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Smash Lord
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.
If we add CO2 to increase its concentration to 0.75 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished?
I would greatly appreciate any help on the matter. Also, an explanation as to how you got your answer would be helpful. I don't know how to do this.
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.
If we add CO2 to increase its concentration to 0.75 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished?
I would greatly appreciate any help on the matter. Also, an explanation as to how you got your answer would be helpful. I don't know how to do this.
