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


  1. Sn/Sn4+
  2. Sn/Sn2+
  3. Sn2+/Sn4+
  4. Ag/Ag+
**Electrochemical Cell Diagram** This diagram illustrates an electrochemical cell setup with two half-cells connected by a salt bridge. - **Left Half-Cell:** - Contains a tin (Sn) electrode immersed in a solution containing tin ions (Sn²⁺, Sn⁴⁺). - The container is represented as a beaker holding the tin electrode and electrolyte. - **Right Half-Cell:** - Contains a silver (Ag) electrode immersed in a solution of silver ions (Ag⁺). - Similar to the left, it’s shown as a beaker holding the silver electrode and electrolyte. - **Salt Bridge:** - A tube containing potassium chloride (KCl) connects the two half-cells. - It allows the flow of ions to maintain electrical neutrality in the solutions. - **External Circuit:** - Wires connect the two electrodes to an external circuit, depicted here as a circular meter or device. This allows the flow of electrons between the electrodes. This setup demonstrates the principles of redox reactions and electron flow in electrochemical cells, essential for generating electrical energy from chemical reactions.
Transcribed Image Text:**Electrochemical Cell Diagram** This diagram illustrates an electrochemical cell setup with two half-cells connected by a salt bridge. - **Left Half-Cell:** - Contains a tin (Sn) electrode immersed in a solution containing tin ions (Sn²⁺, Sn⁴⁺). - The container is represented as a beaker holding the tin electrode and electrolyte. - **Right Half-Cell:** - Contains a silver (Ag) electrode immersed in a solution of silver ions (Ag⁺). - Similar to the left, it’s shown as a beaker holding the silver electrode and electrolyte. - **Salt Bridge:** - A tube containing potassium chloride (KCl) connects the two half-cells. - It allows the flow of ions to maintain electrical neutrality in the solutions. - **External Circuit:** - Wires connect the two electrodes to an external circuit, depicted here as a circular meter or device. This allows the flow of electrons between the electrodes. This setup demonstrates the principles of redox reactions and electron flow in electrochemical cells, essential for generating electrical energy from chemical reactions.
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