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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 standard enthalpy of combustion of toluene is - 3910 kJ/mol. this is the value for the substance quoted in data tables which are nothing to do with this question. The /mol refer to toluene.This is the amount of heat you could expect to be released when 1 mole of toluene is burned in oxygen.t is nothing to do with the calorimeter. The heat released by the (1.55/92.134) mole of toluene will be 65.779 kJ. In your calculation 1.55g = 142.81g is incorrect-I think you have mistaken 1.55 as a number of moles and multiplied it by the mass of 1 mol (1.55 x 92.134 = 142.81g.