CHEMISTRY
posted by Jake on .
If 142.38 g of l water at 21.7 degrees C is placed into a syrofoam cup with 174.36 g of ice at 27.5 degrees C what would be the final temperature of the entire contents at equilibrium? If it is partially frozen, how many g of the ice has melted?
given values
cp water = 4.184 j/g degree c
cp ice = 2.114 j/g degree c
heat of fusion of ice is 335 J/g
so far, i have this:
(174.36g)(2.114g)(27.5 C)
= 10247 g to three sig figs = 10200 J
is that i calculate the energy required to raise the ice to 0 degrees C?
now i know that the next steps are to find the enrgy required to melt the ice and the energy reuired to cool the water down to 0 degrees C. how do i do those two calculations?

Yes. Now, you have ice at 0C. How much did the 142 g of water cool to supply this heat?