C(s) + H20(g)↔ CO(s) + H2(s)
the equilibrium constant for this reaction is 4.251 x 10^-2 at 800 K. if the equilibrium concentration of H2O(g)is 0.1990 M, what are the concentrations of CO, H2, and C?
I think you have this labeled wrong. CO and H2 certainly are not solids at 800 K; however, assuming you meant this then the concn of solid is 1, by definition, for C, CO, and H2. That definitely is not correct.
To find the concentrations of CO, H2, and C at equilibrium, we need to use the equilibrium constant expression and the given information.
The equilibrium constant expression for the reaction is as follows:
Kc = [CO][H2] / [C][H2O]
Given:
Equilibrium constant (Kc) = 4.251 x 10^-2
Concentration of H2O(g) at equilibrium ([H2O]) = 0.1990 M
We can plug in these values into the equilibrium constant expression:
4.251 x 10^-2 = [CO][H2] / [C][H2O]
To solve for the concentrations of CO, H2, and C, we need one more piece of information. It could be either the value of one of the concentrations or the value of the equilibrium constant at the given temperature. Since we don't have any other concentration information, we need to know the value of the equilibrium concentration of at least one of the species.
Please provide additional information or specify a value for one of the concentrations to continue.