Calculating delta G and standard cell potential
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 ...
Solution Summary
The expert examines calculating delta G and standard cell potentials.
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