Jokodo
Veteran Member
I guess my original confusion stemmed mostly from the fact that I would never have guessed that CO2 is almost half of the mass. I guess I could have ballparked it, as in "both have three medium sized (C/N/O range) nuclei, one of them has extra hydrogen but we can ignore hydrogen in a first approximation", but it didn't even come to me that this volatile gas could be anywhere near as massive as that complex organic molecule.Yes, it is. But a little is infinitely better than nothing, and when you have no source of additional oxygen, you have to make do with what you've got.So here is my dumb question:
According to everything I find on the webs, the caloric value of sugar is roughly 400 kcal/ 100g, while for alcohol (ethanol) I find 700kcal/100g.
What's confusing me is that ethanol is the product of fermenting sugars in what I must assume is an exothermic reaction. I mean, it's what yeasts live of, right? I'm aware that this reaction produces carbon dioxide as a side product, but I still can't seem to get the math to work. 1 mol of glucose (180g) produces 2 mol of carbon dioxide (44g each) and 2 mol of ethanol (46g each), so the resulting 82 grams of ethanol must have very nearly the same caloric value as the original glucose (692 for 100g of ethanol vs 757 for the sugar required to obtain those 100g if I plug in concrete figures I find). Is alcoholic fermentation really that marginally exothermic?
That's why yeast goes with aerobic respiration rather than anaerobic fermentation, if you don't restrict its access to oxygen.
Without that information, the math *really* didn't work. With it, it kind of does. 757>692 after all, though the margin still felt smaller than what I would have expected.