   # The reaction between ozone and nitrogen dioxide at 231 K is first-order in both [NO 2 ] and [O 3 ]. 2 NO 2 (g) + O 3 (g) → N 2 O 5 (g) + O 2 (g) (a) Write the rate equation for the reaction. (b) If the concentration of NO 2 is tripled (and [O 3 ] is not changed), what is the change in the reaction rate? (c) What is the effect on reaction rate if the concentration of O 3 is halved (with no change in [NO 2 ])? ### Chemistry & Chemical Reactivity

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

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 14, Problem 9PS
Textbook Problem
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## The reaction between ozone and nitrogen dioxide at 231 K is first-order in both [NO2] and [O3].2 NO2(g) + O3(g) → N2O5(g) + O2(g) (a) Write the rate equation for the reaction. (b) If the concentration of NO2 is tripled (and [O3] is not changed), what is the change in the reaction rate? (c) What is the effect on reaction rate if the concentration of O3 is halved (with no change in [NO2])?

(a)

Interpretation Introduction

Interpretation:

The rate equation for the reaction has to be written.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]nTotalorderof reaction = (m + n)

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

### Explanation of Solution

The rate of the reaction is given as,

Reaction Rate = k [A]n,where n is the order of the reactant.Givenreaction 2NO2(g)+  O3(g)N2O5(g)+O2<

(b)

Interpretation Introduction

Interpretation:

The change in rate of the reaction when the concentration is tripled has to be given.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]nTotalorderof reaction = (m + n)

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

(c)

Interpretation Introduction

Interpretation:

The effect on the reaction rate if the concentration of O3 is halved has to be given.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]nTotalorderof reaction = (m + n)

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

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