The small is great, the great is small; all is in equilibrium in necessity... - Victor Hugo in “Les Miserables” As was discussed in Chapter 6, the natural tendency of chemical systems is to seek a state of minimum Gibbs function. Once the minimum is achieved, movement in any chemical direction will not be spontaneous. It is at this point that the system achieves a state of equilibrium. From the diagram above, it should be clear that the direction of spontaneous change is determined by minimizing \[\left(\frac{\partial G}{\partial \xi}\right)_{p,T}. \nonumber \] If the slope of the curve is negative, the reaction will favor a shift toward products. And if it is positive, the reaction will favor a shift toward reactants. This is a non-trivial point, as it underscores the importance of the composition of the reaction mixture in the determination of the direction of the reaction.