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    Calculating delta G and standard cell potential

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    Consider the oxidation of ammonia:
    4NH3 (g) + 3O2(g) --> 2N2 (g) + 6H2O

    Calcualte the delta G for the reaction. If this reaction were used in a fuel cell, what would the standard cell potential be? What would be the cell potential at 100 degrees C?

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    4NH3 (g) + 3O2(g) --> 2N2 (g) + 6H2O

    equations : ∆G = ∆Gf of products - ∆Gf of reactants -------> standard state conditions
    ∆H = ∆Hf of products - ∆Hf of reactants
    ∆S = ∆Sf of products - ∆Sf of reactants
    ∆G = -nF (Ecell)
    ∆G = ∆H - T∆S

    constants : Faraday's constant --> F = 96500 C/mol e
    there are 12 e transferred from anode to cathode therefore n = 12 e
    note : please check the 3rd page of the attached pdf file for the equations of the
    anode and cathode showing ...

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    The expert examines calculating delta G and standard cell potentials.