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Chemistry Temperature Problem

  1. Mar 26, 2009 #1
    1. The problem statement, all variables and given/known data[/b]

    A 20.0 g sample of ice at -10.0 degrees Celsius is mixed with 100.0 g of water at 80.0 degrees Celsius. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H20 (solid) and H20 (liquid) are 2.08 J/g deg. Celsius and 4.18 J/g deg. Celsius respectively, and the enthalpy of fusion of ice is 6.01 kJ/mol.

    The answer is 52.4 deg. Celsius. But I am unsure of how to get the answer. Please help asap. No heat loss means no heat (J) is lost to the environment, so you can basically ignore that part of the question.

    2. Relevant equations
    q=mc delta T
    phase change formulas: there are none. Have to use a heating curve to change from solid to liquid and so on.

    c=specific heat
    q=heat in Joules
    T=temperature in this case celsius
     
    Last edited: Mar 26, 2009
  2. jcsd
  3. Mar 26, 2009 #2

    Mapes

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    How about an equation associated with phase changes?
    What's the implication of the assumption of "no heat loss"?
     
  4. Mar 27, 2009 #3

    Borek

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    Staff: Mentor

    Latent heat.
     
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