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How do you use the Gibbs free energy equation to find the Gibbs free energy change for the oxidation of iron at 25 degrees C?
Wiki User
∙ 7y ago
The Gibbs free energy change is calculated from the expression
Δ G = Δ H - T(Δ S)
For the oxidation of iron, assuming you mean heating iron in air, where the product is black iron oxide,
3Fe + 2O2 --> Fe3O4
you need to find the enthalpy and entropy changes, which are
Δ H (formation) = - 1118.4 kJ/mol
Δ S (formation) = - 345.5 J/mol/K
Substituting into the first equation, remembering to divide the entropy value by 1000 because it's in J per mol per kelvin, not kJ, and converting the 25 degrees C to kelvin, we get:
Δ G = -1118.4 kj - 298 (- 345.5)/1000 kJ
= - 1015.441 kJ
Wiki User
∙ 7y ago
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