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