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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![**Transcription and Explanation for Educational Website**
**Instruction:**
Write a balanced half-reaction describing the reduction of aqueous iron(III) cations to solid iron.
**Input Box:**
- A blank input box is provided for entering the balanced half-reaction equation.
**Symbol Options:**
- An interface with options for inserting squared brackets and arrows to indicate chemical states and reactions.
- A symbol for an electron, \( e^- \), is provided, which is commonly used in redox reactions to indicate the gaining of electrons.
### Detailed Explanation
**Reduction Reaction:**
When balancing the half-reaction for the reduction of iron(III) cations (\( \text{Fe}^{3+} \)) to solid iron (\( \text{Fe} \)), electrons are added to the equation to balance the charges. The general form of the balanced reduction half-reaction is:
\[ \text{Fe}^{3+} + 3e^- \rightarrow \text{Fe} \]
- **\(\text{Fe}^{3+}\):** Represents the iron(III) cation, which has a charge of +3.
- **\(3e^-\):** Represents the electrons that are gained in the reduction process.
- **\(\rightarrow \text{Fe}\):** The arrow indicates the direction of the reaction, showing that iron cations are reduced to form solid iron.
This balanced equation shows that three electrons are required to reduce one iron(III) ion to metallic iron. Understanding this reaction is fundamental in electrochemistry, particularly in processes like corrosion, metallurgy, and electroplating.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2e8de085-3521-4e76-9213-315082e7bc47%2F30ab4d2d-62a1-4ba1-bea1-7f2be5c2201b%2Flwuwoov_processed.png&w=3840&q=75)
Transcribed Image Text:**Transcription and Explanation for Educational Website**
**Instruction:**
Write a balanced half-reaction describing the reduction of aqueous iron(III) cations to solid iron.
**Input Box:**
- A blank input box is provided for entering the balanced half-reaction equation.
**Symbol Options:**
- An interface with options for inserting squared brackets and arrows to indicate chemical states and reactions.
- A symbol for an electron, \( e^- \), is provided, which is commonly used in redox reactions to indicate the gaining of electrons.
### Detailed Explanation
**Reduction Reaction:**
When balancing the half-reaction for the reduction of iron(III) cations (\( \text{Fe}^{3+} \)) to solid iron (\( \text{Fe} \)), electrons are added to the equation to balance the charges. The general form of the balanced reduction half-reaction is:
\[ \text{Fe}^{3+} + 3e^- \rightarrow \text{Fe} \]
- **\(\text{Fe}^{3+}\):** Represents the iron(III) cation, which has a charge of +3.
- **\(3e^-\):** Represents the electrons that are gained in the reduction process.
- **\(\rightarrow \text{Fe}\):** The arrow indicates the direction of the reaction, showing that iron cations are reduced to form solid iron.
This balanced equation shows that three electrons are required to reduce one iron(III) ion to metallic iron. Understanding this reaction is fundamental in electrochemistry, particularly in processes like corrosion, metallurgy, and electroplating.
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