**Use Measured Cell Potential to Calculate Concentration**When \([ \text{Hg}^{2+} ] = 1.46 \, \text{M}\), the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is \(2.150 \, \text{V}\). What is the \(\text{Mn}^{2+}\) concentration in this cell?\[\text{Hg}^{2+} \, (\text{aq}) + \text{Mn} \, (\text{s}) \rightarrow \text{Hg} \, (\text{l}) + \text{Mn}^{2+} \, (\text{aq})\]\[[ \text{Mn}^{2+} ] = \, \boxed{\phantom{M}}\]

Given, Hg2+(aq) +Mn(s)→Hg(l) +Mn2+(aq) [Hg2+]=1.46MEcell=2.150 V

Use measured cell potential to calculate concentration. When [ Hg2+ ] = 1.46 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.150 V. What is the Mn2+ concentration in this cell? Hg2+ (aq) + Mn (s) Hg (1) + Mn²+ (aq) [ Mn²+ ] = M

Use measured cell potential to calculate concentration. When [ Hg2+ ] = 1.46 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.150 V. What is the Mn2+ concentration in this cell? Hg2+ (aq) + Mn (s) Hg (1) + Mn²+ (aq) [ Mn²+ ] = M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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