Calcium chloride is mixed into concrete when it is cold to keep the concrete mixture warm for a longer period of time. Suppose the heat of dissolution (i.e., heat of dissolving) for CaCl2 (s) was determined via constant pressure calorimetry. If a sample of CaCl2 (s) with a mass of 23.6 g was placed in a calorimeter that contained water at an inital temperature of 23°C, what would be the heat of reaction in kJ/mol after all of the solid calcium chloride dissolves if the temperature increased to 38.7°C? Assume the heat capacity of the calorimeter and its contents was 1258 J/°C.​