Copper metal and zinc metal will both reduce Ag+ ions under standard state conditions. Which metal when used as an electrode in a galvanic cell will have the larger Eºcell? Show your work. (Hint: Write the two possible chemical reactions.) Standard Reduction Potentials: Ag+ (aq) + e¯ ⇒ Ag(s) Cu²+ (aq) + 2e Cu(s) ⇒ Zn²+ (aq) + 2e¯ ⇒ Zn(s) E E E cell - substance reduced - substance oxidized A +0.80 +0.34 -0.76

Copper metal and zinc metal will both reduce Ag+ ions under standard state conditions. Which metal when used as an electrode in a galvanic cell will have the larger Eºcell? Show your work. (Hint: Write the two possible chemical reactions.) Standard Reduction Potentials: Ag+ (aq) + e¯ ⇒ Ag(s) Cu²+ (aq) + 2e Cu(s) ⇒ Zn²+ (aq) + 2e¯ ⇒ Zn(s) E E E cell - substance reduced - substance oxidized A +0.80 +0.34 -0.76

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 86E: An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.0...

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Concept explainers

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

Copper metal and zinc metal will both reduce Ag+ ions under standard
state conditions. Which metal when used as an electrode in a galvanic
cell will have the larger Eºcell? Show your work. (Hint: Write the two
possible chemical reactions.)
Standard Reduction Potentials:
Ag+ (aq) + e¯ = Ag(s)
Cu²+ (aq) +2e=Cu(s)
Zn²+ (aq) + 2e¯ ⇒ Zn(s)
-E
E
cell
= E
substance reduced
substance oxidized
L
+0.80
+0.34
-0.76

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