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Finding Equilibrium Constants

  1. Feb 12, 2006 #1
    a. If the equilibrium concentration of AB3 is 1.5600 mol/L, and the equilibrium concentration of B2 is 0.3300 mol/L, determine the equilibrium constant for this reaction.

    2AB3 (g) <-> A2 (g) + 3B2 (g)


    Well, K_c = [B2]^3[A2]/[AB3]^2

    [B2] = 0.3300 M
    [AB3] = 1.5600 M
    [A2] = ???

    [A2] = 0.3300 M B2 (1 mol A2/3 mol B2) = 0.11 M ???

    K_c = [0.330 M]^3[0.11 M]/[1.5600 M]^2 = 1.624E-3 ??


    b. If the initial concentration of AB3 is 0.6300 mol/L, and the equilibrium concentration of A2 is 0.14600 mol/L, determine the equilibrium constant for this reaction.

    2AB3 (g) <-> A2 (g) + 3B2 (g)

    Once again, K_c = [B2]^3[A2]/[AB3]^2

    But
    [B2] = 0.14600 M A2 * (3 mol B2/ 1 mol A2) = 0.4380 M
    [AB3] = 0.14600 M A2 *(2 mol AB3/ 1 mol A2) = 0.292 M
    so 0.6300 M - 0.292 M = 0.338 M
    [A2] = 0.14600 M

    K_c = [0.14600 M][0.4380 M]^3/[0.3380 M]^2 = 1.074E-1 ?

    Thanks.
     
  2. jcsd
  3. Feb 13, 2006 #2
    They are both correct I believe.
     
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