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Manasa pointed out that a reaction will be spontaneous at low Gibbs energy, but as a whole reactions will proceed until they are at equilibrium where ΔG=0. Since ΔG = ΔGº + RT lnQ and ΔGº= -RT lnK, ΔG=0 when Q=K. Essentially, the reaction tries to minimize its Gibbs free energy as it proceeds towards equilibrium. A spontaneous process (ΔG<0) means that the forward reaction taking place will bring the reaction closer to equilibrium, and a nonspontaneous process (ΔG>0) means that the reverse reaction taking place will bring the reaction closer to equilibrium.
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