Octane (C₈H₁₈)undergoes Combustion According to the Following Thermochemical Equation: 2C₈H₁₈(l) $\rarr$

Multiple Choice

Octane (C₈H₁₈) undergoes combustion according to the following thermochemical equation: 2C₈H₁₈(l) + 25O₂(g) $\rarr$ 16CO₂(g) + 18H₂O(l)
$\Delta$ H°_rxn = -11,020 kJ/mol.
Given that $\Delta$ H°_f[CO₂(g) ] = -393.5 kJ/mol and $\Delta$ H°_f[H₂O(l) ] = -285.8 kJ/mol, calculate the standard enthalpy of formation of octane.

A) -210 kJ/mol
B) -11,230 kJ/mol
C) 22,040 kJ/mol
D) -420 kJ/mol
E) 420 kJ/mol