🤓 Based on our data, we think this question is relevant for Professor Keister's class at UB.

** Arrhenius Equation**:

$\overline{){\mathbf{k}}{\mathbf{=}}{{\mathbf{Ae}}}^{\mathbf{-}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{RT}}}{\mathbf{}}}$

*Ratio of rate constant for catalyzed to uncatalyzed:*

$\frac{{\mathbf{k}}_{\mathbf{catalyzed}}}{{\mathbf{k}}_{\mathbf{uncatalyzed}}}\mathbf{=}\frac{\overline{)\mathbf{A}}{\mathbf{e}}^{\mathbf{-}\frac{{\mathbf{E}}_{\mathbf{a}\mathbf{,}\mathbf{cat}\mathbf{.}}}{\mathbf{RT}}}}{\overline{)\mathbf{A}}{\mathbf{e}}^{\mathbf{-}\frac{{\mathbf{E}}_{\mathbf{a}\mathbf{,}\mathbf{uncat}\mathbf{.}}}{\mathbf{RT}}}}$

T = 25°C + 273 = **298 K**

One mechanism for the destruction of ozone in the upper atmosphere is

c. E_{a} for the uncatalyzed reaction

O_{3} (g) + O (g) → 2O_{2} (g)

is 14.0 kJ. E_{a} for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25°C? Assume that the frequency factor A is the same for each reaction.

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Based on our data, we think this problem is relevant for Professor Keister's class at UB.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.