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Write a balanced half-reaction for the oxidation of solid manganese dioxide (MnO₂) to permanganate ion (MnO4) in acidic aqueous solution. Be sure to add physical state symbols where appropriate.

Write a balanced half-reaction for the oxidation of solid manganese dioxide (MnO₂) to permanganate ion (MnO4) in acidic aqueous solution. Be sure to add physical state symbols where appropriate.

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...
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**Understanding Half-Reactions: Manganese Dioxide Oxidation** **Objective:** Learn to write a balanced half-reaction for the oxidation of solid manganese dioxide (MnO₂) to permanganate ion (MnO₄⁻) in acidic aqueous solution, including physical state symbols. **Step-by-Step Guide:** 1. **Identify Reactants and Products:** - Reactant: Solid manganese dioxide (MnO₂, s) - Product: Permanganate ion (MnO₄⁻, aq) 2. **Understanding the Reaction Conditions:** - The reaction occurs in an acidic aqueous solution, indicating the presence of protons (H⁺, aq). 3. **Balancing the Half-Reaction:** - **Mass Balance:** Ensure the number of Mn atoms and O atoms is the same on both sides. - **Charge Balance:** Adjust for charge with electrons (e⁻). 4. **Incorporate Physical State Symbols:** - Indicate MnO₂ as solid (s) and MnO₄⁻ as aqueous (aq). **Outcome:** The balanced half-reaction combines mass and charge conservation, factoring in additional H₂O and H⁺ molecules needed to balance O and H atoms. **Conclusion:** Writing balanced half-reactions requires attention to detail in stoichiometry and electron transfer, fundamental in understanding redox processes in chemistry.
Transcribed Image Text:**Understanding Half-Reactions: Manganese Dioxide Oxidation** **Objective:** Learn to write a balanced half-reaction for the oxidation of solid manganese dioxide (MnO₂) to permanganate ion (MnO₄⁻) in acidic aqueous solution, including physical state symbols. **Step-by-Step Guide:** 1. **Identify Reactants and Products:** - Reactant: Solid manganese dioxide (MnO₂, s) - Product: Permanganate ion (MnO₄⁻, aq) 2. **Understanding the Reaction Conditions:** - The reaction occurs in an acidic aqueous solution, indicating the presence of protons (H⁺, aq). 3. **Balancing the Half-Reaction:** - **Mass Balance:** Ensure the number of Mn atoms and O atoms is the same on both sides. - **Charge Balance:** Adjust for charge with electrons (e⁻). 4. **Incorporate Physical State Symbols:** - Indicate MnO₂ as solid (s) and MnO₄⁻ as aqueous (aq). **Outcome:** The balanced half-reaction combines mass and charge conservation, factoring in additional H₂O and H⁺ molecules needed to balance O and H atoms. **Conclusion:** Writing balanced half-reactions requires attention to detail in stoichiometry and electron transfer, fundamental in understanding redox processes in chemistry.
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Oxidation : Loss of electrons with increase in the oxidation state .Solid manganese dioxide MnO2 is oxidizes to permanganate ion MnO4- .We have to write a balance half-reaction in acidic aqueous solution .

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