   Chapter 14, Problem 63GQ

Chapter
Section
Textbook Problem

At temperatures below 500 K, the reaction between carbon monoxide and nitrogen dioxideCO(g) + NO2(g) → CO2(g) + NO(g)has the following rate equation: Rate k[NO2]2. Which of the three mechanisms suggested here best agrees with the experimentally observed rate equation? Mechanism 1 Single, elementary step NO 2 + CO → CO 2 + NO Mechanism 2 Two steps Slow NO 2 + NO 2 → NO 3 + NO Fast NO 3 + CO → NO 2 + CO 2 Mechanism 3 Two steps Slow NO 2 → NO + O Fast CO + O → CO 2

Interpretation Introduction

Interpretation:

For the given reaction the mechanism involved should be determined from the given set of mechanisms using the given rate law of the reaction.

Concept introduction:

In order to establish the plausibility of a mechanism, one must compare the rate law of the rate determining step to the experimentally determined rate law.

Rate determining step: In a chemical reaction the rate determining step is the slowest step in which the rate of the reaction depends on the rate of that slowest step.

Rate law: It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.

Rate constant: The rate constant for a chemical reaction is the proportionality term in the chemical reaction rate law which gives the relationship between the rate and the concentration of the reactant present in the chemical reaction.

Rate order: The order of each reactant in a reaction is represented by the exponential term of the respective reactant present in the rate law and the overall order of the reaction is the sum of all the exponents of all reactants present in the chemical reaction. The order of the reaction is directly proportional to the concentration of the reactants.

Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo chemical reaction.

Intermediate species: It is the species formed during the middle of the chemical reaction between the reactant and the desired product.

Explanation

Given:

The rate for the given reaction is as follows,

Rate=k[NO2]2

Reason for correct answer:

The rate law of the given reaction shows that the rate of the reaction depends on the reactant NO2 and is a second order reactant.

Therefore, among the given set of mechanisms only the mechanism 2 contains two steps where two moles NO2 is reacted

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