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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)
^H= -118kJ. DELTA. Calculate the heat when 100.0 L of .500 M HCl is mixed with 300.0 mL of .500 M Ba(OH02. Assuming that the temperature of both solutions was initially 25.0 C and that the final mixture has a mass of 400.0g and a specific heat capacity of 4.18 J/Cxg, calculate the final temperature of the mixture. 2 mole HCl react with 1 mole Ba(OH)2. Find moles of HCl and moles Ba(OH)2 based on volume in L x molarity and decide which is limiting based on the first statement. From the equation, you know that 118kJ are released per mole of Ba(OH)2 or per 2 mole of HCl. So use the limiting one to find the amount of heat that this would release.