A 192 g piece of copper is heated to 100.0 deg C and then dropped into a coffee-cup calorimeter containing 750.0 mL of water at 4.0deg C. What is the final temperature (in degrees C) of the copper and water after they come to thermal equilibrium? (Assume that noheat is lost to the surroundings and that the density of water is1.00 g/mL. Also, the specific heat of water is 4.184 J/g-deg C, and the specific heat of copper is 0.385 J/g-deg C.)