equilibrium consant Kc and concentrations
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Consider the following equilibrium process at 686°C:
CO2(g) + H2(g) CO(g) + H2O(g)
The equilibrium concentrations of the reacting species are [CO] = 0.050 M, [H2] = 0.045 M, [CO2] = 0.086 M, and [H2O] = 0.040 M.
(a) Calculate Kc for the reaction at 686°C.
(I got Kc=.52 which is correct but now I don't know how to do part B)
(b) If we add CO2 to increase its concentration to 0.25 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished?
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Solution Summary
The solution is comprised of step-by-step calculations of the equilibrium constant Kc and the concentrations of the chemicals when a new equilibrium is re-established by adding more reactant.
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(a) Kc =[CO]*[H2O] / {[CO2]*[H2]}
then Kc = (0.050 * 0.040) /(0.086 * 0.045) = 0.52
(b) Write the initial, change and equilibrium concentrations of all chemicals.
Treat the concentrations of previous equilibrium as the initial concentrations except ...
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