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Consider the cell: Cd(s) | Cd2*(aq) (0.035M) || Cu²*(aq) (x M)| Cu(s) Cd2+ + 2e Cd E° = -0.40 V Cu2+ + 2e → Cu E° = +0.34 V The measured potential of the cell at 298 K is +0.77 V, what is the concentration of Cu2+? R = 8.314 J/mol-K F = 96,485 J/mol-V %3D O 0.36 M 0.036 M 0.11 M 0.0034 M

Consider the cell: Cd(s) | Cd2*(aq) (0.035M) || Cu²*(aq) (x M)| Cu(s) Cd2+ + 2e Cd E° = -0.40 V Cu2+ + 2e → Cu E° = +0.34 V The measured potential of the cell at 298 K is +0.77 V, what is the concentration of Cu2+? R = 8.314 J/mol-K F = 96,485 J/mol-V %3D O 0.36 M 0.036 M 0.11 M 0.0034 M

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
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 86E: An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.0...
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Consider the cell: Cd(s) | Cd2*(aq) (0.035M) || Cu²+(aq) (x M)| Cu(s) Cd2+ + 2e → Cd E° = -0.40 V %3D Cu2+ + 2e → Cu E° = +0.34 V %3D The measured potential of the cell at 298 K is +0.77 V, what is the concentration of Cu2+? R = 8.314 J/mol-K %3D F = 96,485 J/mol-V O 0.36 M 0.036 M O 0.11 M O 0.0034 M
Transcribed Image Text:Consider the cell: Cd(s) | Cd2*(aq) (0.035M) || Cu²+(aq) (x M)| Cu(s) Cd2+ + 2e → Cd E° = -0.40 V %3D Cu2+ + 2e → Cu E° = +0.34 V %3D The measured potential of the cell at 298 K is +0.77 V, what is the concentration of Cu2+? R = 8.314 J/mol-K %3D F = 96,485 J/mol-V O 0.36 M 0.036 M O 0.11 M O 0.0034 M
Calculate AG° for a voltaic cell with E° = +0.309 V if the overall reaction involves a 5-electron transfer. R = 8.314 J/mol-K F = 96,485 J/mol-V %3D O-1.49 x 105J O+2.98 x 104 J O+5.96 x 10³ J O+1.49 x 105
Transcribed Image Text:Calculate AG° for a voltaic cell with E° = +0.309 V if the overall reaction involves a 5-electron transfer. R = 8.314 J/mol-K F = 96,485 J/mol-V %3D O-1.49 x 105J O+2.98 x 104 J O+5.96 x 10³ J O+1.49 x 105
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