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I got an exercise and I have to calculate de reaction enthalpy for
acetylsalicylic acid formation considering the reaction between salicylic acid and acetic anhydride in presence of an acid.
In the exercise I have a table with values in kJ/mol. I don't know if I'm doing something wrong but I calculated ΔH and it is equal to zero. In another question they say that the experimental ΔH is equal to -5,2 kJ/mol, asking for an explanation for the diference between calculated ΔH and experimental one.
Am I calculating ΔH correctly? And, how this difference could be explained?
If you show your work it would be helpful. Where are you getting the delta H values. What exactly does the table say? Bond dissociation enthalpies? Heats of formation?
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