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7. An electrolytic cell was constructed from zinc and copper half-cells. The equation of the reaction is shown below. Zn (s) + Cư“ (aq) → Zn²* (aq) + Cu (s) The observed voltage was found to be 1.00 V instead of the standard cell potential, F of 1.10 V. Which of the following accounts for this observation? A. The solutions in the half-cells had different volumes. B. The copper electrode was larger than the zinc electrode. C. The Zn* solution was more concentrated than the Cu²* solution. D. The Zn2* electrolyte was ZnSO4, while the Cu²* electrolyte was Cu(NO:)2-

7. An electrolytic cell was constructed from zinc and copper half-cells. The equation of the reaction is shown below. Zn (s) + Cư“ (aq) → Zn²* (aq) + Cu (s) The observed voltage was found to be 1.00 V instead of the standard cell potential, F of 1.10 V. Which of the following accounts for this observation? A. The solutions in the half-cells had different volumes. B. The copper electrode was larger than the zinc electrode. C. The Zn* solution was more concentrated than the Cu²* solution. D. The Zn2* electrolyte was ZnSO4, while the Cu²* electrolyte was Cu(NO:)2-

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Chemistry
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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
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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7. An electrolytic cell was constructed from zinc and copper half-cells. The equation of the reaction is shown below. Zn (s) + Cu²* (aq) → Zn²* (aq) + Cu (s) The observed voltage was found to be 1.00 V instead of the standard cell potential, F of 1.10 V. Which of the following accounts for this observation? A. The solutions in the half-cells had different volumes. B. The copper electrode was larger than the zinc electrode. C. The Zn solution was more concentrated than the Cu²* solution. D. The Zn* electrolyte was ZnSO4, while the Cu2* electrolyte was Cu(NO3)2.
Transcribed Image Text:7. An electrolytic cell was constructed from zinc and copper half-cells. The equation of the reaction is shown below. Zn (s) + Cu²* (aq) → Zn²* (aq) + Cu (s) The observed voltage was found to be 1.00 V instead of the standard cell potential, F of 1.10 V. Which of the following accounts for this observation? A. The solutions in the half-cells had different volumes. B. The copper electrode was larger than the zinc electrode. C. The Zn solution was more concentrated than the Cu²* solution. D. The Zn* electrolyte was ZnSO4, while the Cu2* electrolyte was Cu(NO3)2.
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