Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →   Ag(s) 0.799 What is the cell potential of the galvanic cell if the concentration of Ag(I) is 0.023 M, Sn(II) is 0.34 M, and Sn(IV) is 0.093 M?

Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →   Ag(s) 0.799 What is the cell potential of the galvanic cell if the concentration of Ag(I) is 0.023 M, Sn(II) is 0.34 M, and Sn(IV) is 0.093 M?

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...
See similar textbooks
icon
Related questions
Question

Consider the following galvanic cell:

 

 

E° (V)

Sn4+  +  2 e−   →   Sn2+

0.139

Ag+  +  e−   →   Ag(s)

0.799

What is the cell potential of the galvanic cell if the concentration of Ag(I) is 0.023 M, Sn(II) is 0.34 M, and Sn(IV) is 0.093 M?

The diagram illustrates a galvanic cell setup commonly used in electrochemistry to demonstrate redox reactions and the flow of electric current. Here’s a detailed explanation of the components: 1. **Electrodes:** - **Sn Electrode (Tin):** On the left side, there is a tin electrode immersed in a solution containing tin ions (Sn²⁺, Sn⁴⁺). - **Ag Electrode (Silver):** On the right side, a silver electrode is immersed in a solution containing silver ions (Ag⁺). 2. **Salt Bridge:** - The salt bridge, labeled KCl, connects the two solutions. It is usually a U-shaped tube filled with a salt solution (potassium chloride in this case) that allows the flow of ions to maintain electrical neutrality in both compartments. 3. **Circuit:** - A wire connects the electrodes, allowing electrons to flow from the tin electrode to the silver electrode. This external circuit also includes a device, possibly a voltmeter or a load, that measures or utilizes the flow of electrons. **Function:** - In this cell, the tin electrode undergoes oxidation, losing electrons, while the silver ions gain electrons and reduce at the silver electrode. This transfer of electrons generates an electric current, which can be harnessed to do work. This setup is an example of a galvanic cell where a spontaneous redox reaction occurs, converting chemical energy into electrical energy.
Transcribed Image Text:The diagram illustrates a galvanic cell setup commonly used in electrochemistry to demonstrate redox reactions and the flow of electric current. Here’s a detailed explanation of the components: 1. **Electrodes:** - **Sn Electrode (Tin):** On the left side, there is a tin electrode immersed in a solution containing tin ions (Sn²⁺, Sn⁴⁺). - **Ag Electrode (Silver):** On the right side, a silver electrode is immersed in a solution containing silver ions (Ag⁺). 2. **Salt Bridge:** - The salt bridge, labeled KCl, connects the two solutions. It is usually a U-shaped tube filled with a salt solution (potassium chloride in this case) that allows the flow of ions to maintain electrical neutrality in both compartments. 3. **Circuit:** - A wire connects the electrodes, allowing electrons to flow from the tin electrode to the silver electrode. This external circuit also includes a device, possibly a voltmeter or a load, that measures or utilizes the flow of electrons. **Function:** - In this cell, the tin electrode undergoes oxidation, losing electrons, while the silver ions gain electrons and reduce at the silver electrode. This transfer of electrons generates an electric current, which can be harnessed to do work. This setup is an example of a galvanic cell where a spontaneous redox reaction occurs, converting chemical energy into electrical energy.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Electrolysis
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS