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Equilibrium Potential of Half Cell

  1. Mar 25, 2008 #1
    1. The problem statement, all variables and given/known data
    Given the following half-reactions:
    Ce4+ + e− → Ce3+ E° = 1.72 V
    Fe3+ + e− → Fe2+ E° = 0.771 V

    A solution is prepared by mixing 9.0 mL of 0.30 M Fe2+ with 7.0 mL of 0.11 M Ce4+.

    1. What is the potential of a platinum electrode dipped into the resulting, equilibrated, solution (relative to SHE)?

    2. Calculate Keq for the reaction

    Ce4+ + Fe2+ ⇌ Ce3+ + Fe3+

    3. Calculate [Ce4+] in the solution.

    2. Relevant equations

    Nernst equation

    3. The attempt at a solution

    I got question 2 since its K = 10^(nEo/0.05916), K= 10^(1(1.72-0.771))/0.05916)=1.1*10^16

    I tried and can't seem to get #1 correct. #3 I used ICE table method but cannot get a answer that makes sense. Any help is appreciated. Thanks.
     
  2. jcsd
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