When Q > K, it means the reaction quotient (Q) is larger than the equilibrium constant (K).
Implications:
- The system has too many products relative to reactants compared to equilibrium.
- To reach equilibrium, the reaction will shift to the left (toward reactants).
- The reverse reaction (products → reactants) will be favored until Q decreases to equal K.
Summary:
- Q > K → shift left → more reactants formed
- Q < K → shift right → more products formed
- Q = K → system at equilibrium, no shift
This is basically the system trying to restore balance according to Le Chatelier’s Principle.