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Balance the following redox reaction in acidic solution. MnO₂(s) + Cu* (aq) 2+ 2+ Mn (aq) + Cu (aq) Cu²+ (aq) 2+ Mn²+ (aq) + Cu² MnO₂ (s) + Cu* (aq) ローロ X 4

Balance the following redox reaction in acidic solution. MnO₂(s) + Cu* (aq) 2+ 2+ Mn (aq) + Cu (aq) Cu²+ (aq) 2+ Mn²+ (aq) + Cu² MnO₂ (s) + Cu* (aq) ローロ X 4

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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**Balancing Redox Reactions in Acidic Solution** **Given Reaction:** \[ \text{Mn}^{2+} (aq) + \text{Cu}^{2+} (aq) \rightarrow \text{MnO}_2 (s) + \text{Cu}^{+} (aq) \] **Task:** Balance the reaction above, showing the oxidation and reduction processes in an acidic solution. **Diagram Explanation:** The image shows the initial unbalanced chemical equation with manganese(II) ions and copper(II) ions reacting to form manganese dioxide and copper(I) ions. The notation \(e^-\) represents the electrons involved in the oxidation-reduction process, essential for redox reaction balancing. To balance this redox reaction, you should ensure the number of each type of atom and the charges are equal on both sides of the equation, considering the acidic environment. This typically involves adding water molecules, hydrogen ions, and electrons where necessary.
Transcribed Image Text:**Balancing Redox Reactions in Acidic Solution** **Given Reaction:** \[ \text{Mn}^{2+} (aq) + \text{Cu}^{2+} (aq) \rightarrow \text{MnO}_2 (s) + \text{Cu}^{+} (aq) \] **Task:** Balance the reaction above, showing the oxidation and reduction processes in an acidic solution. **Diagram Explanation:** The image shows the initial unbalanced chemical equation with manganese(II) ions and copper(II) ions reacting to form manganese dioxide and copper(I) ions. The notation \(e^-\) represents the electrons involved in the oxidation-reduction process, essential for redox reaction balancing. To balance this redox reaction, you should ensure the number of each type of atom and the charges are equal on both sides of the equation, considering the acidic environment. This typically involves adding water molecules, hydrogen ions, and electrons where necessary.
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