At a certain temperature, the reaction below has an equilibrium constant of 42. Which of the following is correct if 2.0 moles of hydrogen, 3.0 moles of oxygen, and 6.0 moles of water are placed in a 12.0 L container and allowed to reach equilibrium at this temperature? 2 H₂ (g) + O₂ (g) ⇒ 2 H₂O (g) Q = 0.33 and the system reaches equilibrium by increasing the amount of H₂O. Q = 3.0 and the system reaches equilibrium by increasing the amount of H₂O. Q = 3.0 and the system reaches equilibrium by decreasing the amount of H₂O. Q = 36 and the system reaches equilibrium by decreasing the amount of H₂O. Q = 36 and the system reaches equilibrium by increasing the amount of H₂O.

At a certain temperature, the reaction below has an equilibrium constant of 42. Which of the following is correct if 2.0 moles of hydrogen, 3.0 moles of oxygen, and 6.0 moles of water are placed in a 12.0 L container and allowed to reach equilibrium at this temperature? 2 H₂ (g) + O₂ (g) ⇒ 2 H₂O (g) Q = 0.33 and the system reaches equilibrium by increasing the amount of H₂O. Q = 3.0 and the system reaches equilibrium by increasing the amount of H₂O. Q = 3.0 and the system reaches equilibrium by decreasing the amount of H₂O. Q = 36 and the system reaches equilibrium by decreasing the amount of H₂O. Q = 36 and the system reaches equilibrium by increasing the amount of H₂O.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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