Octane (C₈H₁₈) Undergoes Combustion According to the Following Thermochemical Equation $\rarr$

question 80

Multiple Choice

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

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