Final answer:
If the reaction quotient Q is greater than the equilibrium constant Keq, the reaction shifts to form more reactants. At Q equals Keq, the reaction is at equilibrium with no net change in reactant or product concentrations. If Q is less than Keq, the reaction proceeds to form more products.
Step-by-step explanation:
If the reaction quotient, Q, is greater than the equilibrium constant, Keq, the reaction will proceed in the reverse direction, or to the left as written. This occurs because there are more products present than what is preferred at equilibrium, so the reaction shifts to form more reactants in an attempt to re-establish equilibrium.
When Q equals Keq, the reaction is at equilibrium. This means that the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant over time.
If Q is less than Keq, the reaction will proceed in the forward direction, or to the right as written. There are more reactants present than desired at equilibrium, and hence, the reaction shifts to form more products to achieve equilibrium.