The equilibrium constant, Kp, for the reaction CO(g) + H₂O(g) CO₂(g) + H₂(g)
At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

Question

The equilibrium constant, Kp, for the reaction CO(g) + H₂O(g)

The equilibrium constant, Kp, for the reaction CO(g) + H<sub>2</sub>O(g) CO<sub>2</sub>(g) + H<sub>2</sub>(g) At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium? A) Yes. B) No, the forward reaction must proceed to establish equilibrium. C) No, the reverse reaction must proceed to establish equilibrium. D) Need to know the volume of the container before deciding. E) Need to know the starting concentrations of all substances before deciding.

CO₂(g) + H₂(g)
At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?

Quizplus · Accepted Answer

To determine if the system is at equilibrium, we need to calculate the reaction quotient, Qp, and compare it to Kp. Qp is calculated using the partial pressures of the gases in the container and is given by:
Qp = (PCO)(PH2O)/(PCOS)(PH2S)
Qp = (1.2 atm)(0.20 atm)/(0.30 atm)(0.27 atm)
Qp = 0.444
Since Qp < Kp, the forward reaction has not proceeded enough to establish equilibrium. Thus, the answer is B, and the forward reaction must proceed to establish equilibrium.

The Equilibrium Constant, Kp, for the Reaction CO(g) + H2O(g)

The Equilibrium Constant, Kp, for the Reaction CO(g) + H₂O(g)