If the reaction were to shift in the forward

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: ln' 1 2 ' (a A ) (aB ) * & ) Δ RG = Δ RG∅ + RT ln(Q) Where ΔRG is the Standard Reaction Gibbs Free Energy, which is easily ∅ € calculated from the Standard Formation Gibbs Free Energies of the substances (using the ΔFG values for each substance in the thermodynamic ∅ tables) and where Q is called the reaction quotient. At equilibrium, we have ΔRG = 0, which leads to: ΔRG = - RT ln(Keq) where Keq is called the equilibrium constant (value of the ∅ reaction quotient when the reaction has reached equilibrium and the mole fractions of reactants and products have their final “equilibrium” values). Note that if the equilibrium constant is larger than one, this implies a reaction where products are more stable than the reactants. Practically speaking, the equilibrium constant can be calculated for any chemical reaction at 298K, since at that temperature we can easily...
View Full Document

Ask a homework question - tutors are online