When [Cu2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 2.806 V. What is the Mg2+ concentration in this cell? Cu²+ (aq) + Mg(s) →→→ Cu(s) + Mg²+ (aq)

When [Cu2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 2.806 V. What is the Mg2+ concentration in this cell? Cu²+ (aq) + Mg(s) →→→ Cu(s) + Mg²+ (aq)

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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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

When [Cu²+] = 1.49 M, the observed cell potential at 298 K for an
electrochemical cell with the reaction shown below is 2.806 V. What is the
Mg2+ concentration in this cell?
2+
Cu²+ (aq) + Mg(s)→→ Cu(s) + Mg²+ (aq)
[Mg2+1 = 8.11x10^-5 X mol/L

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