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Step 4: Fill in the relative half-cell reduction potentials with zinc as the reference electrode using data from the previous steps (Steps 1-3 in Video 2). Zn²+/Zn: vols Cu²+/Cu: Mg2+/Mg: Fe²+/Fe: Step 5: Calculate the expected potentials for the following cells using the half-cell potentials in the table above. Compare them with the measured values (from Video 2) and determine the percent error. Assume that the expected potential is the accepted value. Cell Mg Mg²+||Fe²+ Fe Mg|Mg2+||Cu²+ Cu Fe|Fe²+||Cu²+|Cu CALCULATIONS: Expected Potential Measured Potential Percent Error

Step 4: Fill in the relative half-cell reduction potentials with zinc as the reference electrode using data from the previous steps (Steps 1-3 in Video 2). Zn²+/Zn: vols Cu²+/Cu: Mg2+/Mg: Fe²+/Fe: Step 5: Calculate the expected potentials for the following cells using the half-cell potentials in the table above. Compare them with the measured values (from Video 2) and determine the percent error. Assume that the expected potential is the accepted value. Cell Mg Mg²+||Fe²+ Fe Mg|Mg2+||Cu²+ Cu Fe|Fe²+||Cu²+|Cu CALCULATIONS: Expected Potential Measured Potential Percent Error

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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Step 4 and Step 5. Use the tabel I filled out to find out. 

**Part A: Measuring Electrochemical Cell Potentials (Video 2 on Canvas)** **Steps 1-3:** Complete the following diagrams by adding the cell voltage, both half-reactions, and the overall cell reaction from experimental measurements. Indicate the electrode classification for each metal by circling A for anode or C for cathode. ### Diagram Explanations: **First Diagram:** - **Voltage:** 1.088 - **Metals:** Zn | Cu - **Electrode Classification:** Zn (A), Cu (C) - **Half-Reactions:** - Zn(s) → Zn²⁺ + 2e⁻ - Cu²⁺ + 2e⁻ → Cu(s) - **Cell Reaction:** - Zn + Cu²⁺ → Zn²⁺ + Cu **Second Diagram:** - **Voltage:** -0.572 - **Metals:** Zn | Mg - **Electrode Classification:** Zn (C), Mg (A) - **Half-Reactions:** - Mg → Mg²⁺ + 2e⁻ - Zn²⁺ + 2e⁻ → Zn - **Cell Reaction:** - Mg + Zn²⁺ → Mg²⁺ + Zn **Third Diagram:** - **Voltage:** 0.446 - **Metals:** Zn | Fe - **Electrode Classification:** Zn (A), Fe (C) - **Half-Reactions:** - Zn(s) → Zn²⁺ + 2e⁻ - Fe²⁺ + 2e⁻ → Fe(s) - **Cell Reaction:** - Zn + Fe²⁺ → Zn²⁺ + Fe **Fourth Diagram:** - **Voltage:** 1.017 - **Metals:** Mg | Fe - **Electrode Classification:** Mg (A), Fe (C) - **Half-Reactions:** - Mg → Mg²⁺ + 2e⁻ - Fe²⁺ + 2e⁻ → Fe - **Cell Reaction:** - Mg + Fe²⁺ → Mg²⁺ + Fe **Fifth Diagram:** - **Voltage:** 1.667 - **Metals:** Mg | Cu - **Electrode Classification:** Mg (A),
Transcribed Image Text:**Part A: Measuring Electrochemical Cell Potentials (Video 2 on Canvas)** **Steps 1-3:** Complete the following diagrams by adding the cell voltage, both half-reactions, and the overall cell reaction from experimental measurements. Indicate the electrode classification for each metal by circling A for anode or C for cathode. ### Diagram Explanations: **First Diagram:** - **Voltage:** 1.088 - **Metals:** Zn | Cu - **Electrode Classification:** Zn (A), Cu (C) - **Half-Reactions:** - Zn(s) → Zn²⁺ + 2e⁻ - Cu²⁺ + 2e⁻ → Cu(s) - **Cell Reaction:** - Zn + Cu²⁺ → Zn²⁺ + Cu **Second Diagram:** - **Voltage:** -0.572 - **Metals:** Zn | Mg - **Electrode Classification:** Zn (C), Mg (A) - **Half-Reactions:** - Mg → Mg²⁺ + 2e⁻ - Zn²⁺ + 2e⁻ → Zn - **Cell Reaction:** - Mg + Zn²⁺ → Mg²⁺ + Zn **Third Diagram:** - **Voltage:** 0.446 - **Metals:** Zn | Fe - **Electrode Classification:** Zn (A), Fe (C) - **Half-Reactions:** - Zn(s) → Zn²⁺ + 2e⁻ - Fe²⁺ + 2e⁻ → Fe(s) - **Cell Reaction:** - Zn + Fe²⁺ → Zn²⁺ + Fe **Fourth Diagram:** - **Voltage:** 1.017 - **Metals:** Mg | Fe - **Electrode Classification:** Mg (A), Fe (C) - **Half-Reactions:** - Mg → Mg²⁺ + 2e⁻ - Fe²⁺ + 2e⁻ → Fe - **Cell Reaction:** - Mg + Fe²⁺ → Mg²⁺ + Fe **Fifth Diagram:** - **Voltage:** 1.667 - **Metals:** Mg | Cu - **Electrode Classification:** Mg (A),
**Step 4:** Fill in the relative half-cell reduction potentials with zinc as the reference electrode using data from the previous steps (Steps 1-3 in Video 2). - Zn²⁺/Zn: 0 volts - Cu²⁺/Cu: _____ - Mg²⁺/Mg: _____ - Fe²⁺/Fe: _____ **Step 5:** Calculate the expected potentials for the following cells using the half-cell potentials in the table above. Compare them with the measured values (from Video 2) and determine the percent error. Assume that the expected potential is the accepted value. | Cell | Expected Potential | Measured Potential | Percent Error | |---------------------|--------------------|--------------------|---------------| | Mg|Mg²⁺||Fe²⁺|Fe | | | | | Mg|Mg²⁺||Cu²⁺|Cu | | | | | Fe|Fe²⁺||Cu²⁺|Cu | | | | **CALCULATIONS:** **Step 6:** Rank the reduction potentials of the metal ions (Zn²⁺, Cu²⁺, Mg²⁺, Fe²⁺). | | greatest | | | smallest | |-------------------|----------|------------------|------------------|----------| | | Cu²⁺ | Fe²⁺ | Zn²⁺ | Mg²⁺ |
Transcribed Image Text:**Step 4:** Fill in the relative half-cell reduction potentials with zinc as the reference electrode using data from the previous steps (Steps 1-3 in Video 2). - Zn²⁺/Zn: 0 volts - Cu²⁺/Cu: _____ - Mg²⁺/Mg: _____ - Fe²⁺/Fe: _____ **Step 5:** Calculate the expected potentials for the following cells using the half-cell potentials in the table above. Compare them with the measured values (from Video 2) and determine the percent error. Assume that the expected potential is the accepted value. | Cell | Expected Potential | Measured Potential | Percent Error | |---------------------|--------------------|--------------------|---------------| | Mg|Mg²⁺||Fe²⁺|Fe | | | | | Mg|Mg²⁺||Cu²⁺|Cu | | | | | Fe|Fe²⁺||Cu²⁺|Cu | | | | **CALCULATIONS:** **Step 6:** Rank the reduction potentials of the metal ions (Zn²⁺, Cu²⁺, Mg²⁺, Fe²⁺). | | greatest | | | smallest | |-------------------|----------|------------------|------------------|----------| | | Cu²⁺ | Fe²⁺ | Zn²⁺ | Mg²⁺ |
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