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MarcLeclair

URGENT! Consider the following decomposition reaction of ammonium carbonate ((NH4)2CO3): (NH4)2CO3 (s)  2 NH3 (g) + CO2 (g) + H2O (g) In one experiment at 25.0°C, a sample of pure (NH4)2CO3 is placed in an evacuated 2.00 L vessel. At equilibrium, the total pressure is found to be 0.8944 atm. (a) Determine the equilibrium partial pressure of each gaseous species. (b) Determine the mass of ammonium carbonate ((NH4)2CO3) that must have reacted in order to achieve equilibrium. (c) Determine the value of Kp assuming that the reaction temperature is 25.0°C. I can find a but I am stuck at b

  • one year ago
  • one year ago

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  1. Awstinf
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    use PV=nRT to find the moles and then convert back

    • one year ago
  2. MarcLeclair
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    but wait Im stuck with the ATM at equilibrium, the solid doesnt affect equilibrium at all, so how can I find it with the equilibrium of Pressure Don't I need concentration?

    • one year ago
  3. Awstinf
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    So you have pressure at EQ right?

    • one year ago
  4. Awstinf
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    4x=.8944

    • one year ago
  5. MarcLeclair
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    Yeah, the total, and I can use basic mole ratio to find individual pressure

    • one year ago
  6. Awstinf
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    solve for x then use the pressure for lets say CO2 put that into PV=nRT then solve for n then convert over

    • one year ago
  7. MarcLeclair
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    So I need to find n for one product than just use stoichiometry ?

    • one year ago
  8. Awstinf
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    yeah it should work.

    • one year ago
  9. Awstinf
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    let me work it out for you really fast

    • one year ago
  10. MarcLeclair
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    Alright ill try it and post if it works

    • one year ago
  11. Awstinf
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    (.2236)(2)/(298*.08206) = .0183*96g/mol = 1.76g

    • one year ago
  12. MarcLeclair
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    I cant beleive I didnt think of that, and for C , Q goes to infinity no? How to I possible use my Equilibrium constant equation?

    • one year ago
  13. MarcLeclair
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    How do I possibly*

    • one year ago
  14. Awstinf
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    for C? all you do is [NH3]^2[CO2][H2O]=Kp x=.2236 (2*.2236)^2(.2236)*(.2236)=.001

    • one year ago
  15. Awstinf
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    Not for PNH3 not [NH3] for each

    • one year ago
  16. MarcLeclair
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    Oh I thought you had to use ICE and Q to find the direction of the reaction :/ Apparently you don't thanks a lot!

    • one year ago
  17. Awstinf
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    Q is to judge where you are in respect to K if you have a larger Q you know you have far too many products so you need to get more reactants so the reaction goes to the left, if you have a small Q you know you have too many reactants and you need to go to products. you as in the reaction lol.

    • one year ago
  18. MarcLeclair
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    Ah I get it its just to judge the direction of the reaction BEFORE equilibrium but here we already reached it! Thanks a lot!

    • one year ago
  19. Awstinf
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    Yep you got it! good luck!

    • one year ago
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