Final answer:
The rate equation for the reaction CH₃CH₂CH₂CHBrCH₃ with NaN₃ is most likely first order with respect to the alkyl halide, expressed as Rate = k[CH₃CH₂CH₂CHBrCH₃], but without specific experimental data for this reaction, the exact rate law cannot be definitively determined.
Step-by-step explanation:
To determine the rate equation for the reaction CH₃CH₂CH₂CHBrCH₃ with NaN₃, we need to consider the experimental evidence on how the reaction rates change with varying concentrations of reactants. Rate laws are determined experimentally, and typically, the concentration of each reactant is raised to a power equal to the order of the reaction with respect to that reactant. The examples provided refer to different reactions, illustrating that reactions can be first order with respect to one reactant or second order overall depending on how the rate is affected by changes in reactant concentrations.
In this particular case, given the information provided and the typical behavior of nucleophilic substitution reactions, the most likely rate equation would be Rate = k[CH₃CH₂CH₂CHBrCH₃], indicating a first-order dependence on the concentration of the alkyl halide. This is because the reaction likely involves a rate-determining step where the azide ion (N₃⁻) attacks the alkyl halide, forming the product and releasing a bromide ion (Br⁻).
It's important to note, however, that without experimental data specifically for this reaction, we cannot definitively say which rate law is correct. The provided examples, such as for the reaction rate = k[(CH₃)₃C Br], suggest that a similar alkyl halide reaction is first-order with respect to the alkyl halide and independent of water, but this does not directly provide the rate law for the reaction in question.