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 equilibrium?

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 at equilibrium? 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 at equilibrium?

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 equilibrium? A) 0.362 atm B) 0.489 atm C) 0.667 atm D) 0.915 atm E) 0.921 atm

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)