chemistry

Gaseous CO2 decomposes to form the gaes CO and O2. At 20.0 degrees Celsius, =2.0*10^-8.
2.0 mol carbon dioxide is placed in a 5.0 L flask. What are the equilibrium concentrations of each species.

My attempt to get the answer:
Balanced equation: 2CO2--> 2CO+O2

To get the equilibrium for CO and O2, I know i have to find the initial-change=equil.

I think the Initial for CO2 is 2.0 mol and change is zero, so the equil. for CO2 is 2.0. How do I find the equil. for CO and O2?

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  1. You don't say if 2.0 x 10^-8 is Kp or Kc.
    Your balanced equation is ok but thereafter is not.
    2CO2 ==> 2CO + O2
    If the K you omitted is Kc, then,

    initial:
    (CO2) = 2.0
    (CO)=0
    (O2)=0

    change:
    (CO) = +x
    (O2) = +x
    (CO2) = -2x

    equilibrium:
    (CO) = +x
    (O2) = +x
    (CO2) = 2.0 - 2x
    Now plug these equilibrium values into Kc expression and solve.
    If K is Kp, you need to change Kp to Kc or solve it with partial pressures.

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    posted by DrBob222

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