Final answer:
If Q > Kc, the system will not shift toward products but will instead shift toward reactants to reduce the ratio of product to reactant concentrations and re-establish equilibrium.
Step-by-step explanation:
If Q > Kc, the reaction quotient is greater than the equilibrium constant, indicating that the concentrations of the products are higher relative to the reactants than they would be at equilibrium. Therefore, contrary to the statement in the question, the reaction will not shift toward products to regain equilibrium; instead, the reaction will shift toward reactants. This is because the system will adjust to lower the value of Q to match Kc, thus re-establishing equilibrium by favoring the formation of more reactants.