hi everybody: my problem says the following: A copper calorimeter can with mass 0.100 kg contains 0.160 kg of water and 0.018 kg of ice in thermal equilibrium at atmospheric pressure. If 0.750 kg of lead at a temperature of 255 degree celcius is dropped into the calorimeter can, what is the final temperature? Assume that no heat is lost to the surroundings. when they say that the can , the water and the ice are in thermal equilibrium at atmospheric pressure, what would be their temperatures?? I am not sure how to set up the equations. should i use Qwater+Qice+Qlead+...= 0 where the Q=m*c*delta T and solve for T. Delta T should be T-255???? , what T do i use for what was in the can before adding the lead? thanks.