1. The problem statement, all variables and given/known data A 3.60 kg block of copper at a temperature of 92 °C is dropped into a bucket containing a mixture of ice and water whose total mass is 1.50 kg. When thermal equilibrium is reached the temperature of the water is 5 °C. How much ice was in the bucket before the copper block was placed in it? (ci = 2000 J/(kg.°C), cw = 4186 J/(kg.°C), Lf=3.35 × 105 J/kg, Lv=2.26 × 106 J/kg, ccopper = 387 J/(kg.°C). Neglect the heat capacity of the bucket.) 2. Relevant equations Q=mcΔT Q=mL 3. The attempt at a solution Because of conservation of heat, the energy the copper block loses must be gained by the ice/water system. So; QLOST= QGAINED Expanded it should become something like; (cmΔT)COPPER = (heat to raise temperature of ice) + (heat to raise temperature of water) + (latent heat to melt ice) + (latent heat to vaporize water) However I think there are too many unknowns at this point. Any idea on what a possible next step could be / look like, or if I'm even doing this remotely correctly? All help appreciated!!