**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.

We have to write the balanced reduction half reaction : Fe3+ ----> Fe

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Write a balanced half-reaction describing the reduction of aqueous iron(III) cations to solid iron. 0 ローロ X 90

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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

**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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