An ice cube at 0.00 ∘C with a mass of 21.5 g is placed into 500.0 g of water, initially at 31.0 ∘C, in an insulated container. Part A Assuming that no heat is lost to the surroundings, what is the temperature of the entire water sample after all of the ice has melted?
Answers: 3
.......(1)
= mass of ice = 21.5 g
= mass of water = 500.0 g
= final temperature = ?
= temperature of water =
= specific heat of ice= 
= specific heat of water = 
![21.5\times 2.1\times (T_{final}-0)=-[500.0\times 4.184\times (T_{final}-31.0)]](/tpl/images/0513/4270/003f3.png)
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An ice cube at 0.00 ∘C with a mass of 21.5 g is placed into 500.0 g of water, initially at 31.0 ∘C,...
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