Obviously as the reaction proceeds the mole fraction

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Unformatted text preview: G = nA dµA + nB dµB + nC dµC + nD dµD + µA dnA + µB dnB + µC dnC + µD dnD Invoking the Gibbs- Duhem equation, the sum of the first four terms can be taken as 0. We now define the extent of reaction by the quantity ξ. This quantity will allow us to track how much of the products have formed. At the beginning of the reaction ξ = 0 (if we start with a reactive mixture containing initially only A and B molecules). We arbitrarily define ξ by: dξ = dnC so, on the basis of the reaction stoichiometry, we write dnA = - dξ dnB = - 2 dξ dnD = 3 dξ Therefore dG is written as: dG = dξ (µC + 3 µD - µA - 2 µB) or $ ∂G ' & ) = µ C + 3µ D − µ A − 2µ B = Δ RG % ∂ξ (P,T € 190 So we conclude that the change in Gibbs free energy, G, with extent of reaction...
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