shifting of equilibrium Does it mean that if one side of a reaction is favoured, the reaction will shift to the other side? As I was reading up on the van't Hoff equation, it says that an increase in temperature of an endothermic reaction will favour the products. It also showed a graph where lnK increases with temperature (T). But I thought what would happen in this case is the reactants will be favoured and then the equilibrium will shift to the right to de-stress the equilibrium?

So in summary, I'm just quite confused about what it means by favouring a side of an equilibrium.
In general, a equilibrium will shift in a direction that opposes the stress that was placed on the system. For example, if you add heat to an endothermic reaction, you will receive more products, as this will lower the temperature of the solution. When you have the dissociation of an acid, the acid will dissociate more (act like an acid) when you make the solution more basic. An equilibrium will shift to minimize any change in a system, so when evaluating what will happen after a system is stressed, look to see which side of the equilibrium relives that stress, and that side will be favored.