Enthalpies of reaction calculated from bond energies and from enthalpies of formation
Chapter 9, Problem 9.91(choose chapter or problem)
Enthalpies of reaction calculated from bond energies and from enthalpies of formation are often, but not always, close to each other. (a) Industrial ethanol (CH3CH2OH) is produced by a catalytic reaction of ethylene (CH2CH2) with water at high pressures and temperatures. Calculate DH 8 rxn for this gas-phase hydration of ethylene to ethanol, using bond energies and then using enthalpies of formation. (b) Ethylene glycol is produced by the catalytic oxidation of ethylene to ethylene oxide, which then reacts with water to form ethylene glycol: O CH (l) 2 CH2 H HOCH2CH2OH(l) + 2O(l) The DH8 rxn for this hydrolysis step, based on enthalpies of formation, is 297 kJ/mol. Calculate DH8 rxn for the hydrolysis using bond energies. (c) Why are the two values relatively close for the hydration in part (a) but not close for the hydrolysis in part (b)?
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