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When the Hg2+ concentration is 1.18 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.134V. What is the Mn2+ concentration? Hg2*(aq) + Mn(s) Hg(1) + Mn²+*(aq) Answer: M

When the Hg2+ concentration is 1.18 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.134V. What is the Mn2+ concentration? Hg2*(aq) + Mn(s) Hg(1) + Mn²+*(aq) Answer: M

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 Hg2+ concentration is 1.18 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.134V. What is the Mn2+ concentration? Hg2+(aq) + Mn(s)- → Hg(1) + Mn²+(aq) Answer: M
Transcribed Image Text:When the Hg2+ concentration is 1.18 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.134V. What is the Mn2+ concentration? Hg2+(aq) + Mn(s)- → Hg(1) + Mn²+(aq) Answer: M
Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Hg2*(aq) + 21(aq)- → Hg(1) + I2(s) Answer: kJ K for this reaction would be than one.
Transcribed Image Text:Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: Hg2*(aq) + 21(aq)- → Hg(1) + I2(s) Answer: kJ K for this reaction would be than one.
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