1. The problem statement, all variables and given/known data Calculate the heat absorbed by the water in the calorimeter and the heat released by 1,0g of burning ethanol. Then, calculate the molar heat of combustion (kJ/mol) of the ethanol. The calorimeter used was very makeshift: ethanol in an alcohol burner was lit under a can containing water, both of which were placed inside a hollowed out larger can. Here is what is known: mass of ethanol burned = 20g mass of heated water = 280g change in temperature = 30"degrees"C 2. Relevant equations Q(water) = -Q(ethanol) mc"delta"T = - (mc"delta"T) 280g*4.184J/g"degree"C*30 = -Q(ethanol) 3. The attempt at a solution Q(water) = mc"delta"T = 280g*4.184J/g"degree"C*30"degrees"C = 35145.6J = 35.1kJ Q(ethanol) = -Q(water) = -35.1kJ (for 20g) Q(per gram of ethanol) = -35.1kJ / 20g = -1.755kJ/g = -1.76kJ/g Q or "delta"H? (per mol of ethanol) = -1.76kJ/g * 46.07g/mol = 81.08kJ/mol --> Does this make sense? Is it right? And what is the difference between Q and "delta"H?