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In the method 2 example with CH2=Ch2, is the reason he doesn't include the bond enthalpy of the C-H bonds on the reactants side of the equation is because the products side has one more C-H bonds than the reactants side?
Will we be expected to know which bonds do not break when reactants react to form products? I wouldn't have known that the C-H bonds don't break unless someone were to tell me. Is it okay to assume that all bonds of reactants break?
I think that the reason only some of the C-H bonds were shown to break or form was based on the lewis structure. When he drew CH2=CH2, most of the C-H bonds remained in the "same" place, and so there was no need to show the bond breaking or forming. However, the = definitely broke as the product only had single bonds, which is why he calculated the double bond breaking but not other C-H bonds breaking.
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