college chemistry

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please help!

If the initial pressure of I2(g) is 1.738 atm, calculate the % decomposition of I2(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kp at 1000 K is 0.254. The initial pressure of the reaction products is 0 atm.


I2(g) = 2I(g)

  • college chemistry -

    Set up an ICE chart, substitute into Kp expression, and solve.

  • college chemistry -

    i did.. it was wrong for the last time

  • college chemistry -

    for the last time i did it*

  • college chemistry -

    If you post what you did perhaps I can find the error.

  • college chemistry -

    initial:
    I2 = 1.738 atm
    2I = 0

    change:
    I2 = -2x
    2I = x

    equilibrium:
    I2 = 1.738 - 2x
    2I = x

    so i set the equation as
    0.254 = x/(1.738 - 2x)
    and i solved for x. i got 0.292
    and after that how do i get % decomposition?

  • college chemistry -

    equilibrium:
    I^- (not 2I) = 2x
    I2 = 1.738-x
    Then Kp = pI^-^2/pI2
    0.254 = (2x)^2/(1.738-x).
    Solve for x. You didn't have 2x and then didn't square it.
    %decomposition = (pI^-/1.738)*100 = ??

  • college chemistry -

    What is the pressure in a 10.0- cylinder filled with 0.405 of nitrogen gas at a temperature of 327k?

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