2. Write the half reactions occurring at the cathode and at the anode when each čllshown in problem #1 is delivering current. Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which of thefollowing reactions occur spontaneously.A Zn+ Ni* → Zn* Ni1.ANODE: Zn Zn* +2eÇATHODE: Ni* + 2e-→ NiVOLTAIC CELL: Zn/Zn* || Ni" /NiB. 2Al + 3Cl,→ 2AICI,ANODE: Al→ Al* + 3eCATHODE: 3Cl, + 6e → 6ClVOLTAIC CELL: Al/ Al || Cl./ClC. H2 + 2Ag+ → 2H +2AgCATHODE: 2Ag + 2e AgANODE: H, → 2H + 2eVOLTAIC CELL: H/H||Ag/Ag

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2. Write the half reactions occurring at the cathode and at the anode when each cell shown in problem #1 is delivering current.

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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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

2. Write the half reactions occurring at the cathode and at the anode when each čll
shown in problem #1 is delivering current.

Represent in the conventional manner, i.e., anode/cathode, the voltaic cell in which of the
following reactions occur spontaneously.
A Zn+ Ni* → Zn* Ni
1.
ANODE: Zn Zn* +2e
ÇATHODE: Ni* + 2e-→ Ni
VOLTAIC CELL: Zn/Zn* || Ni" /Ni
B. 2Al + 3Cl,
→ 2AICI,
ANODE: Al→ Al* + 3e
CATHODE: 3Cl, + 6e → 6Cl
VOLTAIC CELL: Al/ Al || Cl./Cl
C. H2 + 2Ag+ → 2H +2Ag
CATHODE: 2Ag + 2e Ag
ANODE: H, → 2H + 2e
VOLTAIC CELL: H/H||Ag/Ag

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