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Octane (C 8H 18) undergoes combustion according to the following thermochemical equation: 2C 8H 18 (l) + 25O 2 (g) --> 16CO2 (g) + 18H2O (l) ∆Hrxn = -11020 kJ Given that: ∆H o fCO 2 (g) = -393.5 kJ/mol and ∆H o fH 2O (l) = -285.8 kJ/mol Calculate the enthalpy of formation of 1 mole of octane.

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Answer:

-210.2 kJ/mol

Explanation:

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