The reaction A + B → products follows the experimentally determined rate law rate = k[B]². If [A] is doubled while [B] is held constant, what happens to the reaction rate?

Core Concept

The rate law contains [B] squared and no [A] term, so the reaction is zero order in A. Zero order means changing that concentration leaves the rate untouched. Doubling a species that does not appear in the rate law cannot change how quickly product forms, because its exponent is zero.