3. Using the Nernst Equation, show the calculation for the expected voltage (Eheo) for the voltaic cells below comprised of the following half-cells. The temperature in the lab was 26.5 "C. a. 0.0400 M CuSo.(aq) and 0.0500 M ZnSO,(aq) Etheo =. %3D b. 0.0400 M CuSo.(aq) and 0.0300 M Pb(NO3);(aq) Etheo= %3D 0.0300 M Pb(NO3)2(aq) and 0.0500 M ZnSO,(aq) C. Etheo =

3. Using the Nernst Equation, show the calculation for the expected voltage (Eheo) for the voltaic cells below comprised of the following half-cells. The temperature in the lab was 26.5 "C. a. 0.0400 M CuSo.(aq) and 0.0500 M ZnSO,(aq) Etheo =. %3D b. 0.0400 M CuSo.(aq) and 0.0300 M Pb(NO3);(aq) Etheo= %3D 0.0300 M Pb(NO3)2(aq) and 0.0500 M ZnSO,(aq) C. Etheo =

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.49QE: A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt...

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A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.