Chapter 13, Problem 58E

Interpretation Introduction

Interpretation: The value of $\Delta \text{H}$ for the given reaction needs to be determined with the help of bond energy value and compare it with $\Delta \text{H}$ using standard enthalpies of formation as well.

  ${\text{CH}}_{\text{3}}{\text{OH}}_{\text{(g)}}\text{+ C}\equiv {\text{O}}_{\text{(g)}}\stackrel{}{\to }{\text{CH}}_{\text{3}}{\text{COOH}}_{\text{(l)}}$

Concept Introduction:

A chemical compound can be formed by either ionic bond or covalent bond between bonded atoms. The ionic compound is formed by opposite charge ions; cations and anions. The covalent compound is formed by sharing of electrons between bonded atoms.

The bond energy of a chemical bond can be defined as the energy required to break that chemical bond. The bond energy that is needed to break the bonds in reactant molecule and the energy released to form chemical bonds in product can be used to calculate the $\Delta \text{H}$ of the chemical reaction.

  $\Delta \text{H=}\sum {\text{BE}}_{\text{reactant }}\text{- }\sum {\text{BE}}_{\text{product }}$

  $\Delta \text{H}$ of reaction can also be calculated with the help of standard heat of formation of reactant and product.

  $\Delta \text{H =}\sum \Delta {\text{H}}_{\text{product }}\text{- }\sum \Delta {\text{H}}_{\text{reactant }}$