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Chemistry need help

using standard potentials given in the appendices calculate the standard cell potentials and the equilibrium constants for the following reactions.

Zn(s)+( Fe^2+(aq)) ---> (Zn^2+(aq))+ Fe(s)

If anyone can show work, then I can do the rest of my homework by looking at this example.

Thank you!!!!!

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  1. Look up and post the reduction reaction and Eo for each half cell so we'll be using the same numbers.

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  2. I've checked every five minutes and no activity. So are you working on your homework?

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  3. Cathode (Reduction)
    Half-Reaction Zn2+(aq) + 2e- -> Zn(s)

    Standard Potential E° (volts)= -0.76

    Cathode (Reduction)
    Half-Reaction Fe2+(aq) + 2e- -> Fe(s)

    Standard Potential E° (volts)= -0.41

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  4. Both can't be the cathode.
    OK. Zn --> Zn^2+ is the half reaction in the problem. What you looked up is the standard reduction potential but this is an oxidation; therefore, reverse the sign. The E value for the half reaction as written is +0.76 v. The other is a reduction and it has the potential you have indicated. Add the oxidation half and the reduction half to obtain the total rxn.
    Ecell as written is 0.76 + (-0.41 = ?

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  5. How do you calculate the equilibrium constants for these reactions? This was the second part of the question!

    Thank you!

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  6. Sorry, I forgot about that.
    dGo = -nFEo

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