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Stoichiometry problem

  1. Feb 10, 2008 #1
    1. The problem statement, all variables and given/known data

    "How many grams of hydrogen are necessary to react completely with 50.0g of nitrogen in the below reaction?"

    2. Relevant equations

    N2+3H3 ---> 2NH3

    3. The attempt at a solution

    16.1g H?
  2. jcsd
  3. Feb 10, 2008 #2
    Show your work.
  4. Feb 10, 2008 #3
    50gN/1 1molN/28gN 3molH/1mol N 3gH/1molH
  5. Feb 10, 2008 #4
    Close enough, I didn't round off like you did.
  6. Feb 10, 2008 #5
    I guess my only question is since N2 is diatomic, then the molar mass of the nitrogen goes from 14 to 28?
  7. Feb 10, 2008 #6
    That's right.
  8. Feb 10, 2008 #7
    Um, so would that also mean here the molar mass of should be changed to 6...so the answer would be 32.14g?
  9. Feb 10, 2008 #8
    Dangit, after looking at your problem. I didn't even notice you messed up the reaction equation. It's Hydrogen gas, [tex]H_2[/tex], not [tex]H_3[/tex]. Fix that and it's solved.
  10. Feb 11, 2008 #9
    Roco, are you slipping? :)
  11. Feb 11, 2008 #10
    Sorry for bringing up a dead topic, but I didnt want to just start a new one for basically the same thing...I just wanted to ask...

    5 L N2/1 1molN2/22.4L N2

    That's how I began setting up a problem, but is 22.4 right? Should it be something different since Nitrogen is diatomic?
  12. Feb 11, 2008 #11
    The volume of one mol of any gas at standard temp/pressure is 22.4 I don't care if it's gaseous Uranium.

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