Using the Nernst equation calculate the cell voltage for: Fe(s) + Cd²+(aq) → Fe2+(aq) + Cd(s) when the [Fe2+] = 0.19 M and [Cd2+] = 2.0 M. %3D Potentially useful information: Fe2+ + 2e- Fe(s); ɛ° = -0.44 V Cd(s); ɛ0 = -0.40 V Cd2+ + 2e- → %3D 0.12 Submit Answer Incorrect. Tries 7/99 Previous Tries
Using the Nernst equation calculate the cell voltage for: Fe(s) + Cd²+(aq) → Fe2+(aq) + Cd(s) when the [Fe2+] = 0.19 M and [Cd2+] = 2.0 M. %3D Potentially useful information: Fe2+ + 2e- Fe(s); ɛ° = -0.44 V Cd(s); ɛ0 = -0.40 V Cd2+ + 2e- → %3D 0.12 Submit Answer Incorrect. Tries 7/99 Previous Tries
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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Finding cell potential with the Nernst equation
![Using the Nernst equation calculate the cell voltage for:
Fe(s) + Cd2+(aq) → Fe2+(aq) + Cd(s)
when the [Fe?+] = 0.19 M and [Cd2+] = 2.0 M.
Potentially useful information:
Fe2+ + 2e-
Fe(s); ɛ0 = -0.44 V
Cd2+ + 2e- →
Cd(s); ɛº = -0.40 V
0.12
Submit Answer
Incorrect. Tries 7/99 Previous Tries](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc7221061-cab3-4d12-b574-9340e14d2678%2F28983acb-3f19-4bf2-978d-d06478af5e38%2Fhfvxvvl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Using the Nernst equation calculate the cell voltage for:
Fe(s) + Cd2+(aq) → Fe2+(aq) + Cd(s)
when the [Fe?+] = 0.19 M and [Cd2+] = 2.0 M.
Potentially useful information:
Fe2+ + 2e-
Fe(s); ɛ0 = -0.44 V
Cd2+ + 2e- →
Cd(s); ɛº = -0.40 V
0.12
Submit Answer
Incorrect. Tries 7/99 Previous Tries
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