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
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![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?
\[ 2 \text{H}_2 (g) + \text{O}_2 (g) \rightleftharpoons 2 \text{H}_2\text{O} (g) \]
- \( \bigcirc \) Q = 0.33 and the system reaches equilibrium by increasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 3.0 and the system reaches equilibrium by increasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 3.0 and the system reaches equilibrium by decreasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 36 and the system reaches equilibrium by decreasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 36 and the system reaches equilibrium by increasing the amount of \( \text{H}_2\text{O} \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2cfc3a1d-71f5-4849-9f61-cac9f1c46434%2Fd68ee912-0911-4cc5-8e16-55f6bb5acb86%2Fz3qybba_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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?
\[ 2 \text{H}_2 (g) + \text{O}_2 (g) \rightleftharpoons 2 \text{H}_2\text{O} (g) \]
- \( \bigcirc \) Q = 0.33 and the system reaches equilibrium by increasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 3.0 and the system reaches equilibrium by increasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 3.0 and the system reaches equilibrium by decreasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 36 and the system reaches equilibrium by decreasing the amount of \( \text{H}_2\text{O} \).
- \( \bigcirc \) Q = 36 and the system reaches equilibrium by increasing the amount of \( \text{H}_2\text{O} \).
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