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Homework Help: Henry's law (finding moles)

  1. Mar 12, 2010 #1
    1. The problem statement, all variables and given/known data

    The henry's law constant (k) for carbon monoxide in water at 25 degree C is 9.71 * 10 ^-4 mol/(L*atm)

    How many moles of CO will dissolve in 1.00 L of water if the partial pressure of CO is 2.75 atm?

    2. Relevant equations

    waht pressure of carbon dioxide is required to keep the carbon dioxide concentration in a bottle of club soda at .12 M at 25 degrees C?
    Info: Kh for Co2 at 25 degrees C = 3.4 * 10^-2 M/atm

    Answer to that is 3.5 atm

    3. The attempt at a solution

    s(g) = Kh * Pg
    Since i don't have the Molarity i have no idea what to do.
    M = moles solute ( i dont know if the water or CO is the solvent or solute)
    divided by L solution

    (9.71*10^-4mol/L*atm)(2.75 atm) = 2.67 *10^-3 mol/L
    2.67*10^-3 mol/L * 1.00 L = 2.67*10^-3 mol
    i have no idea what to do from there
  2. jcsd
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