Final answer:
If Q > 1, the reaction favors the products, meaning the forward reaction is favored and the equilibrium shifts to the product side. The correct option is C.
Step-by-step explanation:
If Q > 1, the reaction favors the products. This means that the reaction quotient, Q, reflects a higher concentration of products than reactants in the reaction mixture, indicating that the forward reaction is favored. Hence, when comparing the choices given, the correct answer is that the reaction favors the products.
It's important to understand that Q, or the reaction quotient, is a way to gauge the direction in which a reaction at equilibrium will shift when subjected to a change. When Q is greater than 1 (Q > 1), the reaction has a greater concentration of products than what would be present at equilibrium. As a result, the equilibrium shifts to the product side to reach a new state of equilibrium.