blazinfury Posted March 9, 2013 Share Posted March 9, 2013 So bond energy is the same bond enthalpy, which means the amount of energy needed to break the bond. Based on this definition, you would need to put in more energy to break the bonds of cyclohexane than cyclopropane due to the increased stability of cyclohexane, correct? From a combustion rxn, which would yield more energy: cyclopropane or cyclohexane? I would think cyclopropane due to the high ring strain within the molecule. Link to comment Share on other sites More sharing options...
Enthalpy Posted March 12, 2013 Share Posted March 12, 2013 Yes and yes. 1 Link to comment Share on other sites More sharing options...
CaptainPanic Posted March 12, 2013 Share Posted March 12, 2013 Yes and yes seems a good reply Here's a link to (Google books) a table that has the actual heat of combustion per CH2 of cyclopropane, cyclohexane, as well as a few more rings. Link to comment Share on other sites More sharing options...
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