M 10000 Eº red Eº red - -1.180 V -
Transcribed Image Text:When the Ag concentration is 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.078 V. What is the Mn2+ concentration? 2Ag+ (aq) + Mn(s) → 2Ag(s) + Mn²+ (aq) Ag+ (aq) + e → Ag(s) = 0.799 V Mn2+ (aq) + 2e → Mn(s) [Mn²+] = M 10000 Eº red Eº red - -1.180 V -
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