Use the data in Table 5.1 (page 139) in the textbook to calculate an approximate ΔH∘ in kilojoules for the industrial synthesis of ethyl alcohol from ethylene: C2H4(g)+H2O(g)→C2H5OH(g).
The table it refers to is a list of Average Bond Dissociation Energies.

Question

Use the data in Table 5.1 (page 139) in the textbook to calculate an approximate ΔH∘ in kilojoules for the industrial synthesis of ethyl alcohol from ethylene: C2H4(g)+H2O(g)→C2H5OH(g). 
The table it refers to is a list of Average Bond Dissociation Energies.

zpupster · Answer

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zpupster · Answer

on the left i get one C-C bond and a O-H broken  bonds  350 and 460 respectively.

on the right i see one C-H bond formed and also a C-O 410 and  350

bonds broken - bonds formed = bond dissociation energy