1. The problem statement, all variables and given/known data A 100g piece of ice at 0.0°C is dropped into 500g of water at 100°C. What is the final temperature of mixture. 2. Relevant equations Q=mL (latent heat) Q=mcΔt Qw=-Qx (energy absorbed by water is equal but opposite to that of substance inserted into water) specific heat ice: 2.09 * 10^3 J/kg * °C specific heat water: 4.186 * 10^3 J/kg * °C specific heat steam: 2.01 * 10^3 J/kg * °C latent heat of fusion: 3.33 * 10^5 J/kg latent heat of vaporization: 2.26 * 10^6 J/kg 3. The attempt at a solution Do you find the total heat including phase change heat for both substances, using final temperature as an unknown variable? If so: Q = mcΔt + mL Qw = (0.5 *4.186 * 10^3 *(Tf-100)) + 0.5 * 2.26 * 10^6 Qx= -((0.5 *4.186 * 10^3 *(Tf-0)) + (0.5 * 3.33 * 10^5)) I set both equal after simplifying, and obtained a final temperature of 264.14°C, which is too bizarre of an answer.