Chemistry

An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has a partial pressure of 217.0 torr, 13.2 torr, and 13.2 torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total pressure jumps to 263.0 torr. The appropriate chemical equation is PCl3(g) + Cl2(g) <=> PCl5(g)
Calculate the new partial pressures of PCl3, Cl2, and PCl5

Am i supposed to find Kp first..? please help me!

asked by Kat
  1. Yes, I would find Kp first.

    posted by DrBob222
  2. Hi lol

    Is this correct?:
    Kp = PPCl5/(PPCl3)(PCl2) = 217.0 torr/(13.2 torr)(13.2 torr) = 1.245

    x/(263 torr - x) = 1.245
    x = 327.435 - 1.245x
    2.245x = 327.435
    x = 145.85 torr = PPCl5

    263.0 total torr - 145.85 PCl5 torr = 117.15 torr - 13.2 torr = 103.95 torr for Cl2
    13.2 torr for Cl3?

    posted by Kat
  3. I would do this. First I would convert torr to atm.
    PPCl5 = 217/760 = 0.2855 atm
    PPCl3 = 13.2/760 = 0.01737 atm.
    PCl2 = 13.2/760 = 0.01737 atm
    Total P = 243.4/760 = 0.3203 atm
    Cl2 added = 263-243 = 19.6 and 19.6/760 = 0.02579

    ............PCl3 + Cl2 ==> PCl5
    initial..0.01737.0.01737..0.2855
    add.............0.02579..........
    change.......-p....-p.......+2p
    equil.0.01737-p.0.04316-p..0.2855+2p
    Substitute into Kp expression with these ICE chart values and solve for p.

    posted by DrBob222
  4. Hi Dr. Bob. I'm coming up with outrageous numbers for when I try to use atm's with my Kp value.. please look!

    Kp = PPCl5/PPCl3PCl2 = (0.2855)/(0.01737)(0.01737) = 946.3

    PCl3 : 0.01737-946.3 = -946.28 atm?!
    Cl2 : 0.04316 - 946.3 = -946.26 atm o.o
    PCl5 : 0.2855 + 2(946.3) = 1,892.8855 >.<

    when i tried it with torr it gave me 11.955, 31.555, and 219.49 >.< am i reading your directions correctly?

    posted by Kat
  5. ohh i'm sorry i understand now thank you Dr. Bob!

    posted by Kat

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