When [Ag*] = 1.34 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.534 V. What is the Al3+ concentration in this cell? 3Ag*(aq) + Al(s)→3A9(s) + Al3+(aq) [AI3+] =| M

When [Ag] = 1.34 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.534 V. What is the Al3+ concentration in this cell? 3Ag(aq) + Al(s)→3A9(s) + Al3+(aq) [AI3+] =| M

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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

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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

Use measured cell potential to calculate concentration.
When [Ag*] = 1.34 M, the observed cell potential at 298K for an electrochemical cell with the reaction shown below is 2.534 V. What is the Al3+
concentration in this cell?
3Ag*(aq) + AI(s)→3A9(s) + Al3+(aq)
[Al3+] =
M

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