# 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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