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Henry's Law Question

  1. Jun 3, 2015 #1
    1. The problem statement, all variables and given/known data
    How much water would be needed to completely dissolve 1.48L of the gas at a pressure of 730torrand a temperature of 28∘C? A gas has a Henry's law constant of 0.190M/atm

    2. Relevant equations
    S=kH * Pgas
    3. The attempt at a solution
    730 torr= .960526316 atm

    S=(.190M/atm)(.960526316 atm)
    S= .1825 M
    .1825 mol = X = .2701 moles
    1 L 1.48L

    After solving that part I don't understand how to get liters of water. Maybe PV=nRT... but I tried that and I got the answer wrong.
     
  2. jcsd
  3. Jun 3, 2015 #2

    Borek

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    Staff: Mentor

    How many moles of the gas? How many dissolved per liter of water?
     
  4. Jun 3, 2015 #3
    .2701 moles of the gas
     
  5. Jun 3, 2015 #4

    Borek

    User Avatar

    Staff: Mentor

    No. 1.48 L of gas at 730 torr and 28°C is not 0.27 moles.
     
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