Final answer:
To find the equilibrium concentrations of CO₂, H₂, CO, and H₂O, an ICE table is utilized to determine changes in concentrations from the initial state to equilibrium. The equilibrium concentrations can then be found by applying the equilibrium constant expression for the reaction and solving for the change in concentration, denoted as x.
Step-by-step explanation:
To calculate the equilibrium concentrations of CO₂, H₂, CO, and H₂O at 800 K when only CO and H₂O are present initially at concentrations of 0.137 M, we must apply the principles of chemical equilibrium using a reaction table.
Let's consider the balanced equilibrium equation:
H₂(g) + CO₂(g) → H₂O(g) + CO(g)
And the given equilibrium constant (K) at a similar temperature (700 K).
Firstly, we set up an ICE (Initial, Change, Equilibrium) table to track the changes in concentration. Since the reaction starts with only CO and H₂O, the initial concentrations of H₂ and CO₂ would be zero, and the change in concentration for H₂ and CO₂ would be +x, whereas for CO and H₂O it would be x (since they're reacting).
Then, we apply the equilibrium constant expression:
K = [CO][H₂O] / [H₂][CO₂]
Substituting the equilibrium concentrations from our ICE table into this expression allows us to solve for x, the change in concentration.
Lastly, the final equilibrium concentrations are the initial concentrations plus or minus x, depending on whether the substance is a reactant or product. We must note that the exact value of K at 800 K may differ from the provided 700 K value, so this answer assumes the K value does not significantly change with temperature which might not be accurate for all reactions.