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

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The Answer of 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

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

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