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A chemist designs a galvanic cell that uses these two half-reactions: half-reaction NO3(aq) + 4 H (aq) + 3e¯¯ Zn(aq)+2e NO(g) + 2 H₂O(1) Zn(s) standard reduction potential red = +0.96 V Ed=-0.763 V "red

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction NO3(aq) + 4 H (aq) + 3e¯¯ Zn(aq)+2e NO(g) + 2 H₂O(1) Zn(s) standard reduction potential red = +0.96 V Ed=-0.763 V "red

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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## Designing a Galvanic Cell Using Specific Half-Reactions A chemist designs a galvanic cell that uses the following two half-reactions: | Half-Reaction | Standard Reduction Potential (\(E^\circ_{\text{red}}\)) | |-----------------------------------------------------------|----------------------------------------------| | \( \text{NO}_3^- (aq) + 4 \text{H}^+ (aq) + 3 e^- \rightarrow \text{NO} (g) + 2 \text{H}_2 \text{O} (l) \) | \( +0.96 \, \text{V} \) | | \( \text{Zn}^{2+} (aq) + 2 e^- \rightarrow \text{Zn}(s) \) | \( -0.763 \, \text{V} \) | **Table Explanation:** - The table provides two half-reactions with their corresponding standard reduction potentials. - The first half-reaction involves the reduction of nitrate ions (\(\text{NO}_3^- \)) in an acidic solution to produce nitric oxide gas (\(\text{NO}\)) and water (\(\text{H}_2 \text{O} \)). This reaction has a standard reduction potential (\(E^\circ_{\text{red}}\)) of \(\ +0.96 \, \text{V} \). - The second half-reaction involves the reduction of zinc ions (\(\text{Zn}^{2+} \)) to solid zinc (\(\text{Zn}(s)\)), with a standard reduction potential (\(E^\circ_{\text{red}}\)) of \(\ -0.763 \, \text{V} \). In constructing a galvanic cell using these half-reactions, the overall cell potential can be determined from these standard reduction potentials, leading to the calculation of the standard cell potential, \(E^\circ_{\text{cell}}\). This is accomplished by combining the oxidation and reduction potentials appropriately and recognizing which half-reaction will serve as the oxidation process and which will serve as the reduction process.
Transcribed Image Text:## Designing a Galvanic Cell Using Specific Half-Reactions A chemist designs a galvanic cell that uses the following two half-reactions: | Half-Reaction | Standard Reduction Potential (\(E^\circ_{\text{red}}\)) | |-----------------------------------------------------------|----------------------------------------------| | \( \text{NO}_3^- (aq) + 4 \text{H}^+ (aq) + 3 e^- \rightarrow \text{NO} (g) + 2 \text{H}_2 \text{O} (l) \) | \( +0.96 \, \text{V} \) | | \( \text{Zn}^{2+} (aq) + 2 e^- \rightarrow \text{Zn}(s) \) | \( -0.763 \, \text{V} \) | **Table Explanation:** - The table provides two half-reactions with their corresponding standard reduction potentials. - The first half-reaction involves the reduction of nitrate ions (\(\text{NO}_3^- \)) in an acidic solution to produce nitric oxide gas (\(\text{NO}\)) and water (\(\text{H}_2 \text{O} \)). This reaction has a standard reduction potential (\(E^\circ_{\text{red}}\)) of \(\ +0.96 \, \text{V} \). - The second half-reaction involves the reduction of zinc ions (\(\text{Zn}^{2+} \)) to solid zinc (\(\text{Zn}(s)\)), with a standard reduction potential (\(E^\circ_{\text{red}}\)) of \(\ -0.763 \, \text{V} \). In constructing a galvanic cell using these half-reactions, the overall cell potential can be determined from these standard reduction potentials, leading to the calculation of the standard cell potential, \(E^\circ_{\text{cell}}\). This is accomplished by combining the oxidation and reduction potentials appropriately and recognizing which half-reaction will serve as the oxidation process and which will serve as the reduction process.
### Worksheet on Electrochemical Reactions --- #### Section 1: Half-Reaction at the Cathode **Instruction:** Write a balanced equation for the half-reaction that happens at the cathode. **Response:** ______________________________________ --- #### Section 2: Half-Reaction at the Anode **Instruction:** Write a balanced equation for the half-reaction that happens at the anode. **Response:** ______________________________________ --- #### Section 3: Overall Reaction of the Cell **Instruction:** Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. **Response:** ______________________________________ --- This worksheet aims to help students understand the chemical reactions that occur in electrochemical cells. The provided tasks guide students through identifying and balancing the half-reactions and the overall cell reaction, which are essential skills in understanding electrochemistry. **Note for Educators:** Encourage students to remember the key principles of identifying oxidation and reduction reactions, as well as the concept of spontaneous reactions in electrochemistry.
Transcribed Image Text:### Worksheet on Electrochemical Reactions --- #### Section 1: Half-Reaction at the Cathode **Instruction:** Write a balanced equation for the half-reaction that happens at the cathode. **Response:** ______________________________________ --- #### Section 2: Half-Reaction at the Anode **Instruction:** Write a balanced equation for the half-reaction that happens at the anode. **Response:** ______________________________________ --- #### Section 3: Overall Reaction of the Cell **Instruction:** Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. **Response:** ______________________________________ --- This worksheet aims to help students understand the chemical reactions that occur in electrochemical cells. The provided tasks guide students through identifying and balancing the half-reactions and the overall cell reaction, which are essential skills in understanding electrochemistry. **Note for Educators:** Encourage students to remember the key principles of identifying oxidation and reduction reactions, as well as the concept of spontaneous reactions in electrochemistry.
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