Final answer:
The half-life of a first-order reaction is constant and does not depend on the starting concentration. This is unique to first-order reactions, as zero-order and second-order reactions do have concentration-dependent half-lives.
Step-by-step explanation:
The statement that the half-life of a first-order rate law depends on the starting concentration is false. For a first-order reaction, the half-life is a constant value that is independent of the initial concentration of the reactants. This is because in first-order reactions, the concentration of the reactant decreases by a constant fraction with each half-life, making the process independent of the amount of reactant [A] initially present. This contrasts with zero-order and second-order reactions, where the half-life does depend on the reactant's concentration.