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You are asked to balance the following redox equation. What characteristics does this equation have that would lead you to balance it using the half-reaction method? +NO₂ 3 → NO + Cu²+ (aq)

You are asked to balance the following redox equation. What characteristics does this equation have that would lead you to balance it using the half-reaction method? +NO₂ 3 → NO + Cu²+ (aq)

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 Equations Using the Half-Reaction Method** In this exercise, you are asked to balance the following redox equation. Consider the characteristics that guide the decision to use the half-reaction method for balancing: **Given Equation:** \[ \text{Cu} _{(s)} + \text{NO}_3 ^{-} _{(aq)} \rightarrow \text{NO} _{(g)} + \text{Cu}^{2+} _{(aq)} \] ### Characteristics for Using the Half-Reaction Method: 1. **Oxidation and Reduction Steps:** - Identify the species undergoing oxidation and reduction. - **Oxidation:** Cu (s) → Cu²⁺ (aq) - **Reduction:** NO₃⁻ (aq) → NO (g) 2. **Balancing the Charges:** - Balance the charges by adding electrons (e⁻) to the half-reactions. - For the copper oxidation half-reaction: Cu (s) → Cu²⁺ (aq) + 2e⁻ - For the nitrate reduction half-reaction: NO₃⁻ (aq) + 4H⁺ + 3e⁻ → NO (g) + 2H₂O (l) 3. **Balancing Atoms and Mass:** - Ensure that all atoms except hydrogen and oxygen are balanced initially. - Use water (H₂O) to balance oxygen atoms and hydrogen ions (H⁺) to balance hydrogen atoms in acidic solutions. 4. **Combining the Half-Reactions:** - Multiply the half-reactions by appropriate factors to equalize the number of electrons involved in both half-reactions. - Add the half-reactions together and simplify to get the balanced redox equation. ### Explanation of Components: - **Cu (s):** Solid Copper, which gets oxidized to Cu²⁺. - **NO₃⁻ (aq):** Nitrate ion in aqueous solution, which gets reduced to NO (g). - **NO (g):** Nitric oxide gas, a product of the reduction half-reaction. - **Cu²⁺ (aq):** Copper ion in an aqueous solution, a product of the oxidation half-reaction. This redox equation balancing requires attention to both the oxidation state changes and charge conservation, making the half
Transcribed Image Text:**Balancing Redox Equations Using the Half-Reaction Method** In this exercise, you are asked to balance the following redox equation. Consider the characteristics that guide the decision to use the half-reaction method for balancing: **Given Equation:** \[ \text{Cu} _{(s)} + \text{NO}_3 ^{-} _{(aq)} \rightarrow \text{NO} _{(g)} + \text{Cu}^{2+} _{(aq)} \] ### Characteristics for Using the Half-Reaction Method: 1. **Oxidation and Reduction Steps:** - Identify the species undergoing oxidation and reduction. - **Oxidation:** Cu (s) → Cu²⁺ (aq) - **Reduction:** NO₃⁻ (aq) → NO (g) 2. **Balancing the Charges:** - Balance the charges by adding electrons (e⁻) to the half-reactions. - For the copper oxidation half-reaction: Cu (s) → Cu²⁺ (aq) + 2e⁻ - For the nitrate reduction half-reaction: NO₃⁻ (aq) + 4H⁺ + 3e⁻ → NO (g) + 2H₂O (l) 3. **Balancing Atoms and Mass:** - Ensure that all atoms except hydrogen and oxygen are balanced initially. - Use water (H₂O) to balance oxygen atoms and hydrogen ions (H⁺) to balance hydrogen atoms in acidic solutions. 4. **Combining the Half-Reactions:** - Multiply the half-reactions by appropriate factors to equalize the number of electrons involved in both half-reactions. - Add the half-reactions together and simplify to get the balanced redox equation. ### Explanation of Components: - **Cu (s):** Solid Copper, which gets oxidized to Cu²⁺. - **NO₃⁻ (aq):** Nitrate ion in aqueous solution, which gets reduced to NO (g). - **NO (g):** Nitric oxide gas, a product of the reduction half-reaction. - **Cu²⁺ (aq):** Copper ion in an aqueous solution, a product of the oxidation half-reaction. This redox equation balancing requires attention to both the oxidation state changes and charge conservation, making the half
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