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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