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= 1211 kJ mol-1. Therefore the molar heat of combustion of ethanol is 1211 kJ mol-1 (The molar enthalpy of combustion of ethanol is 1211 kJ mol-1). (Note that the enthalpy change for the reaction is negative because the reaction is exothermic, so the enthalpy change for the reaction is -1211 kJ mol-1, ÎH = - 1211 kJ mol-1)
The idea here is that the standard molar enthalpy of combustion, Î´Hâcomb, tells you the enthalpy change associated with the combustion of one mole of a given substance under standard conditions. This tells you that every mole of methane that undergoes combustion under standard conditions gives off 890.8 kJ of heat. All you have to do here is use the molar mass of methane to see how many moles you have in that 50.00 g sample. 50.00gâ1 mole CH416.0425g=3.1167 moles CH4.