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Determine if the following reaction is a redox reaction. You evidence from the equation to explain your reasoning. Cu + NO, tag) → NO) + Cu²+, (aq) 3.

Determine if the following reaction is a redox reaction. You evidence from the equation to explain your reasoning. Cu + NO, tag) → NO) + Cu²+, (aq) 3.

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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**Question:** Determine if the following reaction is a redox reaction. Use evidence from the equation to explain your reasoning. **Equation:** Cu\(_{(s)}\) + NO\(_3^{-}\) \(_{(aq)}\) → NO\(_{(g)}\) + Cu\(^{2+}\) \(_{(aq)}\) ### Explanation: In this reaction, we need to determine if there is a transfer of electrons, which would make it a redox (reduction-oxidation) reaction. 1. **Identify Oxidation States:** - **Copper (Cu):** In its elemental form, copper has an oxidation state of 0. - **Nitrate Ion (NO\(_3^-\)):** The nitrate ion typically has nitrogen in the +5 oxidation state because the oxidation state of oxygen is -2 and the overall charge is -1. 2. **Products:** - **Nitric Oxide (NO):** In nitric oxide, the oxidation state of nitrogen is +2. - **Copper Ion (Cu\(^{2+}\)):** This indicates copper has an oxidation state of +2. 3. **Changes in Oxidation States:** - Copper (Cu) changes from 0 to +2, indicating a loss of electrons (oxidation). - Nitrogen (N) in NO\(_3^-\) changes from +5 to +2, indicating a gain of electrons (reduction). Since both oxidation (loss of electrons) and reduction (gain of electrons) are occurring, this reaction is indeed a redox reaction. ### Conclusion: The given reaction is a redox reaction because there is a transfer of electrons. Copper is oxidized from 0 to +2, and nitrogen is reduced from +5 to +2.
Transcribed Image Text:**Question:** Determine if the following reaction is a redox reaction. Use evidence from the equation to explain your reasoning. **Equation:** Cu\(_{(s)}\) + NO\(_3^{-}\) \(_{(aq)}\) → NO\(_{(g)}\) + Cu\(^{2+}\) \(_{(aq)}\) ### Explanation: In this reaction, we need to determine if there is a transfer of electrons, which would make it a redox (reduction-oxidation) reaction. 1. **Identify Oxidation States:** - **Copper (Cu):** In its elemental form, copper has an oxidation state of 0. - **Nitrate Ion (NO\(_3^-\)):** The nitrate ion typically has nitrogen in the +5 oxidation state because the oxidation state of oxygen is -2 and the overall charge is -1. 2. **Products:** - **Nitric Oxide (NO):** In nitric oxide, the oxidation state of nitrogen is +2. - **Copper Ion (Cu\(^{2+}\)):** This indicates copper has an oxidation state of +2. 3. **Changes in Oxidation States:** - Copper (Cu) changes from 0 to +2, indicating a loss of electrons (oxidation). - Nitrogen (N) in NO\(_3^-\) changes from +5 to +2, indicating a gain of electrons (reduction). Since both oxidation (loss of electrons) and reduction (gain of electrons) are occurring, this reaction is indeed a redox reaction. ### Conclusion: The given reaction is a redox reaction because there is a transfer of electrons. Copper is oxidized from 0 to +2, and nitrogen is reduced from +5 to +2.
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