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Enthalpy, water, vaporization

  1. Dec 25, 2015 #1
    1. The problem statement, all variables and given/known data
    If I have a pot of water that I want to bowl so that there won't be any water left then the energy that I have to add is:

    E=c*m*delta T
    E=l(vaporization) * m

    But if I have wet clothes and want the water to evaporate then the energy needed is:

    E=l(vaporization)m

    So from the equations it would take ess energy to evaporate water than to boil it and then make it into a gas. But my book is saying that it takes more energy to evaporate water right away
    2. Relevant equations


    3. The attempt at a solution
     
  2. jcsd
  3. Dec 25, 2015 #2

    Bystander

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    "L," latent heat, is larger for the lower temperature.
     
  4. Dec 26, 2015 #3
    Word-for-word, what exactly does your book say?

    Chet
     
  5. Dec 26, 2015 #4
    the book is in another language so I have to translate it.

    "The clothes will dry even if it is near 0 degrees celsius, it just requires a little more energy.
     
  6. Dec 27, 2015 #5
    See Bystander's answer in post #2.
     
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