1. Magnesium solid reacts with aqueous hydrochloric acid to form the Mg2+ ion in solution. In an experiment, 60.0 mL of aqueous HCI was mixed with 0.1297 g of magnesium solid in a double Styrofoam cup calorimeter. The reaction caused the temperature of the substances in the calorimeter to rise 10.02°C. Assume the density and specific heat of the HCl solution is that of water, 1.00 g/mL and 4.184 J/g °C, respectively. The specific heat of magnesium is 1.02 J/g °C. a. Write the balanced chemical equation for this reaction. b. Calculate the heat of this reaction, AHpx, in kJ. c. Calculate the heat of this reaction per mole of Mg2+ formed, AHx/mole Mg d. The literature value of this reaction is 466.85 kJ/mole. Calculate the percent deviation of the experimental value from the literature value. 2. A 45.5 kg copper rod (s = 0.385 J/g °C) is heated to 475.0°C and then quenched into a well-insulated water bath containing 1000.0 kg of water at 25.0°C. What is the final temperature of the mixture?