Use the References to access important values if needed for this question.Enter electrons as e".Use smallest possible integer coefficients for ALL reactions.If a box is not needed, leave it blank.A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge.2Ag*(aq) + Sn(s) → 2Ag(s) +The anode reaction is:The cathode reaction is:In the external circuit, electrons migrate from v the Ag|Ag" electrode to| the Sn|Sn2* electrode.In the salt bridge, anions migrate to| the AglAg* compartment from v the Sn|Sn2" compartment.Submit AnswerRetry Entire GroupNo more group attempts remain

As we know, Oxidation takes place at anode and reduction takes place at cathode. At anode Sn(s)…

+ Sn(s) → 2Ag(s) + Sn²*(aq) reaction is: de reaction is: mal circuit, electrons migrate from v the AgAg* electrode to v the Sn Sn2* electrod

+ Sn(s) → 2Ag(s) + Sn²(aq) reaction is: de reaction is: mal circuit, electrons migrate from v the AgAg electrode to v the Sn Sn2* electrod

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.

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