Oh okay, just to understand how having a C=C double bond affects combustion: so if the carbon double bond is stronger, its harder to break and so less likely to be fully oxidised and therefore more likely to undergo incomplete combustion? Is that train of thought correct?
Also,
I was thinking about this last night, and I was wondering if this was correct: Assuming that the alkene is left to burn on its own, without any other heat input from other sources but itself(not being continuously heat up by a bunsen burner for example):
because less water is formed, less heat energy is produced overall by the alkene(formation of bonds releases energy), and so the carbons connected by a double bond are overall less likely to undergo complete combustion (because its less likely to break the double bond both because it is strong, and because there is not enough activation energy for the carbon=carbon double bond to break because less heat energy is produced from less water being produced). Is this right as well?
Wait... But when the hydrogens are oxidised, and they leave the alkene molecule as H20, shouldn't that completely destabilise the molecule and make it much easier to oxidise the structure that was the alkene so that the carbon should easily react with oxygen now? If H20 is gone, then you should have some carbon cation intermediates right because the oxygen took the Hs away, then the resulting structure should be very easy to oxidise right?
Hahahaha thanks for answering and you sort of made me understand it more, but i still don't understand it fully, if you have some ideas/answers, please share?