A calorimeter contains 35.0 mL of water at 14.5 °C. When 1.80 g of X (a substance with a molar mass of 62.0 g/mol) is added, it dissolves via the reaction X(s) + H2O(l) → X(aq) and the temperature of the solution increases to 28.5 °C.
Calculate the enthalpy change, ΔH, for this reaction per mole of X.
Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅°C)], that the density of water is 1.00 g/mL, and that no heat is lost to the calorimeter itself, nor to the surroundings.