Chapter 9, Problem 9.144QP

Interpretation Introduction

Interpretation:

Bond enthalpy of $C-C,C-NandO-O$ bonds in $C_2{H}_6,N_2{H}_4$ and $H_2{O}_2$ respectively has to be calculated.  The effect caused by the lone pairs on adjacent atoms on strength of bonds has to be outlined.

Concept Introduction:

$\Delta H°$ refers to change in enthalpy.  Change in enthalpy in a reaction and bond energy (BE) are related as,

$\text{ΔH°}\text{=}\text{ΣBE(reactants)-ΣBE(products)}$

Hess’s law is applied to calculate the enthalpy changes in a reaction.  According to Hess’s law – “The overall enthalpy change of a reaction is equal to the sum of the enthalpy changes involving in each and every individual steps in the reaction.”  Thus if a reaction involves ‘n’ steps then enthalpy change $\Delta H°$ of the reaction is,

$\Delta H°=\Delta {\text{H}}_1^{°}+\Delta {\text{H}}_2^{°}+\Delta {\text{H}}_3^{°}\mathrm{....}+\Delta {\text{H}}_n^{°}$