Chapter 4, Problem 53QRT

Isooctane (2,2,4-trimethylpentane), one of the many hydro carbons that make up gasoline, burns in air to give water and carbon dioxide.

$\begin{array}{l}2{\text{C}}_8{\text{H}}_{18}(\mathcal{l})+25{\text{O}}_2(\text{g})\stackrel{}{\to }16{\text{CO}}_2(\text{g})+18{\text{H}}_2\text{O}(\mathcal{l})\\ {\Delta }_{\text{r}}H°=-10,922\text{kJ/mol}\end{array}$

Calculate the enthalpy change if you burn 1.00 L isooctane (density = 0.69 g/mL).