This is CALORIMETRY PROBLEM. A 0.050kg metal bolt is heated to an unknown initial temperature. It is then dropped into a beaker containing 0.15kg of water with an initial temperature of 21.0 C. The bolt and metal then reach a final temperature of 25.0 C. If the metal has a specific heat capacity of 899 J/kg*C, find the initial temperature of the metal. the solution is: Change in Temp of metal = (C of water *mass of water* Change in temp of water)/(C of metal*mass of metal) Change of temp. of metal = [(4186 J/kg*C)(0.15kg)(25C-21C)]/[(899 j/kg*C)(0.050kg) Change of temp. of metal = 55.87C Change in temperature = Final Temperature-Initial Temperature Initial Temperature = Final Temp.-Change in Temp =25C-55.87C = -30.87C i want to ask why is the answer +80.87C from the book, instead of -30.87C? i hope you could explain so i can also explain it to my students. is the sign of the answer has something to do with the HEAT REMOVAL and HEAT ABSORPTION? Thanks!