Final answer:
The statement in question is false because the rate law includes reactant concentrations raised to powers, which represent the reaction order, and are determined experimentally, not always aligning with the stoichiometric coefficients.
Step-by-step explanation:
The statement 'according to the rate law: the rate will always be proportional to the product of the final concentrations of the reactants, where these concentrations are raised to some exponential powers.' is false. The rate law for a chemical reaction is determined experimentally and can indeed include concentrations of reactants raised to exponential powers. However, these powers represent the reaction order and are not always the same as the stoichiometric coefficients of the reactants in the balanced chemical equation. It's also worth noting that sometimes a reactant concentration might be raised to the zero power, indicating it does not affect the rate (zero-order reaction). Therefore, while the rate can be proportional to the product of reactant concentrations raised to certain powers, these are not always simply the stoichiometric coefficients and are not associated with the 'final' concentrations, but rather with the reacting concentrations.