Chapter 13, Problem 57E

Interpretation Introduction

Interpretation: The requirement of elevated temperature for the given reactions to change in endothermic reactions needs to be explained. ${\text{4CH}}_{\text{2}}{\text{=CH-CH}}_{\text{3}}\text{ + 6 NO }\stackrel{\text{Ag/700°C}}{\to }{\text{4CH}}_{\text{2}}{\text{=CH-CN + 6 H}}_{\text{2}}{\text{O +N}}_{\text{2}}\Delta \text{H= -4256 kJ/mol }$

  ${\text{4CH}}_{\text{2}}{\text{=CH-CH}}_{\text{3}}{\text{ + 2 NH}}_{\text{3 }}{\text{+ 3 O}}_{\text{2}}\stackrel{\text{Catalyst/425-510°C}}{\to }{\text{4CH}}_{\text{2}}{\text{=CH-CN + 6 H}}_{\text{2}}\text{O }\Delta \text{H= -8567 kJ/mol }$

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.

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