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Workshop 11: Electrochemistry Here are some equations and constants that you might need for this part of the workshop: AG=AH - TAS AGO RT ln K AG=-nFE E = Eo - (RT/nF)In Q F = 96,480 C/mole electrons R = 0.082 1-atm/mol-deg = 8.3 J/mol-deg 1V = 1J/1C The Nernst Equation (E = E° - (RT/nF)ln Q) can be used to determine the value of Ecell, and thus the direction of spontaneous redox reaction under any conditions. Consider the cell: Cu | Cu²+ (aq, 1.6 M)|| Fe³+ (aq, 2.5 mM), Fe²+ (aq, 1.5 M) | Pt 1. Write the balanced net chemical reaction. AG= AGO+RT In Q

Workshop 11: Electrochemistry Here are some equations and constants that you might need for this part of the workshop: AG=AH - TAS AGO RT ln K AG=-nFE E = Eo - (RT/nF)In Q F = 96,480 C/mole electrons R = 0.082 1-atm/mol-deg = 8.3 J/mol-deg 1V = 1J/1C The Nernst Equation (E = E° - (RT/nF)ln Q) can be used to determine the value of Ecell, and thus the direction of spontaneous redox reaction under any conditions. Consider the cell: Cu | Cu²+ (aq, 1.6 M)|| Fe³+ (aq, 2.5 mM), Fe²+ (aq, 1.5 M) | Pt 1. Write the balanced net chemical reaction. AG= AGO+RT In Q

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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Workshop 11: Electrochemistry Here are some equations and constants that you might need for this part of the workshop: AG=AH - TAS AG=AGO + RT In Q AGO RT In K AG=-nFE E = Eo - (RT/nF)ln Q 1V = 1J/1C F = 96,480 C/mole electrons R = 0.082 l-atm/mol-deg = 8.3 J/mol-deg The Nernst Equation (E = E° - (RT/nF)In Q) can be used to determine the value of Ecell, and thus the direction of spontaneous redox reaction under any conditions. Consider the cell: Cu | Cu²+ (aq, 1.6 M)|| Fe³+ (aq, 2.5 mM), Fe²+ (aq, 1.5 M) | Pt 1. Write the balanced net chemical reaction. 2. Sketch a diagram of this galvanic cell using a salt bridge, and clearly indicate the anode, the cathode, the direction of electron flow and the direction of ion flow through the salt bridge.
Transcribed Image Text:Workshop 11: Electrochemistry Here are some equations and constants that you might need for this part of the workshop: AG=AH - TAS AG=AGO + RT In Q AGO RT In K AG=-nFE E = Eo - (RT/nF)ln Q 1V = 1J/1C F = 96,480 C/mole electrons R = 0.082 l-atm/mol-deg = 8.3 J/mol-deg The Nernst Equation (E = E° - (RT/nF)In Q) can be used to determine the value of Ecell, and thus the direction of spontaneous redox reaction under any conditions. Consider the cell: Cu | Cu²+ (aq, 1.6 M)|| Fe³+ (aq, 2.5 mM), Fe²+ (aq, 1.5 M) | Pt 1. Write the balanced net chemical reaction. 2. Sketch a diagram of this galvanic cell using a salt bridge, and clearly indicate the anode, the cathode, the direction of electron flow and the direction of ion flow through the salt bridge.
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