Consider the following system at equilibrium where AH° = -16.1 k), and Kc = 154 , at 298 K: 2 NO (g) + Br2 (g) =2 NOB (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to K. C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will: A. Increase. B. Decrease. C. Remain the same.
Consider the following system at equilibrium where AH° = -16.1 k), and Kc = 154 , at 298 K: 2 NO (g) + Br2 (g) =2 NOB (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of Kc A. Increases B. Decreases C. Remains the same The value of Qc A. Is greater than Kc B. Is equal to K. C. Is less than Kc The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of Br2 will: A. Increase. B. Decrease. C. Remain the same.
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 6QRT: Indicate whether each statement below is true or false. If a statement is false, rewrite it to...
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![Consider the following system at equilibrium where AH° = -16.1 k), and Kc = 154 , at 298 K:
2 NO (g) + Br2 (g) =2 NOB (g)
If the TEMPERATURE on the equilibrium system is suddenly decreased :
The value of Kc
A. Increases
B. Decreases
C. Remains the same
The value of Qc
A. Is greater than Kc
B. Is equal to K.
C. Is less than Kc
The reaction must:
A. Run in the forward direction to restablish equilibrium.
B. Run in the reverse direction to restablish equilibrium.
C. Remain the same. Already at equilibrium.
The concentration of Br2 will:
A. Increase.
B. Decrease.
C. Remain the same.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fba6ecc4c-800b-41f4-ac67-14d30661fb42%2F27193d49-c9a1-4fa5-850e-fed5b6a66e3c%2Fuc3hrxw_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the following system at equilibrium where AH° = -16.1 k), and Kc = 154 , at 298 K:
2 NO (g) + Br2 (g) =2 NOB (g)
If the TEMPERATURE on the equilibrium system is suddenly decreased :
The value of Kc
A. Increases
B. Decreases
C. Remains the same
The value of Qc
A. Is greater than Kc
B. Is equal to K.
C. Is less than Kc
The reaction must:
A. Run in the forward direction to restablish equilibrium.
B. Run in the reverse direction to restablish equilibrium.
C. Remain the same. Already at equilibrium.
The concentration of Br2 will:
A. Increase.
B. Decrease.
C. Remain the same.
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