Answer and Explanation:
If the standard free energy change [ΔGo'] for the reaction A + B > Y + Z equals zero (0), then you would correctly predict that this reaction is at equilibrium.
The standard free energy change, ΔGo', measures the spontaneity of a chemical reaction. A ΔGo' value of zero indicates that the forward and reverse reactions have equal tendencies to occur, meaning the reaction is in equilibrium. At equilibrium, the concentrations of the reactants and products remain constant over time, with the forward and reverse reactions occurring at the same rate.
In the given reaction A + B > Y + Z, if the ΔGo' is zero, it means that the reaction is neither thermodynamically favored nor disfavored. Both the forward and reverse reactions have equal tendencies to occur, resulting in a state of equilibrium where the concentrations of A, B, Y, and Z remain constant.
To summarize, if the standard free energy change ΔGo' for the reaction A + B > Y + Z equals zero, it correctly predicts that the reaction is at equilibrium.