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Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →   Ag(s) 0.799 The cathode is Sn/Sn4+ Sn/Sn2+ Sn2+/Sn4+ Ag/Ag+

Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →   Ag(s) 0.799 The cathode is Sn/Sn4+ Sn/Sn2+ Sn2+/Sn4+ Ag/Ag+

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 cathode is


  1. Sn/Sn4+
  2. Sn/Sn2+
  3. Sn2+/Sn4+
  4. Ag/Ag+
### Electrochemical Cell Diagram This diagram illustrates a galvanic cell, which is a type of electrochemical cell that converts chemical energy into electrical energy through a spontaneous redox reaction. The cell consists of two half-cells connected by a salt bridge containing KCl (potassium chloride). **Components:** 1. **Left Half-Cell:** - **Electrode:** Tin (Sn) electrode. - **Solution:** Contains Sn²⁺ and Sn⁴⁺ ions. - **Reaction:** The tin electrode undergoes oxidation, releasing electrons. 2. **Right Half-Cell:** - **Electrode:** Silver (Ag) electrode. - **Solution:** Contains Ag⁺ ions. - **Reaction:** Silver ions undergo reduction, gaining electrons. 3. **Salt Bridge:** - The U-shaped tube containing KCl allows ions to flow between the two solutions, maintaining charge balance. 4. **External Circuit:** - Connects the two electrodes, allowing electron flow from the tin electrode to the silver electrode. This setup demonstrates the principles of a galvanic cell, where oxidation occurs at the anode (tin electrode) and reduction takes place at the cathode (silver electrode).
Transcribed Image Text:### Electrochemical Cell Diagram This diagram illustrates a galvanic cell, which is a type of electrochemical cell that converts chemical energy into electrical energy through a spontaneous redox reaction. The cell consists of two half-cells connected by a salt bridge containing KCl (potassium chloride). **Components:** 1. **Left Half-Cell:** - **Electrode:** Tin (Sn) electrode. - **Solution:** Contains Sn²⁺ and Sn⁴⁺ ions. - **Reaction:** The tin electrode undergoes oxidation, releasing electrons. 2. **Right Half-Cell:** - **Electrode:** Silver (Ag) electrode. - **Solution:** Contains Ag⁺ ions. - **Reaction:** Silver ions undergo reduction, gaining electrons. 3. **Salt Bridge:** - The U-shaped tube containing KCl allows ions to flow between the two solutions, maintaining charge balance. 4. **External Circuit:** - Connects the two electrodes, allowing electron flow from the tin electrode to the silver electrode. This setup demonstrates the principles of a galvanic cell, where oxidation occurs at the anode (tin electrode) and reduction takes place at the cathode (silver electrode).
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