Here is the question from my textbook:
"In an insulated vessel, 250g of ice at $0^{\circ}$C is added to 600g of water at $18^{\circ}$C. What is the final temperature of the system?"
The solution says that it takes more heat to melt ice than to cool water, so some ice will remain. It says the final temperature should be $0^{\circ}$C, but no equation is given to explain that conclusion. Can the final temperature of this system be determined by reasoning alone?
Best Answer
You need to consider the heat capcity of liquid water and the latent heat of fusion of water, and calculate whether the amount of heat removal needed to cool the water to 0 degrees is more or less than the amount of heat needed to melt the ice.