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HS Thermochemistry Problem

  1. Nov 5, 2014 #1
    1. The problem statement, all variables and given/known data

    If 13.4 kJ of heat is added 1.00 kg of ice at 0ºC, how much ice will be melted

    2. Relevant equations

    Change of Heat = mass*change of temperature*constant

    change of heat fusion (water) = 333 J/g

    change of heat water vapor = 2260 J/g

    change of heat total = change of heat (state) + change of heat (temp change)

    constant of water = 4.184 J/gºC

    constant of ice = 2.1 J/gºC
    3. The attempt at a solution

    (1000g)(2.1J/gºC)(?-0) + (13400g*333J/gºC)

    Answer = 40g
     
  2. jcsd
  3. Nov 5, 2014 #2
    Hi ThePageHendrix. Welcome to Physics Forums!!!

    If it takes 333 kj to melt the entire 1 kg of ice, how much ice will only 13.4 kj melt?

    Chet
     
  4. Nov 5, 2014 #3
    Thanks for answering!

    Sorry, but it takes 333 joules, not kj, to melt the ice. I'm sorry, but I am just really lost on how to approach this problem.

    Any more help is appreciated, thanks!
     
  5. Nov 5, 2014 #4
    It takes 333J to melt 1 gm; it takes 333kJ to melt 1 kg.
     
  6. Nov 6, 2014 #5

    Borek

    User Avatar

    Staff: Mentor

    This equation describes amount of heat when dealing with the temperature change. When the ice melts, temperature doesn't change (in such cases we say it is a "latent heat"). Latent heat requires different equation. Chet already pointed you at the intuition behind the other equation you need.
     
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