A calorimeter contains 22.0mL of water at 12.0 Celcius. When 2.30g of (a substance with a molar mass of 56.0 g/mol ) is added, it dissolves via the reaction X(s)+H_2O(l) --> X (aq) and the temperature of the solution increases to 25.5 Celcius.
Calculate the enthalpy change (in kJ/mol),delata h , for this reaction per mole of X .
Assume that the specific heat and density of the resulting solution are equal to those of water [4.18 J/(g \degrees Celsius}) and 1.00 g/mL] and that no heat is lost to the calorimeter itself, nor to the surroundings.