When cyclohexane (C6H12) is burned in excess oxygen to produce carbon dioxide gas and liquid water, it releases 3919kJ of heat per mole of cyclohexane burned. A) Write the balanced chemical equation that corresponds to this reaction. B) If 15g cyclohexane is burned in a calorimeter with a heat capacity of 230kJ/K, what temperature change do you expect (assuming that all the heat is deposited in the calorimeter)? C) How much heat is associated with the production of 5.5g water? D) What is the (Delta H(f)) of cyclohexane, given that the (delta H(f)) of H20(g) is -242 kJ, the (delta H(f)) of CO2(g) is -393.5kJ, the reaction CO2(s)=CO2(g) has a (delta H) of 25.2kJ and the reaction H20(l)=H20(g) has a (delta H) of 44kJ.