[winnie07]

Ok so I have this problem, I already figured out 2/3 but I don't know how to find the last part.

What amount of energy is required to melt a 11.5 g piece of ice at 0^oC?
The heat of fusion of ice = 333 Jg-1

Heat required to melt the ice = 3829 J

What amount of energy must be removed from 112 g of water to cool it from 74.5^oC to 5.36^oC?
Specific heat of water = 4.184 JK-1g-1

Enter the heat as a negative amount (heat removed from a system is by convention always negative).
Heat removed to cool the water = -32399 J

What is the final temperature after a 11.5 g piece of ice is placed into a styrofoam cup containing 112 g of hot water at 74.5oC. The mass of the ice, and the mass and initial temperature of the hot water are the same as in the two previous parts of this question.

Final temperature = ? (^oC)

[Borek]

Heat lost = heat gained, both are a function of the final temperature. Assume final temperature is your unknown, express a heat balance in terms of this unknown, solve.