The enthalpy of formation is the standard way of computing, because there are fewer of them. Combustion is one reaction among many, tables won't give all the reactions, but from the enthalpies of formation of the reactants and products you deduce the reaction, here a combustion.
For instance the handbook of chemistry and physics has a tables of the heats of formation. Search also for Janaf, Argonne... Whatever the table, double and triple-check that all compounds are in the desired state, generally they aren't. And beware that most tables are just meaningless values estimated by software (inaccurate and for a gas at zero kelvin), totally insufficient for thermochemistry.
Beware two heats of combustion exist, depending on whether the produced water is liquid or gaseous. You must check each and every time.
Note also that the position of the hydroxyl has the same influence of the heats of formation and combustion (possibly with a sign), because isomers follow the same combustion reaction. That is, if an isomer has 1 J more heat of formation, the combustion produces 1 J more too.