Chemistry

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Please help me solve this problem:
What is the value of the equilibrium constant (K) for the reaction below 25^o C?
3I2(s) + 2Fe(s) --> 2Fe^3+(aq) + 6I^-

  • Chemistry -

    What do you have for data? My crystal ball is hazy today.

  • Chemistry -

    I know that I'm suppose to use the formula Ecell = 0.0592V/n*logK and solve for K, but before I do that, I have to find the oxidation and reduction from the chemical equation that was given for me. But I just do not know how to approach it. And i'm pretty stuck.

  • Chemistry -

    That helps but not enough.
    Ecell = Eocell + (0.0592/n)*logK and you can findEocell from the reactants and products. Furthermore, Ecell = Eocell if you are at standard conditions.
    Look up the potentials for the following:
    I2 + 2e ==> 2I^- Eo = ??(as a reduction)
    Fe ==> Fe^3+ + 3e Eo = ??(as an oxidation)
    Add the Eo redn to Eo oxdn to find Eo for the cell (at standard conditions)

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