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On part (b) of problem 7.115, we are asked to use bond enthalpies to calculate the enthalpy of combustion of each fuel, assuming they burn to produce gaseous CO2 and gaseous H2O. For CH4, I know we have to find all of the enthalpies and add them together, but why do the products, CO2 and H20, have negative bond enthalpies? Is this because the bonds are formed?
It's the delta H of combustion divided by the number of moles of CO2 gas produced for each substance (which can be found by the balanced equation of combustion for each substance—methane, ethanol, and octane).
Ahh, because the answer for octane threw me off in the solutions manual. If the delta h of combustion for octane is -5471kj/mol and there are 2 mols of C02, shouldnt it be -2735.5 k/mol CO2 instead of -684kj/mol?
is the combustion reaction for octane, but since enthalpies are per mole, the reaction for which enthalpy is calculated is: . So there's 8 CO2 produced and you would divide the enthalpy of combustion by 8 to get -684 kJ/mol CO2 produced.
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