A 0.100 mol sample of propane, a gas used in many homes in these days of load shedding, was placed in a bomb calorimeter with excess oxygen and ignited. The reaction was C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (l) The initial temperature was 25.000 0C and its total heat capacity was 97.1 kJ 0C –1 . The reaction raised the temperature of the calorimeter to 27.282 0C? A. How many joules were liberated by the combustion of the propane? B. What is the ΔE for the reaction expressed in kJ mol–1 C3H8? C. Calculate ΔH for the reaction in kJ mol–1 C3H8