Chemistry: The Molecular Nature of Matter and Change - Standalone book
Chemistry: The Molecular Nature of Matter and Change - Standalone book
7th Edition
ISBN: 9780073511177
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 16, Problem 16.81P

(a)

Interpretation Introduction

Interpretation:

If [NO2] is doubled, then rate quadruples, then the rate law for the given reaction (1) has to be predicted.

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.

(a)

Expert Solution
Check Mark

Explanation of Solution

The overall rate law of reaction (1) is,

Rate =  k [A]m[B]n=  k [NO2]m[CO]n

When [NO2] increases by a factor of 2, the rate increases by a factor of 4.

While considering only the concentration of [NO2], the reaction rate becomes,

Rate1 =  k [NO2]1m;Rate2 =  k [NO2]2mRate2Rate1 =  k [NO2]2m[NO2]1mratioofrateis4;[NO2]increasesbyafactorof2,thus4 = [2]mm=2

So, Rate = k [NO2]m[CO]n

Totalorderofreaction(Second order):m + n = 22 + n = 2n=22=0.

The overall order of the reaction is SECOND; but the order with respect to [CO] is ZERO ORDER.

Therefore, the overall reaction rate law is Rate = k [NO2]2[CO]0(or) k [NO2]2.

(b)

Interpretation Introduction

Interpretation:

If [NO] is doubled, then rate doubles, then the rate law for the given reaction (2) has to be predicted.

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.

(b)

Expert Solution
Check Mark

Explanation of Solution

The overall rate law of reaction (2) is,

Rate =  k [A]m[B]n=  k [NO]m[O3]n

When [NO] increases by a factor of 2, the rate increases by a factor of 2.

While considering only the concentration of [NO], the reaction rate becomes,

Rate1 =  k [NO]1m;Rate2 =  k [NO]2mRate2Rate1 =  k [NO]2m[NO]1mratioofrate is 2;[NO]increasesbyafactorof2,thus2 = [2]mm=1

So, Rate = k [A]m[B]n=  k [NO]m[O3]n

Totalorderofreaction(Second order):m + n = 21 + n = 2n=21=1.

The overall order of the reaction is SECOND; but the order with respect to [O3] is FIRST ORDER.

Therefore, the overall reaction rate law is Rate = k [NO]1[O3]1.

(c)

Interpretation Introduction

Interpretation:

The ratio of the initial rate to the rate when the reaction is 50% complete has to be determined.

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)

Expert Solution
Check Mark

Explanation of Solution

When the concentrations of the reactants are reduced to one-half of the initial concentration, then the reaction is considered as 50% completion.

For reaction (1):

The concentration [NO2] decreases by one-half its initial during 50% of reaction completion.

Rateinitial =  k [NO2]2;Rate50% =  k [0.5×NO2]2RateinitialRate50% = [NO2]2[0.5×NO2]2=4

For reaction (2):

The concentration [NO]and[O3] decreases by one-half its initial during 50% of reaction completion.

Rateinitial =  k [NO]1[O3]1;Rate50% =  k [0.5×NO]1[0.5×O3]1RateinitialRate50% = [NO]1[O3]1 k [0.5×NO]1[0.5×O3]1=4.

Therefore, the ratio of the initial rate to the rate when the reaction is 50% complete was calculated as shown above.

(d)

Interpretation Introduction

Interpretation:

The ratio of the initial rate to the rate when the reaction is 50% complete when the initial [NO2] is twice the initial [CO] has to be determined.

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.

(d)

Expert Solution
Check Mark

Explanation of Solution

When the concentrations of the reactants are reduced to one-half of the initial concentration, then the reaction is considered as 50% completion.

For reaction (1):

The ratio of the initial rate to the rate when the reaction is 50% complete when the initial [NO2] is twice the initial [CO]

[NO2]initial=  2[CO]initial; [CO]=(12)[CO]initial;[NO2]=(0.75)[NO2]initial

Rateinitial =  k [NO2]2;Rate50% =  k [0.5×NO2]2RateinitialRate50% = [NO2]2[0.75×NO2]2=1.778=1.8

Therefore, the ratio of the initial rate to the rate when the reaction is 50% complete was calculated as shown above.

(e)

Interpretation Introduction

Interpretation:

The ratio of the initial rate to the rate when the reaction is 50% complete when the initial [NO] is twice the initial [O3] has to be determined.

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.

(e)

Expert Solution
Check Mark

Explanation of Solution

When the concentrations of the reactants are reduced to one-half of the initial concentration, then the reaction is considered as 50% completion.

For reaction (2):

The ratio of the initial rate to the rate when the reaction is 50% complete when the initial [NO] is twice the initial [O3].

[NO]initial=  2[O3]initial; [O3]=(12)[O3]initial;[NO]=(0.75)[NO]initial

Rateinitial =  k [NO][O3];Rate50% =  k [0.75×NO][0.5×O3]RateinitialRate50% = [NO][O3][0.75×NO][0.5×O3]=2.6667=2.7.

Therefore, the ratio of the initial rate to the rate when the reaction is 50% complete was calculated as shown above.

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Chapter 16 Solutions

Chemistry: The Molecular Nature of Matter and Change - Standalone book

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