Organic Chemistry
Organic Chemistry
4th Edition
ISBN: 9780073402772
Author: Janice G. Smith
Publisher: MCG
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Chapter 6, Problem 6.32P
Interpretation Introduction

(a)

Interpretation: The value of ΔH° for the given reaction is to be calculated.

Concept introduction: The chemical reaction in which energy is released during the formation of products is known as exothermic reaction. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Expert Solution
Check Mark

Answer to Problem 6.32P

The value of ΔH° is 51kJ/mol.

Explanation of Solution

The chemical equation for the given reaction is,

H3CCH3+BrBrH3CCH2Br+HBr

The bond dissociation energy of CH2H, and BrBr bond is 410kJ/mol and 192kJ/mol and CH2Br is 285kJ/mol and HBr is 368kJ/mol respectively.

The overall enthalpy change in the chemical reaction is calculated by the formula,

ΔH°=SumofΔH°ofbondsbroken+SumofΔH°ofbondsformed

Substitute the values of ΔH°ofbondsbroken and ΔH°ofbondsformed in the above expression.

ΔH°=(410kJ/mol+192kJ/mol)+((285kJ/mol)+ (368 kJ/mol))=51kJ/mol

Therefore, the value of ΔH° is 51kJ/mol. The negative sign indicates that the given reaction is an exothermic reaction and the energy is released during the reaction.

Conclusion

The value of ΔH° is 51kJ/mol.

Interpretation Introduction

(b)

Interpretation: The value of ΔH° for the given reaction is to be calculated.

Concept introduction: The chemical reaction in which energy is released during the formation of products is known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Expert Solution
Check Mark

Answer to Problem 6.32P

The value of ΔH° is 63kJ/mol.

Explanation of Solution

The chemical equation for the given reaction is,

HO+CH4CH3+H2O

The bond dissociation energy of CH3H, and HOH bond is 435kJ/mol and 498kJ/mol respectively.

The overall enthalpy change in the chemical reaction is calculated by the formula,

ΔH°=SumofΔH°ofbondsbroken+SumofΔH°ofbondsformed

Substitute the values of ΔH°ofbondsbroken and ΔH°ofbondsformed in the above expression.

ΔH°=(435kJ/mol)+(498kJ/mol)=63kJ/mol

Therefore, the value of ΔH° is 63kJ/mol. The negative sign indicates that the given reaction is an exothermic reaction and the energy is released during the reaction.

Conclusion

The value of ΔH° is 63kJ/mol.

Interpretation Introduction

(c)

Interpretation: The value of ΔH° for the given reaction is to be calculated.

Concept introduction: The chemical reaction in which energy is released during the formation of products is known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Expert Solution
Check Mark

Answer to Problem 6.32P

The value of ΔH° is 34kJ/mol.

Explanation of Solution

The given reaction is,

CH3OH+HBrCH3Br+H2O

The bond dissociation energy of CH3OH, HBr, CH3Br and HOH is 389kJ/mol, 368kJ/mol, 293kJ/mol and 498kJ/mol respectively.

The bonds broken in the reactants are CH3OH and HBr, whereas the bonds formed in the products are CH3Br and HOH.

The overall enthalpy change in the chemical reaction is calculated by the formula,

ΔH°=SumofΔH°ofbondsbroken+SumofΔH°ofbondsformed

Substitute the values of ΔH°ofbondsbroken and ΔH°ofbondsformed in the above expression.

ΔH°=(389kJ/mol+368kJ/mol)+(293kJ/mol498kJ/mol)=757kJ/mol791kJ/mol=34kJ/mol

Therefore, the value of ΔH° is 34kJ/mol. The negative sign indicates that the given reaction is an exothermic reaction and the energy is release during the reaction.

Conclusion

The value of ΔH° is 34kJ/mol.

Interpretation Introduction

(d)

Interpretation: The value of ΔH° for the given reaction is to be calculated.

Concept introduction: The chemical reaction in which energy is released during the formation of products is known as exothermic reactions. The energy released during the reaction is denoted by ΔH°. Exothermic and endothermic reactions are opposite to each other. The value of ΔH° for exothermic and endothermic reactions is positive and negative respectively.

Expert Solution
Check Mark

Answer to Problem 6.32P

The value of ΔH° is +142kJ/mol.

Explanation of Solution

The given reaction is,

Br+CH4H+CH3Br

The bond dissociation energy of CH3H, and CH3Br bond is 435kJ/mol and 293kJ/mol respectively.

The overall enthalpy change in the chemical reaction is calculated by the formula,

ΔH°=SumofΔH°ofbondsbroken+SumofΔH°ofbondsformed

Substitute the values of ΔH°ofbondsbroken and ΔH°ofbondsformed in the above expression.

ΔH°=(435kJ/mol)+(293kJ/mol)=+142kJ/mol

Therefore, the value of ΔH° is +142kJ/mol. The positive sign indicates that the given reaction is an endothermic reaction and the energy is absorbed during the reaction.

Conclusion

The value of ΔH° is +142kJ/mol.

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Chapter 6 Solutions

Organic Chemistry

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