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Part 1. (Black) Anode (Red) Cathede voltage Trial I Zinc (s) Copper (s) Trial 2 Copper CS) Graphite (s) 0.90 0.23V Trial 3 Zinc (S) Graphite (s) 1.26 V ELECTROCHEMISTRY AND CELL POTENTIALS DATA ANALYSIS: Part 1: 1. Exploring the Cell Potentials of Different Materials For each cell measured in Part 1, a. identify the anode electrode b. identify the cathode electrode c. write the balanced oxidation half reaction and its standard oxidation potentia d. write the balanced reduction half reaction and its standard reduction potenti e. write the overall balanced redox reaction and its standard cell potential f. write the line notation for the cell g. calculate the theoretical cell voltage using the standard cell potential and solution concentrations h. report the experimentally measured cell voltage i. calculate the % error between the theoretical cell voltage and the measured voltage (Note: recall that the I2 used in this experiment is aqueous, not solid, so us provided value of Ered I2(aq) = +0.62 V.)

Part 1. (Black) Anode (Red) Cathede voltage Trial I Zinc (s) Copper (s) Trial 2 Copper CS) Graphite (s) 0.90 0.23V Trial 3 Zinc (S) Graphite (s) 1.26 V ELECTROCHEMISTRY AND CELL POTENTIALS DATA ANALYSIS: Part 1: 1. Exploring the Cell Potentials of Different Materials For each cell measured in Part 1, a. identify the anode electrode b. identify the cathode electrode c. write the balanced oxidation half reaction and its standard oxidation potentia d. write the balanced reduction half reaction and its standard reduction potenti e. write the overall balanced redox reaction and its standard cell potential f. write the line notation for the cell g. calculate the theoretical cell voltage using the standard cell potential and solution concentrations h. report the experimentally measured cell voltage i. calculate the % error between the theoretical cell voltage and the measured voltage (Note: recall that the I2 used in this experiment is aqueous, not solid, so us provided value of Ered I2(aq) = +0.62 V.)

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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Part 1. (Black) Anode (Red) Cathede voltage Trial I Zinc (s) Copper (s) Trial 2 Copper CS) Graphite (s) 0.90 0.23V Trial 3 Zinc (S) Graphite (s) 1.26 V ELECTROCHEMISTRY AND CELL POTENTIALS DATA ANALYSIS: Part 1: 1. Exploring the Cell Potentials of Different Materials For each cell measured in Part 1, a. identify the anode electrode b. identify the cathode electrode c. write the balanced oxidation half reaction and its standard oxidation potentia d. write the balanced reduction half reaction and its standard reduction potenti e. write the overall balanced redox reaction and its standard cell potential f. write the line notation for the cell g. calculate the theoretical cell voltage using the standard cell potential and solution concentrations h. report the experimentally measured cell voltage i. calculate the % error between the theoretical cell voltage and the measured voltage (Note: recall that the I2 used in this experiment is aqueous, not solid, so us provided value of Ered I2(aq) = +0.62 V.)
Transcribed Image Text:Part 1. (Black) Anode (Red) Cathede voltage Trial I Zinc (s) Copper (s) Trial 2 Copper CS) Graphite (s) 0.90 0.23V Trial 3 Zinc (S) Graphite (s) 1.26 V ELECTROCHEMISTRY AND CELL POTENTIALS DATA ANALYSIS: Part 1: 1. Exploring the Cell Potentials of Different Materials For each cell measured in Part 1, a. identify the anode electrode b. identify the cathode electrode c. write the balanced oxidation half reaction and its standard oxidation potentia d. write the balanced reduction half reaction and its standard reduction potenti e. write the overall balanced redox reaction and its standard cell potential f. write the line notation for the cell g. calculate the theoretical cell voltage using the standard cell potential and solution concentrations h. report the experimentally measured cell voltage i. calculate the % error between the theoretical cell voltage and the measured voltage (Note: recall that the I2 used in this experiment is aqueous, not solid, so us provided value of Ered I2(aq) = +0.62 V.)
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