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The reaction of NO 2 (g) and CO(g) is thought to occur in two steps to give NO and CO 2 : Step 1: Slow NO 2 (g) + NO 2 (g) → NO(g) + NO 3 (g) Step 2: Fast NO 3 (g) + CO(g) → NO 2 (g) + CO 2 (g) (a) Show that the elementary steps add up to give the overall, stoichiometric equation. (b) What is the molecularity of each step? (c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? (d) Identify any intermediates in tins reaction.

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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 14, Problem 46PS
Textbook Problem
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The reaction of NO2(g) and CO(g) is thought to occur in two steps to give NO and CO2:

Step 1: Slow

NO2(g) + NO2(g) → NO(g) + NO3(g)

Step 2: Fast

NO3(g) + CO(g) → NO2(g) + CO2(g)

  1. (a) Show that the elementary steps add up to give the overall, stoichiometric equation.
  2. (b) What is the molecularity of each step?
  3. (c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation?
  4. (d) Identify any intermediates in tins reaction.

(a)

Interpretation Introduction

Interpretation:

For the given reactions, it has to be shown that the elementary steps add up to give the overall, stoichiometric equation.

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. 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.

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

Molecularity: The molecularity of the reaction actually denotes the number of species that present in the rate determining step of the reaction.

Explanation of Solution

The overall chemical reaction can be obtained by the given elementary steps.

The sum of elementary steps results in an equation which contains equal species on the reactant and the product side that cancels each other and finally leads to the overall chemical equation as follows,

    NO2(g)+NO2(g)NO(g)+NO3(g)NO3(g)+CO(g)NO2(g)+CO2(g</

(b)

Interpretation Introduction

Interpretation:

The molecularity of each step has to be determined.

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. 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.

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

Molecularity: The molecularity of the reaction actually denotes the number of species that present in the rate determining step of the reaction.

(c)

Interpretation Introduction

Interpretation:

The experimental rate equation which gives that the given mechanism is consistent with kinetic data

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. 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.

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

Molecularity: The molecularity of the reaction actually denotes the number of species that present in the rate determining step of the reaction.

(d)

Interpretation Introduction

Interpretation:

The intermediates in the given reaction have to be determined.

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. 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.

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

Molecularity: The molecularity of the reaction actually denotes the number of species that present in the rate determining step of the reaction.

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Chapter 14 Solutions

Chemistry & Chemical Reactivity
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Ch. 14.4 - Using the rate constant for HI decomposition given...Ch. 14.4 - The catalyzed decomposition of hydrogen peroxide...Ch. 14.4 - Americium is used in smoke detectors and in...Ch. 14.4 - The decomposition of N2O5 is a first-order...Ch. 14.4 - Which of the following will confirm that the...Ch. 14.4 - 3. The equation for the decomposition of NO2(g) at...Ch. 14.5 - Rate constants were determined for the...Ch. 14.5 - The colorless gas N2O4, decomposes to the brown...Ch. 14.5 - Which of the following graphs will produce a...Ch. 14.5 - 2. 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