Part A: A calorimeter contains 18.0 mL of water at 13.5∘C. When2.30 g of X (a substance with a molar mass of 69.0 g/mol) is added,it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperatureof the solution increases to 30.0∘C. Calculate the enthalpy change,ΔH, for this reaction per mole of X. Assume that the specific heatof the resulting solution is equal to that of water [4.18J/(g⋅∘C)], that density of water is 1.00 g/mL, and that no heat islost to the calorimeter itself, nor to the surroundings. Part B:the reaction C12H22O11(s)+12O2(g)→12CO2(g)+11H2O(l) in which 10.0 gof sucrose, C12H22O11, was burned in a bomb calorimeter with a heatcapacity of 7.50 kJ/∘C. The temperature increase inside thecalorimeter was found to be 22.0∘C. Calculate the change ininternal energy, ΔE, for this reaction per mole of sucrose.
