Three processes that have been used for the industrial manufacture of acrylonitrile (CH 2 CHCN), 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. b. The nitrogen-oxygen bond energy in nitric oxide (NO) is 630. kJ/mol. c.

Question

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Answer 1

Textbook Question

Chapter 3, Problem 152CP

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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 1

b. Chapter 3, Problem 152CP, 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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 3

(a)

Expert Solution

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 152CP

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

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , 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: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 2

Figure 2

For first reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

2 C−O = 358 kJ1 mol×2 mol=716 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For HC≡N,

1 C≡N = 891 kJ1 mol×1 mol=891 kJ

1 C−H = 413 kJ1 mol×1 mol=413 kJ

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

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

Product bonds,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

So the change in energy for the first reaction is,

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

In the second reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 3

Figure 3

For the reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

For product,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

Hence,

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

For water,

2 O−H = 2 mol×467 kJ/mol = 934 kJ

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

So the change in energy for the second reaction is,

ΔΗ=(4062-4025) kJ = 37 kJ_ (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

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 152CP

The required energy change is -850 kJ_.

Explanation of Solution

Given

The given reaction is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 4

Figure 4

For the reactant side,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For NO,

6 NO = (6×630) kJ = 3780 kJ (2)

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

For products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

For N2,

1 N−N = 418 kJ1 mol×1 mol=418 kJ (6)

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

So the change in energy for the second reaction is,

ΔΗ=(17536-18386) kJ = -850 kJ_ (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

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 152CP

The required energy change is -1077 kJ_.

Explanation of Solution

Given

For the given reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

(since 2 molecules are formed)

For NH3,

3 N−H = 391 kJ1 mol×3 mol=1173 kJ

Total energy =2×1173 kJ=2346 kJ (2)

(since 2 molecules are formed)

For O2,

1 O=O = 495 kJ1 mol×1 mol=495 kJ (3)

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

Energy for products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

(since 2 molecules are formed)

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

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

So the change in energy for the second reaction is,

ΔΗ=(10709-11786) kJ = -1077 kJ_ (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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Answer 2

Textbook Question

Chapter 3, Problem 152CP

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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 1

b. Chapter 3, Problem 152CP, 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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 3

(a)

Expert Solution

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 152CP

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

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , 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: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 2

Figure 2

For first reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

2 C−O = 358 kJ1 mol×2 mol=716 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For HC≡N,

1 C≡N = 891 kJ1 mol×1 mol=891 kJ

1 C−H = 413 kJ1 mol×1 mol=413 kJ

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

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

Product bonds,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

So the change in energy for the first reaction is,

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

In the second reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 3

Figure 3

For the reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

For product,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

Hence,

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

For water,

2 O−H = 2 mol×467 kJ/mol = 934 kJ

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

So the change in energy for the second reaction is,

ΔΗ=(4062-4025) kJ = 37 kJ_ (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

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 152CP

The required energy change is -850 kJ_.

Explanation of Solution

Given

The given reaction is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 4

Figure 4

For the reactant side,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For NO,

6 NO = (6×630) kJ = 3780 kJ (2)

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

For products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

For N2,

1 N−N = 418 kJ1 mol×1 mol=418 kJ (6)

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

So the change in energy for the second reaction is,

ΔΗ=(17536-18386) kJ = -850 kJ_ (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

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 152CP

The required energy change is -1077 kJ_.

Explanation of Solution

Given

For the given reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

(since 2 molecules are formed)

For NH3,

3 N−H = 391 kJ1 mol×3 mol=1173 kJ

Total energy =2×1173 kJ=2346 kJ (2)

(since 2 molecules are formed)

For O2,

1 O=O = 495 kJ1 mol×1 mol=495 kJ (3)

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

Energy for products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

(since 2 molecules are formed)

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

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

So the change in energy for the second reaction is,

ΔΗ=(10709-11786) kJ = -1077 kJ_ (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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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Textbook Question

Chapter 3, Problem 152CP

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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 1

b. Chapter 3, Problem 152CP, 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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 3

(a)

Expert Solution

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 152CP

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

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , 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: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 2

Figure 2

For first reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

2 C−O = 358 kJ1 mol×2 mol=716 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For HC≡N,

1 C≡N = 891 kJ1 mol×1 mol=891 kJ

1 C−H = 413 kJ1 mol×1 mol=413 kJ

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

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

Product bonds,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

So the change in energy for the first reaction is,

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

In the second reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 3

Figure 3

For the reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

For product,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

Hence,

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

For water,

2 O−H = 2 mol×467 kJ/mol = 934 kJ

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

So the change in energy for the second reaction is,

ΔΗ=(4062-4025) kJ = 37 kJ_ (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

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 152CP

The required energy change is -850 kJ_.

Explanation of Solution

Given

The given reaction is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 4

Figure 4

For the reactant side,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For NO,

6 NO = (6×630) kJ = 3780 kJ (2)

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

For products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

For N2,

1 N−N = 418 kJ1 mol×1 mol=418 kJ (6)

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

So the change in energy for the second reaction is,

ΔΗ=(17536-18386) kJ = -850 kJ_ (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

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 152CP

The required energy change is -1077 kJ_.

Explanation of Solution

Given

For the given reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

(since 2 molecules are formed)

For NH3,

3 N−H = 391 kJ1 mol×3 mol=1173 kJ

Total energy =2×1173 kJ=2346 kJ (2)

(since 2 molecules are formed)

For O2,

1 O=O = 495 kJ1 mol×1 mol=495 kJ (3)

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

Energy for products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

(since 2 molecules are formed)

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

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

So the change in energy for the second reaction is,

ΔΗ=(10709-11786) kJ = -1077 kJ_ (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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Answer 4

Textbook Question

Chapter 3, Problem 152CP

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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 1

b. Chapter 3, Problem 152CP, 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 3, Problem 152CP, Three processes that have been used for the industrial manufacture of acrylonitrile (CH2CHCN), an , example 3

(a)

Expert Solution

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 152CP

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

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , 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: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 2

Figure 2

For first reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

2 C−O = 358 kJ1 mol×2 mol=716 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For HC≡N,

1 C≡N = 891 kJ1 mol×1 mol=891 kJ

1 C−H = 413 kJ1 mol×1 mol=413 kJ

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

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

Product bonds,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

So the change in energy for the first reaction is,

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

In the second reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 3

Figure 3

For the reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

For product,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

Hence,

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

For water,

2 O−H = 2 mol×467 kJ/mol = 934 kJ

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

So the change in energy for the second reaction is,

ΔΗ=(4062-4025) kJ = 37 kJ_ (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

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 152CP

The required energy change is -850 kJ_.

Explanation of Solution

Given

The given reaction is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 4

Figure 4

For the reactant side,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For NO,

6 NO = (6×630) kJ = 3780 kJ (2)

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

For products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

For N2,

1 N−N = 418 kJ1 mol×1 mol=418 kJ (6)

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

So the change in energy for the second reaction is,

ΔΗ=(17536-18386) kJ = -850 kJ_ (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

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 152CP

The required energy change is -1077 kJ_.

Explanation of Solution

Given

For the given reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

(since 2 molecules are formed)

For NH3,

3 N−H = 391 kJ1 mol×3 mol=1173 kJ

Total energy =2×1173 kJ=2346 kJ (2)

(since 2 molecules are formed)

For O2,

1 O=O = 495 kJ1 mol×1 mol=495 kJ (3)

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

Energy for products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

(since 2 molecules are formed)

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

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

So the change in energy for the second reaction is,

ΔΗ=(10709-11786) kJ = -1077 kJ_ (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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Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

(a)

Expert Solution

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 152CP

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

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , 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: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 2

Figure 2

For first reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

2 C−O = 358 kJ1 mol×2 mol=716 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For HC≡N,

1 C≡N = 891 kJ1 mol×1 mol=891 kJ

1 C−H = 413 kJ1 mol×1 mol=413 kJ

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

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

Product bonds,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

So the change in energy for the first reaction is,

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

In the second reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 3

Figure 3

For the reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

For product,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

Hence,

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

For water,

2 O−H = 2 mol×467 kJ/mol = 934 kJ

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

So the change in energy for the second reaction is,

ΔΗ=(4062-4025) kJ = 37 kJ_ (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

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 152CP

The required energy change is -850 kJ_.

Explanation of Solution

Given

The given reaction is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 4

Figure 4

For the reactant side,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For NO,

6 NO = (6×630) kJ = 3780 kJ (2)

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

For products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

For N2,

1 N−N = 418 kJ1 mol×1 mol=418 kJ (6)

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

So the change in energy for the second reaction is,

ΔΗ=(17536-18386) kJ = -850 kJ_ (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

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 152CP

The required energy change is -1077 kJ_.

Explanation of Solution

Given

For the given reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

(since 2 molecules are formed)

For NH3,

3 N−H = 391 kJ1 mol×3 mol=1173 kJ

Total energy =2×1173 kJ=2346 kJ (2)

(since 2 molecules are formed)

For O2,

1 O=O = 495 kJ1 mol×1 mol=495 kJ (3)

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

Energy for products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

(since 2 molecules are formed)

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

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

So the change in energy for the second reaction is,

ΔΗ=(10709-11786) kJ = -1077 kJ_ (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.

Answer 8

(a)

Expert Solution

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 152CP

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

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , 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: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 2

Figure 2

For first reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

2 C−O = 358 kJ1 mol×2 mol=716 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For HC≡N,

1 C≡N = 891 kJ1 mol×1 mol=891 kJ

1 C−H = 413 kJ1 mol×1 mol=413 kJ

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

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

Product bonds,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

So the change in energy for the first reaction is,

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

In the second reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 3

Figure 3

For the reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

For product,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

Hence,

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

For water,

2 O−H = 2 mol×467 kJ/mol = 934 kJ

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

So the change in energy for the second reaction is,

ΔΗ=(4062-4025) kJ = 37 kJ_ (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.

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

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 13

Answer to Problem 152CP

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

Answer 14

Explanation of Solution

Given

The chemical reaction involved is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , 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: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 2

Figure 2

For first reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

2 C−O = 358 kJ1 mol×2 mol=716 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For HC≡N,

1 C≡N = 891 kJ1 mol×1 mol=891 kJ

1 C−H = 413 kJ1 mol×1 mol=413 kJ

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

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

Product bonds,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

So the change in energy for the first reaction is,

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

In the second reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 3

Figure 3

For the reactant,

4 C−H = 413 kJ1 mol×4 mol=1652 kJ

1 C−O = 358 kJ1 mol×1 mol=358 kJ

2 C−C = 347 kJ1 mol×2 mol=694 kJ

1 C≡N = 891 kJ

1 O−H = 467 kJ

Hence,

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

For product,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

Hence,

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

For water,

2 O−H = 2 mol×467 kJ/mol = 934 kJ

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

So the change in energy for the second reaction is,

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

Answer 15

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.

Answer 16

(b)

Expert Solution

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 152CP

The required energy change is -850 kJ_.

Explanation of Solution

Given

The given reaction is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 4

Figure 4

For the reactant side,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For NO,

6 NO = (6×630) kJ = 3780 kJ (2)

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

For products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

For N2,

1 N−N = 418 kJ1 mol×1 mol=418 kJ (6)

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

So the change in energy for the second reaction is,

ΔΗ=(17536-18386) kJ = -850 kJ_ (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.

Answer 17

(b)

Expert Solution

Answer 18

(b)

Expert Solution

Answer 19

Expert Solution

Answer 20

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 21

Answer to Problem 152CP

The required energy change is -850 kJ_.

Answer 22

Explanation of Solution

Given

The given reaction is,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 4

Figure 4

For the reactant side,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

For NO,

6 NO = (6×630) kJ = 3780 kJ (2)

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

For products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

For N2,

1 N−N = 418 kJ1 mol×1 mol=418 kJ (6)

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

So the change in energy for the second reaction is,

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

Answer 23

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.

Answer 24

(c)

Expert Solution

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 152CP

The required energy change is -1077 kJ_.

Explanation of Solution

Given

For the given reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

(since 2 molecules are formed)

For NH3,

3 N−H = 391 kJ1 mol×3 mol=1173 kJ

Total energy =2×1173 kJ=2346 kJ (2)

(since 2 molecules are formed)

For O2,

1 O=O = 495 kJ1 mol×1 mol=495 kJ (3)

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

Energy for products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

(since 2 molecules are formed)

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

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

So the change in energy for the second reaction is,

ΔΗ=(10709-11786) kJ = -1077 kJ_ (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.

Answer 25

(c)

Expert Solution

Answer 26

(c)

Expert Solution

Answer 27

Expert Solution

Answer 28

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 29

Answer to Problem 152CP

The required energy change is -1077 kJ_.

Answer 30

Explanation of Solution

Given

For the given reaction,

Chemistry: An Atoms First Approach, Chapter 3, Problem 152CP , additional homework tip 5

Figure 5

Energy for reactants,

For H2C=CHCH3,

6 C−H = 413 kJ1 mol×6 mol=2478 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

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

(since 2 molecules are formed)

For NH3,

3 N−H = 391 kJ1 mol×3 mol=1173 kJ

Total energy =2×1173 kJ=2346 kJ (2)

(since 2 molecules are formed)

For O2,

1 O=O = 495 kJ1 mol×1 mol=495 kJ (3)

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

Energy for products,

For H2C=CHCN,

3 C−H = 413 kJ1 mol×3 mol=1239 kJ

1 C=C = 614 kJ1 mol×1 mol=614 kJ

1 C−C = 347 kJ1 mol×1 mol=347 kJ

1 C≡N = 891 kJ

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

(since 2 molecules are formed)

For H2O,

2 O−H = 467 kJ1 mol×2 mol=934 kJ

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

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

So the change in energy for the second reaction is,

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

Answer 31

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.