In a well-insulated calorimeter, 1.0 kg of water at 20 C is mixed with 1.0 g (.001 kg) of ice at 0 C. What is the net change in entropy of the system by the moment the ice completely melts? The heat of fusion of ice is 3.34 x 10^5 J/kg. I must find the changes in entropy for the water and for the ice, then find the net change. Net change = /_\S1 + /_\S2 This is what I did so far: S_ice = (mL)/T, where Q = mL S_ice = [(3.34 x 10^5 J/kg)*.001 kg]/[273 K] = 1.223 J/K ??? How do I find the change in entropy for H2O?? Thanks.