Final answer:
For the reaction ClO + O ⟶ Cl + O2, the rate law is rate = k[ClO][O], and for NO2 + O ⟶ NO + O2, it is rate = k[NO2][O]. These rate laws reflect the direct proportionality to reactant concentrations for elementary reactions and are used to compare with experimentally determined rate laws.
Step-by-step explanation:
The rate law for an elementary reaction can be directly written from the reaction stoichiometry. For the reaction ClO + O ⟶ Cl + O2, the rate law would be rate = k[ClO][O], assuming this is an elementary step. This is because the rate of an elementary reaction is directly proportional to the concentration of the reactants raised to the power of their stoichiometric coefficients in the balanced equation. Similarly, for the reaction NO2 + O ⟶ NO + O2, the rate law is rate = k[NO2][O]. Both rate laws are consistent with the general form of rate = k[Reactant1][Reactant2]... for elementary reactions.
Checking the consistency with the experimentally determined rate law isn’t possible for these individual steps without additional context. However, generally, if an elementary reaction is the rate-determining step of a multi-step mechanism, its rate law should agree with the experimentally determined rate law.