The rate equation for the reaction of CH3 CH2 Br with ^- OH is: rate =k[CH3 CH2 Br][ ^- OH] Wha

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The rate equation for the reaction of CH3 CH2 Br with ^- OH...

The rate equation for the reaction of $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}$ with ${ }^{-} \mathrm{OH}$ is: rate $=\mathrm{k}\left[\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}\right]\left[{ }^{-} \mathrm{OH}\right]$ What effect does the indicated concentration change have on the overall rate of the reaction? a. tripling the concentration of $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}$ only b. tripling the concentration of $^{-} \mathrm{OH}$ only c. tripling the concentration of both $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}$ and ${ }^{-} \mathrm{OH}$

The rate equation for the reaction of $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}$ with ${ }^{-} \mathrm{OH}$ is: rate $=\mathrm{k}\left[\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}\right]\left[{ }^{-} \mathrm{OH}\right]$
What effect does the indicated concentration change have on the overall rate of the reaction?
a. tripling the concentration of $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}$ only
b. tripling the concentration of $^{-} \mathrm{OH}$ only
c. tripling the concentration of both $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Br}$ and ${ }^{-} \mathrm{OH}$

Key Concepts

Rate Law

The rate law is an expression that relates the speed of a chemical reaction to the concentrations of its reactants. It specifies how the reaction rate depends on changes in the concentrations, with the rate constant k being a proportionality factor that carries information about the specific reaction and its conditions.

Reaction Order

The reaction order refers to the powers to which the concentrations of reactants are raised in the rate equation. For instance, if the rate is directly proportional to the concentration of each reactant (each raised to the first power), the reaction is first order with respect to each reactant. The overall reaction order is the sum of the orders with respect to each reactant, which influences how the rate responds to simultaneous changes in concentrations.

Effect of Concentration Changes

Small changes in the concentrations of reactants can have a significant impact on the reaction rate based on the reaction order. For example, if the concentration of one reactant is tripled in a first order reaction, the rate will triple, while if both reactants are tripled in a bimolecular (second order overall) reaction, the rate increases by a factor of nine because the effects are multiplicative.

Bimolecular Reactions

Bimolecular reactions involve two reactants coming together in the rate-determining step, resulting in a rate law that is typically first order in each reactant. This means that the overall reaction is second order, and the rate is directly proportional to the product of the two concentrations. Understanding this concept is crucial for predicting how simultaneous changes in multiple reactant concentrations affect the reaction rate.

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