Final answer:
To determine which direction the reaction proceeds, we compare Q to K. In the absence of K or a chemical equation, we cannot definitively say which direction the reaction will proceed with given equal initial concentrations.
Step-by-step explanation:
To determine the direction in which a reaction proceeds toward equilibrium, we need to compare the reaction quotient, Q, with the equilibrium constant, K. If Q is less than K, the reaction will proceed to the right as written, indicating that the reactants will be converted to products. If Q is greater than K, the reaction proceeds to the left, converting products back to reactants. In the case where Q equals K, the system is already at equilibrium, and no net change occurs.
Since the question does not provide a value for K or a chemical equation, we can only make an assumption based on the given initial conditions ([X] = [Y] = [Z] = 1.0 M). Without additional information, we cannot specify whether the reaction will proceed to the right or left. However, typically in a reaction where all reactant and product concentrations start at the same value and no further information is given, we might assume that the reaction will proceed in the forward direction (to the right) to form more products. Yet, this is not a definitive conclusion without knowing the equilibrium constant.