Final answer:
The rate law for the elementary reaction O₃(g) + NO(g) → O₂(g) + NO₂(g) is given by rate = k[O₃][NO], reflecting the direct proportionality of the reaction rate to the concentrations of both ozone and nitrogen monoxide.
Step-by-step explanation:
To write the rate law for the given elementary reaction where ozone (O₃) reacts with nitrogen monoxide (NO) to form oxygen (O₂) and nitrogen dioxide (NO₂), it is essential to know that elementary reactions have rate laws that are directly deducible from their stoichiometry. For an elementary reaction, the rate law expression is based on the molecularity of the reaction, which refers to the number of molecules participating in the reaction step. Since the given reaction involves a collision between two molecules of different substances, it can be classified as a bimolecular reaction.
The rate law for the reaction O₃(g) + NO(g) → O₂(g) + NO₂(g) can be written as:
rate = k[O₃][NO]
In this expression, 'k' represents the rate constant for the reaction at a given temperature, and [O₃] and [NO] represent the concentrations of ozone and nitrogen monoxide, respectively. Because this reaction involves one molecule of O₃ and one molecule of NO, the rate law indicates that the reaction rate is directly proportional to the concentration of both reactants.