No. You find the heat of combustion which is in tables (or you can calculate it), then
q = dHcombustion x (23g/molar mass ethanol)
If you don't have heat combustion tables you can calculate it this way. From your equation above, use
dHfrxn = dH combustion = (n*dHf products) - (n*dHf reactants). The heats of formation are in tables, too, usually in the appendix. CO2 is approx -393.5 kJ/mol (but I don't remember all of these so you must look them up) and H2O is about -285 kJ/mol or so. I don't have the foggiest about ethanol.
Question as follows:
If you combusted 23g of ethanol with an excess of oxygen how much heat would be released or absorbed?
the only thing I've deduced is the chemical reaction:
C2H6O + 302 -> 3H20 + 2C02
I'm not sure how to proceed. I need Q. Not sure which equation to use since there is no temperature. Am I to assume 298K?
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