1. The problem statement, all variables and given/known data An 18g ice cube at -4.0ºC is placed into 75g of water at 10 ºC in an insulated container. a. What is the final temperature of the system? b. How much of the ice melts? I have a sheet full of these & ice to water to steam I really need somone to explain how to find the results so I can get my brain around these 2. Relevant equations Q=MCΔT C ice =2.09j/g°c Cwater = 4.186j/g°c M=Mass in g T = temp in Degrees C Q=ML M=Mass in g Lice =334j/g 3. The attempt at a solution So heres what i think is right so far Raise the temp of ice to 0 18 x 2.09 x 4 = 150 joules Remove this energy from the water 150.48=75 x 4.186 x(10-Tf)is this part right? 150.48= 3139.5-313.95(Tf) I am not sure how to get to the resultant temp of the water propery before I consider a phase change in the ice but I have a feeling there wont be enough heat energy in the water to melt all of the ice.