Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained …
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I also need the net ionic equation 

### Electrochemistry: Redox Reactions and Cell Potentials #### Example a: Iron (Fe) in Zinc Sulfate (ZnSO₄) Solution To analyze the redox reaction and determine the cell potential for iron (Fe) in a zinc sulfate (ZnSO₄) solution, use the following standard reduction potentials: - **Fe²⁺/Fe**: -0.44 V - **Zn²⁺/Zn**: -0.76 V **Standard Reduction Potentials Table:** | **Standard reduction potential (V)** | **Standard reduction potential (V)** | |---------------------------------------|---------------------------------------| | Fe²⁺/Fe: -0.44 | Zn²⁺/Zn: -0.76 | **Redox Reaction:** - The species with the higher (less negative) reduction potential will be reduced. - The species with the lower (more negative) reduction potential will be oxidized. **Cell Potential Calculation:** 1. **Identify the half-reactions:** - Reduction: Fe²⁺ + 2e⁻ → Fe (E° = -0.44 V) - Oxidation: Zn → Zn²⁺ + 2e⁻ (E° = -0.76 V) 2. **Calculate the cell potential:** - Cell Potential (E°cell) = Reduction potential (cathode) - Oxidation potential (anode) - E°cell = (-0.44 V) - (-0.76 V) - E°cell = 0.32 V Therefore, the overall redox reaction for Fe in ZnSO₄ solution can be written, and the cell potential is 0.32 V. #### Diagrams or Graphs Explanation: In this context, the table provided lists standard reduction potentials for Fe²⁺/Fe and Zn²⁺/Zn half-reactions, and there are blank spaces for writing the overall redox reaction and calculating the cell potential based on these values. This setup is useful for students to practice identifying and calculating standard cell potentials for various electrochemical cells. Demonstrating the relationship between the standard reduction potentials of different metals and how to determine the overall cell potential for a spontaneous redox reaction is critical in understanding electrochemistry.
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Transcribed Image Text:### Electrochemistry: Redox Reactions and Cell Potentials #### Example a: Iron (Fe) in Zinc Sulfate (ZnSO₄) Solution To analyze the redox reaction and determine the cell potential for iron (Fe) in a zinc sulfate (ZnSO₄) solution, use the following standard reduction potentials: - **Fe²⁺/Fe**: -0.44 V - **Zn²⁺/Zn**: -0.76 V **Standard Reduction Potentials Table:** | **Standard reduction potential (V)** | **Standard reduction potential (V)** | |---------------------------------------|---------------------------------------| | Fe²⁺/Fe: -0.44 | Zn²⁺/Zn: -0.76 | **Redox Reaction:** - The species with the higher (less negative) reduction potential will be reduced. - The species with the lower (more negative) reduction potential will be oxidized. **Cell Potential Calculation:** 1. **Identify the half-reactions:** - Reduction: Fe²⁺ + 2e⁻ → Fe (E° = -0.44 V) - Oxidation: Zn → Zn²⁺ + 2e⁻ (E° = -0.76 V) 2. **Calculate the cell potential:** - Cell Potential (E°cell) = Reduction potential (cathode) - Oxidation potential (anode) - E°cell = (-0.44 V) - (-0.76 V) - E°cell = 0.32 V Therefore, the overall redox reaction for Fe in ZnSO₄ solution can be written, and the cell potential is 0.32 V. #### Diagrams or Graphs Explanation: In this context, the table provided lists standard reduction potentials for Fe²⁺/Fe and Zn²⁺/Zn half-reactions, and there are blank spaces for writing the overall redox reaction and calculating the cell potential based on these values. This setup is useful for students to practice identifying and calculating standard cell potentials for various electrochemical cells. Demonstrating the relationship between the standard reduction potentials of different metals and how to determine the overall cell potential for a spontaneous redox reaction is critical in understanding electrochemistry.
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