1. The problem statement, all variables and given/known data I did an experiment where crushed ice was added to a known volume of warm water and stirred until all the ice melted. My initial water temperature was 40.2°C and the final water temperature was 3.1°C. The known volume of water is 150 mL = 150 g and the melted ice was found to be 93 mL = 85.3 g. The question is: What would be the final temperature if the ice was initially at -10°C when it was added to the water? 2. Relevant equations Q = mLf where Lf = heat of fusion = 3.33 * 10^5 J/kg C (water) = 4186 J/kg C C(ice) = 2100 J/kg C 3. The attempt at a solution This is what I have: (heat to raise 85.3 g of ice from -10 to 0°C) + (heat to change 85.3 g of ice to water) + (heat to raise 85.3 g of water (melted ice) from 0°C to final temperature) = (heat lost by the 150 g of water from 40.2°C to final temperature) [m(ice) * c(ice) * (0 - (-10))] + [m(ice) * Lf] + [m(ice)* c(water) * (T - 0)] = [m(water) * c(water) * (40.2 - T)] T = - 5.03 °C Is that right?