Calculate Ecell at 298 K for an electrochemical cell based on the overall redox reaction between Cu2+ and Ag if [Ag*] = 2.56× 10-3 Mand [Cu?+] = 8.25 x 10-4 M. Standard tables of reduction potentials assume standard conditions, but many electrochemical cells operate under nonstandard conditions.An electrochemical cell is constructed based on the following balanced equation:Cu(s) + 2 Ag*(aq) → Cu2*(aq) + 2 Ag(s)Half-reactions with standard reduction potentials are given below.Cu2*(aq) + 2 e → Cu(s); E° = 0.342 VAg*(aq) + e¯ → Ag(s); E° = 0.800 V

1- First calculate the E°cell : E°cell = E°(cathode) - E°(anode) E°cell = E°(Ag+/Ag) - E°(Cu2+/Cu)…

Answered: alculate Ecell at 298 K for an…

alculate Ecell at 298 K for an electrochemical cell based on the overall redox reaction between Cu2+ and Ag if [Ag*] = 2.56 × 10- Mand [Cu2+] = 8.25 × 10-4 M.

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

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Question

Calculate Ecell at 298 K for an electrochemical cell based on the overall redox reaction between Cu2+ and Ag if [Ag*] = 2.56× 10-
3 Mand [Cu?+] = 8.25 x 10-4 M.

Standard tables of reduction potentials assume standard conditions, but many electrochemical cells operate under nonstandard conditions.
An electrochemical cell is constructed based on the following balanced equation:
Cu(s) + 2 Ag*(aq) → Cu2*(aq) + 2 Ag(s)
Half-reactions with standard reduction potentials are given below.
Cu2*(aq) + 2 e → Cu(s); E° = 0.342 V
Ag*(aq) + e¯ → Ag(s); E° = 0.800 V

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