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Chemistry "Equilibrium" help?

Consider the following equilibrium at 1000K:

2SO2 (g) + O2 (g) ↔ 2SO3 (g)

A study of this system reveals that there are 3.5E-3 moles of sulfur dioxide gas, and 5.0E-3 moles of oxygen gas present in a 12.0L flask at equilibrium. The equilibrium constant for this reaction is 3.5E-3. Calculate the number of moles of SO3(g) in the flask at equilibrium.

2 Answers

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  • Dr.A
    Lv 7
    1 decade ago
    Favorite Answer

    initial concentration SO2 = 3.5 x 10^-3 / 12.0 = 0.00029 M

    initial concentration O2 = 5.0 x 10^-3 / 12.0 =0.00042 M

    2 SO2 + O2 <------> 2SO3

    change

    -2x .. .. . .-x .. . . . . . +2x

    3.5 x 10^-3 = (2x)^2 / (0.00029 - 2x)^2 ( 0.00042-x)

    solve for x

    concentration SO2 at equilibrium = 0.00029 - 2x

    multiply by 12.0 to get the moles

  • ?
    Lv 4
    4 years ago

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