Heats of reaction calculated from bond energies and from heats of formation are often
Chapter 9, Problem 9.93(choose chapter or problem)
Heats of reaction calculated from bond energies and from heats of formation are often, but not always, close to each other. (a) Industrial ethanol (CH3CH2OH) is produced by a catalytic reaction of ethylene (CH2NCH2) with water at high pressures and temperatures. Calculate _H_rxn for this gas-phase hydration of ethylene to ethanol, using bond energies and then using heats 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: The _H_rxn for this hydrolysis step, based on heats of formation, is _97 kJ/mol. Calculate _H_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)?
Unfortunately, we don't have that question answered yet. But you can get it answered in just 5 hours by Logging in or Becoming a subscriber.
Becoming a subscriber
Or look for another answer