Chapter 9, Problem 9.11P

Interpretation Introduction

Interpretation:

The balanced equation for the combustion of gaseous methanol ${\text{CH}}_{\text{3}}\text{OH}$ is to be written and the enthalpy of combustion of methanol using bond enthalpies is to be calculated.

Concept introduction: Bond energy or bond enthalpy is the amount of energy required to break one mole of bonds. Breaking of bonds is an endothermic reaction because energy is always absorbed in the process and its value is always positive. Formation of bonds is an exothermic reaction because energy is always released in the process and its value is always negative.

The enthalpy change for a reaction is calculated by the formula,

$\text{Δ}{H}_{\text{rxn}}={\displaystyle \sum \left(\text{Δ}{H}_{\text{bonds}\text{broken}}\right)}+{\displaystyle \sum \left(\text{Δ}{H}_{\text{bonds}\text{formed}}\right)}$

To determine: The balanced equation for the combustion of gaseous methanol ${\text{CH}}_{\text{3}}\text{OH}$ and the enthalpy of combustion of methanol using bond enthalpies.