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Problem- A 53.7 g ice cube at -19 C is dropped into an insulated cup containing 125.0 ml of hot water at 78 C. The specific heat of ice is 2.12 J/g deg. assuming no heat is able to pass through the insulated cup

a) How much energy would be needed to warm the ice to 0 C and then melt it?

b) How much energy would be needed to cool the 78 C water down to 0 C and

c) What will be the final temperature of the water and how much (if any) ice will be left?

I just need a general explanation of it please- Thanks!

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Category:- Chemistry
Reference No.:- M91245915

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