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Chemistry Equilibrium with Kp

  1. Oct 18, 2011 #1
    Ok so I don't know what to do to find out whether the reaction has reached equilibrium or not because I wasn't sure whether the relationship between the equilibrium constant and the reaction quotient is the same for the equilibrium partial pressures(Kp)

    N2(g) + 3H2(g) <----> 2NH3(g)

    PNH3 = 3.1 X 10-2 atm
    PN2 = 8.5 X 10-1 atm
    PH2 = 3.1 X 10-3 atm

    I calculated the Kp value for these pressures to be 3.8 X 104

    The problem next says: If PN2 = 0.525 atm, PNH3 = 0.0167 atm ,and PH2 = 0.00761 atm, does this represent a system at equilibrium.

    I calculated the Kp value for these and got 1.2 X 103

    So do I next find the reaction quotient and compare the 2nd Kp value to that in order to find out whether the second set of values reaches equilibrium or not.

    PLEASE HELP I'M SORRY FOR ALL THE WRITING
     
  2. jcsd
  3. Oct 19, 2011 #2

    Borek

    User Avatar

    Staff: Mentor

    Yes, it is the same as between concentrations and Kc.
     
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