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.
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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