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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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The expert examines calculating delta G and standard cell potentials.

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

equations : &#8710;G = &#8710;Gf of products - &#8710;Gf of reactants -------> standard state conditions
&#8710;H = &#8710;Hf of products - &#8710;Hf of reactants
&#8710;S = &#8710;Sf of products - &#8710;Sf of reactants
&#8710;G = -nF (Ecell)
&#8710;G = &#8710;H - T&#8710;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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