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9 months ago
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.

▸ –210 kJ/mol

▸ –11,230 kJ/mol

▸ 22,040 kJ/mol

▸ –420 kJ/mol

▸ 420 kJ/mol
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Chemistry

Chemistry


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9 months ago
Thank you, thank you, thank you!
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You make an excellent tutor!
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this is exactly what I needed
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