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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 Δ H°f[CO2(g)] = –393.5 kJ/mol and ΔH°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
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 Δ H°f[CO2(g)] = –393.5 kJ/mol and ΔH°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
(A) –210 kJ/mol