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    Energy Released by a Reaction

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    I have been given the attached as a balanced chemical equation for the complete oxidation of one mole of oleic acid.

    2CH3(CH2)7CH = CH(CH2)7COOH + 51)2 = 36CO2 = 36CO2 + 34H20

    Using the following table how do I work out the energy released by the reaction?

    TYPE OF BOND
    AVERAGE ENERGY CONTENT/kJ mol-1

    Single carbon-to-carbon (C-C) 330
    Double carbon-to-carbon (C=C) 589
    Carbon-to-hydrogen (C-H) 416
    Single carbon-to-oxygen (C-O) 327
    Double carbon-to-oxygen (C=O) 804
    Double oxygen-to-oxygen (O=O) 498
    Oxygen-to-hydrogen (O-H) 463

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    https://brainmass.com/chemistry/bonding/energy-released-reaction-31657

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    Answer) Here is how it works.
    Calculate the bond formation energy of products:
    products: 36(O=C=O) + 34(H-O-H) = 36(2*804)+34(2*463) = 89372 kJ

    Now ...

    Solution Summary

    This solution demonstrates how to calculate the bond formation energy of products and the energy to break the bonds of the reactants.

    $2.49

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