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Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →   Ag(s) 0.799 The electron flow is clockwise electrons don't move in this galvanic cell counterclockwise

Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →   Ag(s) 0.799 The electron flow is clockwise electrons don't move in this galvanic cell counterclockwise

Chemistry
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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Consider the following galvanic cell:

 

 

E° (V)

Sn4+  +  2 e−   →   Sn2+

0.139

Ag+  +  e−   →   Ag(s)

0.799

The electron flow is


  1. clockwise
  2. electrons don't move in this galvanic cell
  3. counterclockwise
The image illustrates an electrochemical cell setup, which is a fundamental concept in chemistry, particularly in the study of electrochemistry. **Description of the Setup:** 1. **Electrodes:** - On the left, there is a tin (Sn) electrode immersed in a solution containing tin ions (Sn²⁺, Sn⁴⁺). - On the right, there is a silver (Ag) electrode immersed in a solution containing silver ions (Ag⁺). 2. **Salt Bridge:** - A salt bridge containing potassium chloride (KCl) connects the two solutions. The salt bridge allows the flow of ions to maintain electrical neutrality. 3. **External Circuit:** - The electrodes are connected to an external circuit through wires, enabling the flow of electrons. The flow of electrons constitutes an electric current, which can be used to perform work. 4. **Cell Function:** - In this electrochemical cell, oxidation and reduction reactions occur. Tin (Sn) undergoes oxidation, and silver ions (Ag⁺) are reduced. This process results in the transfer of electrons through the external circuit, creating an electric current. This diagram is a practical representation of how chemical reactions can be harnessed to produce electrical energy, illustrating key principles such as redox reactions, electrode potentials, and the role of a salt bridge in electrochemical cells.
Transcribed Image Text:The image illustrates an electrochemical cell setup, which is a fundamental concept in chemistry, particularly in the study of electrochemistry. **Description of the Setup:** 1. **Electrodes:** - On the left, there is a tin (Sn) electrode immersed in a solution containing tin ions (Sn²⁺, Sn⁴⁺). - On the right, there is a silver (Ag) electrode immersed in a solution containing silver ions (Ag⁺). 2. **Salt Bridge:** - A salt bridge containing potassium chloride (KCl) connects the two solutions. The salt bridge allows the flow of ions to maintain electrical neutrality. 3. **External Circuit:** - The electrodes are connected to an external circuit through wires, enabling the flow of electrons. The flow of electrons constitutes an electric current, which can be used to perform work. 4. **Cell Function:** - In this electrochemical cell, oxidation and reduction reactions occur. Tin (Sn) undergoes oxidation, and silver ions (Ag⁺) are reduced. This process results in the transfer of electrons through the external circuit, creating an electric current. This diagram is a practical representation of how chemical reactions can be harnessed to produce electrical energy, illustrating key principles such as redox reactions, electrode potentials, and the role of a salt bridge in electrochemical cells.
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