1. The problem statement, all variables and given/known data - 82 grams of ice is added to 0.15 liters of water at 35 degrees C. If the solution is allowed to cool to 0 degrees C, how much ice remain? (Heat of fusion of ice is 333 J/g) - Many cigarette lighters contain liquid butane, C4H10 for which ΔH(formation) = -127 kJ/mol. Calculate the heat of combustion of this reaction, and then how much energy is produced when 1.00 grams of liquid butane is burned. The products of the combustion are CO2 and water vapor. - Using the following data: Ca + 2C = CaC2 H°=-62.8 kJ Ca + 1/2O2 = CaO H°= -635.5 kJ CaO + H2O = Ca(OH)2 H°= -653.1 kJ C2H2 + 5/2O2 = 2CO2 + H2O H°= -1300 kJ C + O2 = CO2 H°= -393.5 kJ Calculate the change in enthalpy for the following equation CaC2 + 2H2O = Ca(OH)2 + C2H2 2. Relevant equations mc=ΔT q=mcΔT 3. The attempt at a solution I know that for the Hess Law problem, I need to cancel out unimportant elements and compounds, but I'm completely lost with the other two problems.