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The sign of the heat of formation matters. Using hess's law: 2(-238kJ) + 4(242kJ) + 2(393)= -1279=Heat of reaction Heat of combustion of methanol is just the heat of reaction divided by the molar coefficient for methanol in the chemical equation so about -639.5kJ/mol. In acuality it is somewhere near -727kJ/mol.
Describe how you could use the information in the graph you sketched for Q 11 to separate a mixture of methanol and ethanol. (Look on page at #11) By heating the mixture while measuring the temperature one could collect the vapor at 65ÂºC which would be near pure methanol. As soon as the temperature begins to heat again essentially pure ethanol is left in the container.