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?

The temperature of the entire water sample after all of the ice has melted is  

Explanation:

As we know that,  

.......(1)

where,

q = heat absorbed or released

= 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 =

Now put all the given values in equation (1), we get

Thus the temperature of the entire water sample after all of the ice has melted is  

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