At 850°C, the equilibrium constant K_p for the reaction C(s) + CO₂(g) 2CO(g)
Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Question

At 850°C, the equilibrium constant K_p for the reaction C(s) + CO₂(g)

At 850°C, the equilibrium constant K<sub>p</sub> for the reaction C(s) + CO<sub>2</sub>(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide? A) 0.362 atm B) 0.489 atm C) 0.667 atm D) 0.915 atm E) 0.921 atm

2CO(g)
Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

Quizplus · Accepted Answer

The Answer of At 850°C, the equilibrium constant K_p for the reaction C(s) + CO₂(g) 2CO(g) Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?

At 850°C, the Equilibrium Constant Kp for the Reaction C(s)

At 850°C, the Equilibrium Constant K_p for the Reaction C(s)