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A quantity of ice at 0.0 degrees C was added to 33.6 of water at 21.0 degree C to give water at 0.0 degrees C. How much ice was added? The heat of fusion of water is 6.01 kJ/mol and the specific heat is 4.18 J/(g * degrees C)

q = mass x specific heat x delta T?
q = mass x heat fusion?

I don't understand what to plug in
and where

  • Chemistry -

    heat removed from water in going from 21.0 to zero C is
    mass x specific heat x delta T.
    mass = 33.6 g
    specific heat is 4.184 J/g*K
    delta T is 21.0 - 0.

    heat added to ice to melt it is
    mass x heat fusion.
    mass is the unknown.
    heat fusion is given.
    Note: you need to work in the same units. The heat of fusion is quoted in the problem in kJ/mol but I quoted the specific heat of water in J/gram. One needs to be changed. I would suggest the 4.184 be changed.

  • Chemistry -

    how much energy is required to melt 32.0 grams of ice (8.02 g/mol)?

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