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Homework Help: When heat becomes confusing

  1. Sep 26, 2010 #1
    1. The problem statement, all variables and given/known data

    Question 1: Hot water at 100 degrees is added to 5 g of ice at 0 degrees. What is the minimum mass of hot water needed to melt all the ice? (Specific latent heat of fusion of ice = 336Jg-1, specific heat capacity of water is 4.2Jg-1K-1)

    2. The attempt at a solution

    Question 1:
    mc[tex]\Delta[/tex][tex]\theta[/tex] = m(latent fusion)
    m[tex]\Delta\theta[/tex] = 400
    And then I have a doubt: How can the hot water's temperature decrease from 100 degrees to 0 degrees? ([tex]\Delta\theta[/tex] = 100 - 0)
  2. jcsd
  3. Sep 26, 2010 #2
    what does this mean?
  4. Sep 28, 2010 #3
    Change in temperature.
  5. Sep 28, 2010 #4
    Think about it this way.
    What is the starting temperature of my hot water? 100
    What is the final temperature of my "hot" water? 0
    What is the change in temperature? 100-0
    Delta T is 100
  6. Sep 28, 2010 #5


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    Staff Emeritus
    Science Advisor

    The questions asks for "the minimum mass of hot water to melt ice". So all of the heat must go into the ice to melt it. The melting temperature of water/ice is 0°C.
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