Say I have an exothermic reaction, whose change in Entropy is positive. (not the most common of reactions, but it can still happen) If I increase the temperature, by La Chatlier's principle, the reaction should move to the left. However, by Gibbs free energy, if I increase the temperature, the second term (dH - TdS) TdS, becomes more positive (and thus Gibb's free energy becomes more negative). So the reaction should move to the right? So is La Chatlier's just a guiding tool for the majority of reactions, and not always correct? Like in this situation.