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Potassium nitrate, KNO3, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 49.8 g of KNO3 is dissolved in 305 g of water at 23.00 °C. KNO3(s)→H2O→K+(aq)+NO3−(aq) The temperature of the resulting solution decreases to 19.90 °C. Assume that the resulting solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. a) How much heat was released by the solution? (kJ) b)What is the enthalpy of the reaction? (kJ/mol)