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Can someone tell me why this method is wrong even though it seems logical?

  1. Aug 24, 2007 #1
    1. The problem statement, all variables and given/known data
    Solid lithium hydroxide is used in space vehicles to remove exhaled carbon dioxide from the living environment by forming solid lithium carbonate and liquid water. What mass of gaseous carbon dioxide can be absorbed by 1.00kg of lithium hydroxide?

    3. The attempt at a solution

    First, I balanced out the equation with the reactants and products:

    [tex]2LiOH+CO_2 \right arrow Li_{2}CO_{3}+H_{2}O[/tex]

    Then I found the molar mass of LiHO to be: 23.949g/ mol LiHO

    So then I did this:

    [tex]\frac{23.949g}{mol \\LiHO} \times \frac{2mol LiHO}{1molCO_{2}}=\frac{47.898g}{1molCO_2} \times \frac{1molCO_2}{44.01g}[/tex]

    Other than that the units cancel out.. can someone tell me why it is wrong and how to avoid these problems? As of now, I just try to cancel the units out to get grams but I don't really have a "systematic" way of doing things. Is there a a systematic way? How do avoid not knowing what you are doing and how to arrive at the right answer? Thanks.
  2. jcsd
  3. Aug 24, 2007 #2
    [tex]1000g LiOH \frac{(12.01+32.0)g CO_2}{2(6.941+16.0+1.01)g LiOH} = 919g CO_2[/tex]

    Last edited: Aug 24, 2007
  4. Aug 24, 2007 #3
    My book says the answer is 920g.
  5. Aug 24, 2007 #4
    lol damn i'm way off, ok let me check

    EDIT: ok i obviously shouldn't calculate in the dark, lol

    i got 919g CO2

    since you have a 2:1 stoichiometric ratio between LiOH and CO_2. i assume bc like to avoid writing too much, so i skip out on the moles and assume they cancel out nicely and just stick to the units that i am required in my answer.
    Last edited: Aug 24, 2007
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