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The rate law for the decomposition of ozone to molecular oxygen$$2 \mathrm{O}_{3}(g) \longrightarrow 3 \mathrm{O}_{2}(g)$$ is$$\text { rate }=k \frac{\left[\mathrm{O}_{3}\right]^{2}}{\left[\mathrm{O}_{2}\right]}$$The mechanism proposed for this process is $$\begin{array}{l}\mathrm{O}_{3} \frac{k_{1}}{k_{-1}} \mathrm{O}+\mathrm{O}_{2} \\\mathrm{O}+\mathrm{O}_{3} \stackrel{k_{2}}{\longrightarrow} 2\mathrm{O}_{2}\end{array}$$ Derive the rate law from these elementary steps. Clearly state the assumptions you use in the derivation. Explain why the rate decreases with increasing $\mathrm{O}_{2}$ concentration.

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rate $=\frac{k\left[\mathrm{O}_{3}\right]^{2}}{\left[\mathrm{O}_{2}\right]}$From the rate law, $\left[\mathrm{O}_{2}\right]$ is in the denominator so as the concentration of $\mathrm{O}_{2}$ increases, the rate decreases. From the first step of the mechanism, we can also see that $\mathrm{O}_{2}$ can react with $\mathrm{O}$ to form back the reactant $\mathrm{O}_{3}$ resulting in decreased reaction rate.

Chemistry 102

Chapter 6

Chemical Kinetics

Kinetics

Drexel University

University of Kentucky

University of Toronto

Lectures

22:42

In probability theory, the conditional probability of an event A given that another event B has occurred is defined as the probability of A given B, written as P(A|B). It is a function of the probability of B, the probability of A given B, and the probability of B.

04:55

In chemistry, kinetics is the study of the rates of chemical reactions. The rate of a reaction is the change in concentration of a reactant over time. The rate of reaction is dependent on the concentration of the reactants, temperature, and the activation energy of the reaction.

02:20

The rate law for the decom…

02:07

Ozone decomposes to oxygen…

02:36

The decomposition of ozone…

02:50

The ozone in the Earth…

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