# Trying to figure out heat of reaction

A question in Thermodynamics of Natural Systems by G. M. Anderson is to find the "standard heat of reaction" of this reaction: $$\ce{C8H16N2O3(aq) + H2O(l) -> C6H13NO2(aq) + C2H5NO2(aq)}$$

As far as I understand it, it should be a rather simple problem of finding $\Delta_\mathrm r H$. So it should be:

$\Delta_\mathrm r H=\Delta_\mathrm fH (\ce{C6}) + \Delta_\mathrm fH (\ce{C2}) - \Delta_\mathrm fH (\ce{C8}) - \Delta_\mathrm fH (\ce{H2O})$ (note that I shortened the organic formulae)

According to the data from the same textbook, it's: $(-632077~\pu{J/mol}-513988~\pu{J/mol})-(-847929~\pu{J/mol}-285830~\pu{J/mol})=-12306~\pu{J/mol}$

However, the answer given is $−89475~\pu{J/mol}$.

Am I missing something? Do I need to add some terms of pressure or volume expansion? Is this not the enthalpy that I'm looking for?

• Have you considered estimating the enthalpy change using bond energies? It's more approximate than using standard formation enthalpies, but might be useful to compare against your value and the textbook value. It would require knowing the structures for the organic molecules, however. Mar 9, 2015 at 14:31
• @NicolauSakerNeto this is a basic textbook for introductory thermodynamics. I'm certain that using bond energies is not required as it is not even covered in this book. I'm thinking that it may be an error either in the data provided or in the answer given... Mar 9, 2015 at 14:41
• It might not be required, but it's a way to check! Do you have the structures or the compound names? Mar 9, 2015 at 14:43
• Leucylglycine + water = leucine + glycine Mar 9, 2015 at 14:43
• Interesting, a calculation by bond energies assuming Dave has the right structures (Dave, are you a wizard?!) suggests the reaction enthalpy should be $-85\ kJ\ mol^{-1}$. Maybe there is a print error in the enthalpy data. Mar 9, 2015 at 14:59