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23 April, 20:55

A 10.0 g ice cube is placed into 250 g of water with an initial temperature of 20.0 C. If the water drops to a temperature of 16.8 C, has a specific heat of 4.18 J/g*K, what is the enthalpy of fusion of the ice. Ignore the fact that the ice, once melted, has to be heated again.

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  1. 23 April, 21:35
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    the mass of ice taken = 10 g

    the mass of water = 250 g

    initial temperature of water = 20 C

    the final temperature of water = 16. 8 C

    specific heat of water = 4.18 J/g*K

    the heat absorbed by ice to melt = heat loss by water

    heat loss by water = mass X specific heat of water X change in temperature

    heat loss by water = 250 X 4.18 X (20-16.8) = 3344 Joules

    heat gained by ice = 3344 J

    heat gained by ice = enthalpy of fusion X moles of ice

    moles of ice = mass / molar mass = 10 / 18 = 0.56 moles

    enthalpy of fusion = 3344 / 0.56 = 5971.43 J / mole
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