Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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In a particular redox reaction, NO is oxidized to NO₃⁻ and Cu²⁺ is reduced to Cu⁺. Complete and balance the equation for this reaction in acidic solution. Phases are optional.

**Balanced redox reaction:**

\[ \text{NO} + 4\text{OH}^- + 3\text{Cu}^{2+} \rightarrow \text{NO}_3^- + 2\text{H}_2\text{O} + 3\text{Cu}^+ \]

**Explanation:**

This chemical equation is a redox reaction. In this reaction, nitric oxide (NO) is oxidized, meaning it loses electrons to become the nitrate ion (NO₃⁻). Concurrently, copper(II) ions (Cu²⁺) are reduced, meaning they gain electrons to form copper(I) ions (Cu⁺). The hydroxide ions (OH⁻) and water (H₂O) are involved to balance the equation in acidic conditions.
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Transcribed Image Text:In a particular redox reaction, NO is oxidized to NO₃⁻ and Cu²⁺ is reduced to Cu⁺. Complete and balance the equation for this reaction in acidic solution. Phases are optional. **Balanced redox reaction:** \[ \text{NO} + 4\text{OH}^- + 3\text{Cu}^{2+} \rightarrow \text{NO}_3^- + 2\text{H}_2\text{O} + 3\text{Cu}^+ \] **Explanation:** This chemical equation is a redox reaction. In this reaction, nitric oxide (NO) is oxidized, meaning it loses electrons to become the nitrate ion (NO₃⁻). Concurrently, copper(II) ions (Cu²⁺) are reduced, meaning they gain electrons to form copper(I) ions (Cu⁺). The hydroxide ions (OH⁻) and water (H₂O) are involved to balance the equation in acidic conditions.
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