   Chapter 8.9, Problem 8.15CYU

Chapter
Section
Textbook Problem

Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.

Interpretation Introduction

Interpretation: The enthalpy of combustion of gaseous methane,(CH4) that forms water vapor and carbon dioxide gas should be estimated.

Concept Introduction:

Bond dissociation enthalpy:

Bond energy or more correctly the bond dissociation enthalpy is the enthalpy change when breaking a bond in a molecule with the reactant and products in the gas phase.

The process of breaking bonds in a molecule is always endothermic, so ΔIH for bond breaking is always positive.

Explanation

Consider the combustion of one mole of methane gas.

CH4(gas)+2O2(gas)CO2(gas)+2H2O

From table 8.8, Bond dissociation enthalpy for C-His413kJ/molO=Ois498kJ/mol C=Ois803kJ/mol and H-Ois463kJ/mol

Examining the reaction shows that there are 4C-H,2O=O,2C=Oand4H-O

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