Homework Help is Here – Start Your Trial Now!
Science
Chemistry
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu(aq) + e MnO4(aq) + 2 H₂O(1)+3e + Cu (aq) MnO₂(s) + 4 OH (aq) standard reduction potential = +0.153 V red Ered = +0.59 V

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu(aq) + e MnO4(aq) + 2 H₂O(1)+3e + Cu (aq) MnO₂(s) + 4 OH (aq) standard reduction potential = +0.153 V red Ered = +0.59 V

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
100%
### Galvanic Cell Design using Copper and Manganese Half-Reactions In the design of a galvanic cell, a chemist utilizes the following two half-reactions, each with specified standard reduction potentials. | **Half-Reaction** | **Standard Reduction Potential** | |------------------------------------------------------|----------------------------------------| | Cu<sup>2+</sup>(aq) + e<sup>-</sup> → Cu<sup>+</sup>(aq) | \( E^\circ_{red} = +0.153 \, \text{V} \) | | MnO<sub>4</sub><sup>-</sup>(aq) + 2 H<sub>2</sub>O(l) + 3 e<sup>-</sup> → MnO<sub>2</sub>(s) + 4 OH<sup>-</sup>(aq) | \( E^\circ_{red} = +0.59 \, \text{V} \) | #### Table Explanation: - **Half-Reaction Column**: This column lists the chemical reactions where reduction occurs (gaining electrons). - **Standard Reduction Potential Column**: This column lists the standard reduction potential (E<sup>0</sup><sub>red</sub>) for each half-reaction in volts (V), describing the tendency of each species to gain electrons and be reduced. **Key concepts**: - **Reduction Potential**: A measure of the tendency of a chemical species to acquire electrons and thereby be reduced. The higher the value, the greater the species' affinity for electrons. - **Standard Conditions**: Typically refer to a solution at 1 M concentration, 25°C temperature, and 1 atm pressure. In the galvanic cell designed here, the MnO<sub>4</sub><sup>-</sup> reaction has a higher reduction potential and will act as the cathode. The Cu<sup>2+</sup> reaction, with a lower reduction potential, will act as the anode. This setup ensures the spontaneous flow of electrons from the anode to the cathode, generating electric current. This example illustrates how understanding standard reduction potentials aids in predicting the direction of redox reactions and designing efficient electrochemical cells.
Transcribed Image Text:### Galvanic Cell Design using Copper and Manganese Half-Reactions In the design of a galvanic cell, a chemist utilizes the following two half-reactions, each with specified standard reduction potentials. | **Half-Reaction** | **Standard Reduction Potential** | |------------------------------------------------------|----------------------------------------| | Cu<sup>2+</sup>(aq) + e<sup>-</sup> → Cu<sup>+</sup>(aq) | \( E^\circ_{red} = +0.153 \, \text{V} \) | | MnO<sub>4</sub><sup>-</sup>(aq) + 2 H<sub>2</sub>O(l) + 3 e<sup>-</sup> → MnO<sub>2</sub>(s) + 4 OH<sup>-</sup>(aq) | \( E^\circ_{red} = +0.59 \, \text{V} \) | #### Table Explanation: - **Half-Reaction Column**: This column lists the chemical reactions where reduction occurs (gaining electrons). - **Standard Reduction Potential Column**: This column lists the standard reduction potential (E<sup>0</sup><sub>red</sub>) for each half-reaction in volts (V), describing the tendency of each species to gain electrons and be reduced. **Key concepts**: - **Reduction Potential**: A measure of the tendency of a chemical species to acquire electrons and thereby be reduced. The higher the value, the greater the species' affinity for electrons. - **Standard Conditions**: Typically refer to a solution at 1 M concentration, 25°C temperature, and 1 atm pressure. In the galvanic cell designed here, the MnO<sub>4</sub><sup>-</sup> reaction has a higher reduction potential and will act as the cathode. The Cu<sup>2+</sup> reaction, with a lower reduction potential, will act as the anode. This setup ensures the spontaneous flow of electrons from the anode to the cathode, generating electric current. This example illustrates how understanding standard reduction potentials aids in predicting the direction of redox reactions and designing efficient electrochemical cells.
### Electrochemical Cells: Writing Balanced Equations Here are a series of tasks aimed at formulating and balancing chemical equations pertinent to electrochemical cells: **Task 1: Cathode Half-Reaction** - **Instruction:** Write a balanced equation for the half-reaction that happens at the cathode. - **Response Area:** [ ] **Task 2: Anode Half-Reaction** - **Instruction:** Write a balanced equation for the half-reaction that happens at the anode. - **Response Area:** [ ] **Task 3: Overall Reaction** - **Instruction:** Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. - **Response Area:** [ ] --- By completing these tasks, you will gain a better understanding of the individual and overall reactions that occur in electrochemical cells, which are fundamental components in batteries and various types of fuel cells.
Transcribed Image Text:### Electrochemical Cells: Writing Balanced Equations Here are a series of tasks aimed at formulating and balancing chemical equations pertinent to electrochemical cells: **Task 1: Cathode Half-Reaction** - **Instruction:** Write a balanced equation for the half-reaction that happens at the cathode. - **Response Area:** [ ] **Task 2: Anode Half-Reaction** - **Instruction:** Write a balanced equation for the half-reaction that happens at the anode. - **Response Area:** [ ] **Task 3: Overall Reaction** - **Instruction:** Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. - **Response Area:** [ ] --- By completing these tasks, you will gain a better understanding of the individual and overall reactions that occur in electrochemical cells, which are fundamental components in batteries and various types of fuel cells.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 3 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