O0.02O 0.44O 0.48O 0.46 Using the Nernst Equation, Calculate Ecell for the following electrochemical cell under the stated (non-standard) conditions.CuCu²+ (0.2 M)Balanced Redox:Cu(s) | Cu²+ (aq, 0.20 M) || Ag+(aq, 1.0 M) | Ag(s)E = E° -AgCu (s) + 2 Ag+ (aq) → Cu²+ (aq) + 2 Ag (s) Eº =cell0.0592 VAg+ (1.0 M)nlog Q (T = 298 K)+0.46 V

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Using the Nernst Equation, Calculate Ecell for the following electrochemical cell under the stated (non- standard) conditions. Cu Cu2+ (0.2 M) Ag Ag+ (1.0 M) Cu(s) | Cu²+ (aq, 0.20 M) || Ag+(aq, 1.0 M) | Ag(s)

Using the Nernst Equation, Calculate Ecell for the following electrochemical cell under the stated (non- standard) conditions. Cu Cu2+ (0.2 M) Ag Ag+ (1.0 M) Cu(s) | Cu²+ (aq, 0.20 M) || Ag+(aq, 1.0 M) | Ag(s)

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

Using the Nernst Equation, Calculate Ecell for the following electrochemical cell under the stated (non-
standard) conditions.
Cu
Cu²+ (0.2 M)
Balanced Redox:
Cu(s) | Cu²+ (aq, 0.20 M) || Ag+(aq, 1.0 M) | Ag(s)
E = E° -
Ag
Cu (s) + 2 Ag+ (aq) → Cu²+ (aq) + 2 Ag (s) Eº =
cell
0.0592 V
Ag+ (1.0 M)
n
log Q (T = 298 K)
+0.46 V

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