Observe the equilibrium reaction below: CO (g) + H 2 O (g) ↔ CO 2(g) + H 2(g) K = 4.00 at 900 ̊C

Question

If the following concentrations are introduced into a reaction vessel, in which direction would the reaction proceed to establish equilibrium? Show your work.

[CO] = 8.00 mol/L

[CO 2 ] = 8.00 mol/L

[H 2 O] = 4.00 mol/L

[H 2 ] = 4.00 mol/L

Answer 1

CO(g) + H₂O(g) <==> CO₂(g) + H₂(g) ... K = 4.00

8.00........4.00..............8.00.........4.00......concentrations in M

Reaction quotient = Q = [CO₂][H₂] / [CO][H₂O] = (8)(4) / (8)(4) = 1.00

Q = 1.00

K = 4.00

Q < K means the reaction must go toward the products in order to establish equilibrium. Under the current conditions, there aren't enough products and there is too much reactant.