I need help with this lab

How much heal was lost by lhe warm waler? Show your work. Qh= J How much heal was gained by the cool water? Again, show your work Q = J How does the but lost compare with the heat gained? Does this make sense in terms of the law ofconservation ofencrgy? This is an example of the First Law of' Thermodynamics, which is the law ofeonservation of energy including heat and internal energy. We XVI\" new use the First law of Thermodynamics to nd the specic heat capacity of a metal. CliCR reset and choose a solid and choose Copper. Set the mass to 50 g and the temperature to 100\"C. Record them below where the m Indicates metal. Measure and record the mass of the metal sample. mm = g Cwmcr = JIgC Click the \"Next" button. You must do this for the simulation to let you move on! Check the boxes \"Show graph View\" and \"show macroscopic View\" and then press start. Sketch the temperature graph and descnbe what happens in the macroscopic view. When the simulation has nished, record the nal temperature of the water in the cup with the metal. 0 Tr: __ C Calculate the heat gained by the cool water. Show your work. How did the water heat up? What must be the heat lost by the metal? (you should NOT use the specic heat of the metal here!) Use the heat equation to solve for the specic heat capacity of the metal. Show your work, c... : J/gC How close did you come to the specic heat of copper