Yeah, basically Le Chatelier's principle means that if you change something in an equilibrium, the system will move so as to restore it to the original conditions. So if you you have a reaction where the forward one is exothermic (say the Haber process, N2 + 3H2 --> 2NH3), then if you increase the temperature, the equilibrium will shift to the left (because the equilibrium favours the backward endothermic reaction, in order to absorb the extra heat produced). Similarly, in the above example if you increase the pressure, the equilibrium will shift to the right because it favours the reaction that reduces the pressure, ie the reaction that produces less gas molecules. Hope that made sense.