1. The problem statement, all variables and given/known data A 10 kg block of ice has a temperature of -8°C. The pressure is one atmosphere. The block absorbs 4.17 x10^6 J of heat. What is the final temperature of the liquid water? Q=4.17x10^6J T_0=-8 Mass=10kg 4184= specific heat of water 2000=specific heat of ice 333.5=latent heat of fusion 2. Relevant equations Q=mc(deltaT) Q=mL 3. The attempt at a solution Q_1=mc(delta)T Q_1=(10kg)(2000)(8°C) Q_1=160,000J of energy was needed to raise the temperature to 0 degrees Celsius Q_2=mL Q_2=(10kg)(333.5) Q_2=3335J of energy needed to change ice to water. 160,000J+3335J=163,335J of energy used. 4,170,000J-163,335J= 4,006,665J of energy left 4,006,665J=mc(delta)T 4,006,665J=(10kg)(4184)(delta)T 4,006,665/(10*4184)=deltaT deltaT=95.761°C 95.761 degrees Celsius should be the final temperature according to my calculations. I'm fairly sure the process is right, my money is there is something wrong with a coefficient, but I can't figure it out.