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Consider the following electochemical cell.

Pt | Fe3+ (0.0600 M), Fe2+ (6.50e-5 M) || Sn2+ (0.0620 M), Sn4+ (3.90e-4 M) | Pt

(a) Calculate the voltage of the cell, Ecell, including the sign.

Question ID
524809

Created
April 3, 2011 9:18pm UTC

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0

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https://questions.llc/questions/524809

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2

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501

2 answers

  1. Use the Nernst equation to calculate the half cell potential of the Fe+3/Fe+2 electrode.
    Use the Nernst equation to calculate the half cell potential of the Sn+4/Sn+2 electrode. Note I used REDUCTIONS for both. Then I would proceed as follows:
    Identify the more negative electrode of the two reduction potentials, reverse it and the sign, add the two half equations to find the SPONTANEOUS cell reaction and spontaneous cell potential. Compare the spontaneous reaction with the reaction of the cell, which I've given below. Adjust your equation and potential (the sign) as needed. The reaction of the cell, as written, is:
    2Fe^+3 + Sn^+2 ==> 2Fe+2 + Sn^+4

    Answer ID
    524829

    Created
    April 3, 2011 9:47pm UTC

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    0

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  2. klj

    Answer ID
    1044677

    Created
    April 13, 2014 4:57pm UTC

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