At 200°C, the equilibrium constant (K_p) for the reaction below is 2.40 × 10³. 2NO (g) N₂ (g) + O₂ (g)
A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O₂ is __________ atm.

Question

At 200°C, the equilibrium constant (K_p) for the reaction below is 2.40 × 10³. 2NO (g)

At 200°C, the equilibrium constant (K<sub>p</sub>) for the reaction below is 2.40 × 10<sup>3</sup>. 2NO (g) N<sub>2</sub> (g) + O<sub>2</sub> (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O<sub>2</sub> is __________ atm. A) 294 B) 35.7 C) 17.9 D) 6.00 E) 1.50 × 10<sup>-2</sup>

N₂ (g) + O₂ (g)
A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O₂ is __________ atm.

Quizplus · Accepted Answer

From the equilibrium constant, we can write the expression for the reaction quotient as: Qp=P₂/NO^2.O₂ At equilibrium, Qp=K_p=2.40×10³ Let the partial pressure of O₂ at equilibrium be x atm. Then, Qp=x^2/36.1 Equating the two expressions for Qp and solving for x, we get: x=6.76 atm Therefore, the partial pressure of O₂ at equilibrium is 6.76 atm, which is closest to option C (17.9 atm).

At 200°C, the Equilibrium Constant (Kp)for the Reaction Below Is

At 200°C, the Equilibrium Constant (K_p)for the Reaction Below Is