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Consider the following chemiluminescent (gives off light) chemical reaction between the pollutant...

Question:

Consider the following chemiluminescent (gives off light) chemical reaction between the pollutant nitric oxide and the photochemical pollutant ozone.

{eq}\rm O_3 + NO \to NO_2 + O_2{/eq}

In one laboratory experiment, the rate of disappearance of ozone (O{eq}_3{/eq}) was measured to be 6.0 x 10{eq}^{-4}{/eq} M/s. Simultaneously, the concentration of ozone was measured to be 9.0 x 10{eq}^{-6}{/eq} M and the concentration of nitric oxide (NO) was measured to be 2.5 x 10{eq}^{-6}{/eq} M. Given that this chemiluminescent chemical reaction follows the rate law {eq}\rm \text{rate} = \textit{k}\;[O_3][NO] {/eq}, calculate the rate constant, k.

Rate Constant:

The rate of a reaction can be expressed as either the rate of disappearance of a reactant or rate of appearance of product.

The rate constant, k, of a reaction is a proportionality constant relating the rate of a reaction to the product of the individual reactant concentrations raised to their respective orders of reaction. This rate constant is temperature dependent.

Answer and Explanation: 1

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Given,

{eq}\rm O_3 + NO \to NO_2 + O_2{/eq}

Rate of disappearance of ozone = {eq}\rm 6.0 \times 10^{-4}\;Ms^{-1}{/eq}

Concentration of NO is...

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Rate Constant and Rate Laws

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Chapter 12 / Lesson 2
14K

Rate law is defined as the relationship between the rate of reaction and the concentration of the reactants. Learn about rate law, rate constant, and how to use rate law equations to determine reaction order for one or two reactants.


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