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A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e- → Ag(s) +0.80 Cu2+(aq) +2e- Cu(s) +0.34 Zn2+(ag) +2e-→ Zn(s) -0.76 1. Identify the reduction half-reaction involved. O a. Ag (aq) +e → Ag(s) O b. Cu²+ (aq) +2e → Cu(s) O c. Zn²+ (aq) +2e- Zn(s) 2. Determine the concentration of the anode electrolyte solution using the Nernst equation. →

A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e- → Ag(s) +0.80 Cu2+(aq) +2e- Cu(s) +0.34 Zn2+(ag) +2e-→ Zn(s) -0.76 1. Identify the reduction half-reaction involved. O a. Ag (aq) +e → Ag(s) O b. Cu²+ (aq) +2e → Cu(s) O c. Zn²+ (aq) +2e- Zn(s) 2. Determine the concentration of the anode electrolyte solution using the Nernst equation. →

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.49QE: A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt...
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A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(ag) +2e-→ Cu(s) +0.34 Zn2+(ag) +2e- → Zn(s) -0.76 1. Identify the reduction half-reaction involved. o a. Agt(aq) +e-- Ag(s) O b. Cu²+ (aq) +2e → Cu(s) c. Zn²+ (aq) +2e- Zn(s) 2. Determine the concentration of the anode electrolyte solution using the Nernst equation.
Transcribed Image Text:A galvanic cell is set-up in the laboratory with a copper anode and an unidentified cathode. Your teacher asks you to identify the cathode of the solution with the given information. The anode metal is lustrous and grey in color, so you narrow it down to silver and zinc. The voltmeter reading shows that the cell potential is 0.50 V. The copper (II) sulfate solution was indicated to have a concentration of 0.10 M. Reduction Half-Reaction Standard Reduction Potential (V) Ag+(ag) +e-→ Ag(s) +0.80 Cu2+(ag) +2e-→ Cu(s) +0.34 Zn2+(ag) +2e- → Zn(s) -0.76 1. Identify the reduction half-reaction involved. o a. Agt(aq) +e-- Ag(s) O b. Cu²+ (aq) +2e → Cu(s) c. Zn²+ (aq) +2e- Zn(s) 2. Determine the concentration of the anode electrolyte solution using the Nernst equation.
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