Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 8, Problem 162CP

Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an important chemical used in the manufacture of plastics, synthetic rubber, and fibers, are shown below. Use bond energy values (Table 3-3) to estimate ∆E for each of the reactions.

a. Chapter 8, Problem 162CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example  1

b. Chapter 8, Problem 162CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example  2

The nitrogen-oxygen bond energy in nitric oxide (NO) is 630. kJ/mol.

c. Chapter 8, Problem 162CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example  3

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The change in energy for the given chemical reactions has to be calculated.

Concept introduction: In a chemical reaction, energy is gained, endothermic reactions, or released, exothermic reactions. The change in energy can be stated as the difference between the energy required to break the bonds in case of reactants and the energy released on the formation of the products.

To determine: The change in energy for the stated reactions.

Answer to Problem 162CP

The required energy change is -43kJ_ and 37kJ_.

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry, Chapter 8, Problem 162CP , additional homework tip  1

Figure 1

Formula

The change in energy=(energy required to breakthe bonds in reactants)-(energy released whenproducts are formed)

In the first reaction,

Chemistry, Chapter 8, Problem 162CP , additional homework tip  2

Figure 2

For first reactant,

4CH=413kJ1mol×4mol=1652kJ

2CO=358kJ1mol×2mol=716kJ

1CC=347kJ1mol×1mol=347kJ

Hence, the total energy required =(1652+716+34)kJ=2715kJ

For HCN,

1CN=891kJ1mol×1mol=891kJ

1CH=413kJ1mol×1mol=413kJ

Hence, the total energy required =(891+431)kJ=1304kJ (1)

Now, the total energy required for the reactants combined =(2715+1304)kJ=4019kJ.

Product bonds,

4CH=413kJ1mol×4mol=1652kJ

1CO=358kJ1mol×1mol=358kJ

2CC=347kJ1mol×2mol=694kJ

1CN=891kJ

1OH=467kJ

Hence,

The total energy released when the product is formed =(1652+358+694+891+467)kJ=4062kJ (2)

So the change in energy for the first reaction is,

ΔΗ=(4019-4062)kJ=-43kJ_ (Using equation (1) and (2)) (3)

In the second reaction,

Chemistry, Chapter 8, Problem 162CP , additional homework tip  3

Figure 3

For the reactant,

4CH=413kJ1mol×4mol=1652kJ

1CO=358kJ1mol×1mol=358kJ

2CC=347kJ1mol×2mol=694kJ

1CN=891kJ

1OH=467kJ

Hence,

The total energy released when the product is formed =(1652+358+694+891+467)kJ=4062kJ (4)

For product,

3CH=413kJ1mol×3mol=1239kJ

1C=C=614kJ1mol×1mol=614kJ

1CC=347kJ1mol×1mol=347kJ

1CN=891kJ

Hence,

The total energy released when the product is formed =(1239+614+891+347)kJ=3091kJ (5)

For water,

2OH=2mol×467kJ/mol=934kJ

So, the total energy of products =(3091+934)kJ=4025kJ (6)

So the change in energy for the second reaction is,

ΔΗ=(4062-4025)kJ=37kJ_ (Using equation (4) and (6))

Conclusion

The change in energy can be stated as the difference between the energy required to break the bonds in case of reactants and the energy released on the formation of the products.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The change in energy for the given chemical reactions has to be calculated.

Concept introduction: In a chemical reaction, energy is gained, endothermic reactions, or released, exothermic reactions. The change in energy can be stated as the difference between the energy required to break the bonds in case of reactants and the energy released on the formation of the products.

To determine: The change in energy for the stated reactions.

Answer to Problem 162CP

The required energy change is -850kJ_.

Explanation of Solution

Given

The given reaction is,

Chemistry, Chapter 8, Problem 162CP , additional homework tip  4

Figure 4

For the reactant side,

For H2C=CHCH3,

6CH=413kJ1mol×6mol=2478kJ

1C=C=614kJ1mol×1mol=614kJ

1CC=347kJ1mol×1mol=347kJ

The energy required =4×(2478+614+347)kJ=13756kJ (since 4 molecules are present) (1)

For NO,

6NO=(6×630)kJ=3780kJ (2)

Total reactant energy =13756+3780kJ=17536kJ (using equation (1) and (2)) (3)

For products,

For H2C=CHCN,

3CH=413kJ1mol×3mol=1239kJ

1C=C=614kJ1mol×1mol=614kJ

1CC=347kJ1mol×1mol=347kJ

1CN=891kJ

The total energy is =4×(1239+614+891+347)kJ=12364kJ (since, 4 molecules are formed) (4)

For H2O,

2OH=467kJ1mol×2mol=934kJ

Since 6 molecules are formed, energy =(6×934)kJ=5604kJ (5)

For N2,

1NN=418kJ1mol×1mol=418kJ (6)

The total energy for products is =(12364+5604+418)kJ=18286kJ (7)

So the change in energy for the second reaction is,

ΔΗ=(17536-18386)kJ=-850kJ_ (Using equation (3) and (7))

Conclusion

The change in energy can be stated as the difference between the energy required to break the bonds in case of reactants and the energy released on the formation of the products.

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The change in energy for the given chemical reactions has to be calculated.

Concept introduction: In a chemical reaction, energy is gained, endothermic reactions, or released, exothermic reactions. The change in energy can be stated as the difference between the energy required to break the bonds in case of reactants and the energy released on the formation of the products.

To determine: The change in energy for the stated reactions.

Answer to Problem 162CP

The required energy change is -1077kJ_.

Explanation of Solution

Given

For the given reaction,

Chemistry, Chapter 8, Problem 162CP , additional homework tip  5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6CH=413kJ1mol×6mol=2478kJ

1C=C=614kJ1mol×1mol=614kJ

1CC=347kJ1mol×1mol=347kJ

Total energy =2×(2478+614+347)kJ=6878kJ (1)

(since 2 molecules are formed)

For NH3,

3NH=391kJ1mol×3mol=1173kJ

Total energy =2×1173kJ=2346kJ (2)

(since 2 molecules are formed)

For O2,

1O=O=495kJ1mol×1mol=495kJ (3)

The total energy of reactants =(6878+2346+495)kJ=10709kJ (4)

Energy for products,

For H2C=CHCN,

3CH=413kJ1mol×3mol=1239kJ

1C=C=614kJ1mol×1mol=614kJ

1CC=347kJ1mol×1mol=347kJ

1CN=891kJ

The total energy =2×(1239+614+891+347)kJ=6182kJ (5)

(since 2 molecules are formed)

For H2O,

2OH=467kJ1mol×2mol=934kJ

Since 6 molecules are formed, energy =(6×934)kJ=5604kJ (6)

The total energy for products =(6182+5604)kJ=11786kJ (7)

So the change in energy for the second reaction is,

ΔΗ=(10709-11786)kJ=-1077kJ_ (Using equation (4) and (7))

Conclusion

The change in energy can be stated as the difference between the energy required to break the bonds in case of reactants and the energy released on the formation of the products.

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Chapter 8 Solutions

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