General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 14, Problem 14.14QP

(a)

Interpretation Introduction

Interpretation: The rate law for the given reaction has to be deduced.

Concept Introduction:

Rate law: An expression relating the rate of a reaction to the rate constant and concentrations of the reactants that are involved in the reaction.

For a given type of reaction:

aA+bBcC+dD

The rate law takes the form as:

Rate=k[A]x[B]y

k= Rate constant. It is the constant of proportionality between the rate of a reaction and the concentration of the reactants. Its unit is s-1.

[A]-Concentration of the reactant A in molarity.

[B]-Concentration of the reactant B in molarity.

It is important to note that x and y are not related to a and b.

Rather, they are determined experimentally.

(a)

Expert Solution
Check Mark

Explanation of Solution

The reaction to be considered is:

F2(g)+2ClO2(g)2FClO2(g)

General Chemistry, Chapter 14, Problem 14.14QP , additional homework tip  1

Figure 1

In this table:

The data entries in 1st and 3rd columns show the following observations:

  • While holding [ClO2] as constant, if [F2] is doubled then the rate of the reaction is also doubled. Therefore, the rate of the reaction is directly proportional to the concentration of F2.
  • While holding [F2] as constant, if [ClO2] is quadruple then the rate of the reaction is increased by four times. Therefore, the rate of the reaction is also directly proportional to the concentration of ClO2.

The experimental observations tell that the rate of the reaction is dependent on the concentrations of the reactants such as F2 and ClO2.

So, the rate law for the reaction takes the form as:

Rateα[F2][ClO2]Rate=k[F2][ClO2]

(b)

Interpretation Introduction

Interpretation:  The rate constant of the considered reaction has to be calculated.

Concept Introduction:

Rate constant:

k= Rate constant. It is the constant of proportionality between the rate of a reaction and the concentration of the reactants. Its unit is s-1.

For a given type of reaction:

aA+bBcC+dD

The rate law takes the form as:

Rate=k[A]x[B]y

The rate constant takes the form as:

Rate=k[A]x[B]yk=Rate[A]x[B]y

It is important to note that x and y are not related to a and b.

Rather, they are determined experimentally.

(b)

Expert Solution
Check Mark

Answer to Problem 14.14QP

The rate constant of the reaction is k=1.2M1s-1.

Explanation of Solution

The reaction to be considered is:

F2(g)+2ClO2(g)2FClO2(g)

General Chemistry, Chapter 14, Problem 14.14QP , additional homework tip  2

Figure 1

Among the three experiments in the table, data of any one experiment can be considered to calculate the rate constant for the reaction.

The rate law takes the form as:

Rate=k[F2][ClO2]

The rate constant takes the form as:

Rate=k[F2][ClO2]k=Rate[F2][ClO2]

Considering the 3rd experiment:

[F2]=0.20M[ClO2]=0.010MRate=2.4×103M/s

k=Rate[F2][ClO2]=2.4×103M/s(0.20M)×(0.010M)=1.2M1s-1

Therefore, the rate constant of the reaction is k=1.2M1s-1

Conclusion

The rate constant of the considered reaction has been calculated.

(c)

Interpretation Introduction

Interpretation: From the given data, the rate of the reaction has to be calculated.

Concept Introduction:

The rate of a reaction is the measure of how fast a reactant is consumed or a product is formed. It can be calculated using the rate law expression.

For a given type of reaction:

aA+bBcC+dD

The rate law takes the form as:

Rate=k[A]x[B]y

k= Rate constant. It is the constant of proportionality between the rate of a reaction and the concentration of the reactants. Its unit is s-1.

[A]-Concentration of the reactant A in molarity.

[B]-Concentration of the reactant B in molarity.

It is important to note that x and y are not related to a and b.

Rather, they are determined experimentally.

(c)

Expert Solution
Check Mark

Answer to Problem 14.14QP

The rate of the reaction is 2.4×104Ms-1.

Explanation of Solution

The reaction to be considered is:

F2(g)+2ClO2(g)2FClO2(g)

Given data:

[F2]=0.010M[ClO2]=0.020M

It is known that k=1.2M1s-1

Rate=k[F2][ClO2]=(1.2M1s-1)×(0.010M)×(0.020M)=2.4×104Ms-1

Therefore, the rate of the reaction is 2.4×104Ms-1.

Conclusion

From the given data, the rate of the reaction has been calculated.

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Chapter 14 Solutions

General Chemistry

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