1. The problem statement, all variables and given/known data An ice cube of volume 12.1 cm3 is initially at a temperature of -18.1°C. How much heat is required to convert this ice cube into steam? (the final answer must be in Joules) 2. Relevant equations Q = m*c*deltaT Q = m*Lf (latent heat of fusion) Q = m*Lv (latent heat of vaporization) density = m/v 3. The attempt at a solution Since I was only given the volume of the ice cube, I decided to use density = mass/volume to find the mass of the ice cube. Since the final answer must be in joules, I used the density of 9.17 kg/cm^3 as the density, and found the mass to be 1109570. I then plugged in that mass into Q = (1109570) (2090 J/kg°C the c of ice) (18.1) to convert ice to water Q = (1109570) (4180 J/kg°C the c of water) (100) to convert water to steam Q = (1109570) (334000 J - the Lf of water) Q = (1109570) (2200000 J - Lv of water) I added all the Qs together and found the final answer to be 5.09e14, which is incorrect. Finding the correct units was a bit tricky so I may have done something wrong there. If anyone has any suggestions, please let me know.