1. The problem statement, all variables and given/known data Several small piece of aluminum, having total (combined) mass of 2.5 kg are placed in liquid nitrogen and, when removed, are at a temperature of -135C. The aluminum is transferred to an insulating container with 0.50 kg of water. The water is at 25.0C [ Ignore heat lost from the system] C Al = 910 J/kg K C water = 4190 J/kg K ; Lf = 334000 J/kg ; Freezing pt = 0C C ice = 2100 J/ kg K 2. Relevant equations Q = mc(change)T Lf = mLf Conservation of Energy ( because system is isolated ) Qcold = -Qhot 3. The attempt at a solution Before I attempted to do this problem, I wasnt sure if there would be a latent phase change for the water to ice because if there was then I would include that eq. Lf = mLf into my solution. Gained Energy = Aluminum from water Lose Energy = Water from Aluminum (2.5 kg)(910 J/kg K)(T - (-135C)) = - (0.5 kg)(4190 J/kg K)( T - 25C) 2275(T + 135C) + 2095 (T - 25C) = 0 ??? I am unsure if thats what your suppose to do and is it suppose to be +135C?