Calculate the heat energy released when 10.3 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for Mercury at 1 atm: Heat capacity: 28.0 J/(mol*K) Melting Point: 234.32 K Enthalpy of fusion: 2.29 kJ/mol 2. At 1 atm, how much energy is required to heat 55.0 g of H2O(s) at -10.0 °C to H2O(g) at 119.0 °C? 3. Two 20.0-g ice cubes at -16.0 °C are placed into 205 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts. Heat capacity of H2O (s): 37.7 J/(mol*K) Heat capacity of H2O (l): 75.3 J/(mol*K) Enthalpy of fusion H2O: 6.01 kJ/mol