Calculate the Ecell value at 298 Kfor the cell based on the reaction: Cu(s)+2Ag*(aq) Cu?+(aq) + 2Ag(s) where [Ag*] = 0.00150 M and [Cu2+] = 7.50x10-4 M. The standard reduction potentials are shown below: Ag"(aq) +e - Ag(s) E° = 0.7996 V Cu2+ (aq) +2e → Cu(s) E° = 0.3419 V
Calculate the Ecell value at 298 Kfor the cell based on the reaction: Cu(s)+2Ag*(aq) Cu?+(aq) + 2Ag(s) where [Ag*] = 0.00150 M and [Cu2+] = 7.50x10-4 M. The standard reduction potentials are shown below: Ag"(aq) +e - Ag(s) E° = 0.7996 V Cu2+ (aq) +2e → Cu(s) E° = 0.3419 V
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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![Calculate the Ecell value at 298 K for the cell based on the reaction:
Cu(s)+2Ag*(aq)
Cu?+(aq) + 2Ag(s)
where [Ag*] = 0.00150 M and [Cu2+] = 7.50x10-4 M.
The standard reduction potentials are shown below:
Ag"(aq) +e - Ag(s) E° = 0.7996 V
Cu+ (aq)+ 2e
→ Cu(s) E° =
0.3419 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2b6c2e9e-a347-484d-9c96-cdd239fef4f7%2Fe6c52caa-c31c-491c-a959-31785d57dc33%2Fg84ol4_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Calculate the Ecell value at 298 K for the cell based on the reaction:
Cu(s)+2Ag*(aq)
Cu?+(aq) + 2Ag(s)
where [Ag*] = 0.00150 M and [Cu2+] = 7.50x10-4 M.
The standard reduction potentials are shown below:
Ag"(aq) +e - Ag(s) E° = 0.7996 V
Cu+ (aq)+ 2e
→ Cu(s) E° =
0.3419 V
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