Determine the enthalpy of the products of ideal combustion, i. e., no dissociation, resulting from the combustion of an isooctane-air mixture

The combustion of isooctane (C₈H₁₈) is written below:

2 C₈H₁₈ (l) + 25 O₂ (g) → 16 CO₂ (g) + 18 H₂O (l)

The formula for heat of combustion is:

ΔHc = (∑Stoichiometric coefficient*ΔHf of products) - (∑Stoichiometric coefficient*ΔHf of reactants), where ΔHf is heat of formation.

ΔHf of isooctane = - 259.2 kJ/mol

ΔHf of O₂ = 0 kJ/mol

ΔHf of CO₂ = - 393.5 kJ/mol

ΔHf of H₂O = - 285.8 kJ/mol

ΔHc = [ (16 mol*-393.5 kJ/mol) + (18 mol*-285.8 kJ/mol) ] - [ (2 mol*-259.2 kJ/mol) + (25 mol*0 kJ/mol) ]

ΔHc = - 10,922 kJ