Le Chatelier's Principle Basics
Think of equilibrium as a perfectly balanced seesaw that doesn't want to be disturbed. When you mess with the conditions, the system fights back to restore balance - that's Le Chatelier's principle in action.
Concentration changes are the easiest to understand. Add more reactants? The reaction shifts right to make more products. Flood the system with products? It shifts left to create more reactants. The system is essentially trying to use up whatever you've added.
Temperature changes depend on whether your reaction gives out heat (exothermic) or takes in heat (endothermic). Crank up the temperature and equilibrium favours the endothermic direction - it's trying to absorb that extra heat you've added.
Quick tip: Remember that increasing temperature always favours the endothermic direction, whilst decreasing temperature favours the exothermic direction.
