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The equilibrium constant for 2 CO2 (g) ⇌ 2 CO (g) + O2 (g) is 1.12x10-45...

The equilibrium constant for 2 CO2 (g) ⇌ 2 CO (g) + O2 (g) is 1.12x10-45 at room temperature. If the initial concentration of CO2 is 10 mM, what are the equilibrium concentrations of all three chemicals? The equilibrium constant is small, so you can assume x will be small.

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Answer #1

            2 CO2 (g) ⇌ 2 CO (g) + O2 (g)

Initial   10mM            0              0

Final   (10mM-2x)    2x              x

Keq = 1.12 * 10^(-45) = [CO]^2[O2]/[CO2]^2

1.12 * 10^(-45) = 4x^3/10mM (assuming 2x is very small as compared to x)

11.2 * 10^(-48) = 4x^3

x^3 = 2.8 * 10^(-48)

x = 1.4094 * 10^(-16) M

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