Final answer:
The claim that the rate law for the reaction A₂ + 2B₂ → 2AB₂ has orders of 1 for A₂ and 2 for B₂ is false; the reaction orders must be determined experimentally and cannot be inferred directly from the stoichiometric coefficients.
Step-by-step explanation:
The statement that for the general equation A₂ + 2B₂ → 2AB₂, the rate law for the reaction is rate = k [A₂]ᵦ [B₂]ᵡ, where the exponent p must be 1 and q must be 2, is false. The stoichiometric coefficients of a balanced chemical equation do not necessarily determine the reaction orders in a rate law. Instead, the reaction order for each reactant must be determined experimentally. Therefore, without empirical data showing how the concentration of A₂ and B₂ affects the reaction rate, one cannot assert the exact values of p and q.