Consider the following system at equilibrium where AH = -198 kJ, and K. = 34.5 , at 1.15×103 K:2 S02 (g) + 02 (g) 2 S03 (g)If the TEMPERATURE on the equilibrium system is suddenly decreased:The value of K.A. IncreasesB. DecreasesC. Remains the sameThe value of QcA. Is greater than K.B. Is equal to K.C. Is less than K.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 0, will:A. Increase.B. Decrease.C. Remain the same.

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Consider the following system at equilibrium where AH° = -198 kJ, and K. = 34.5 , at 1.15×10³ K: 2 S02 (g) + 02 (g) 2 S03 (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of K. A. Increases B. Decreases C. Remains the same

Consider the following system at equilibrium where AH° = -198 kJ, and K. = 34.5 , at 1.15×10³ K: 2 S02 (g) + 02 (g) 2 S03 (g) If the TEMPERATURE on the equilibrium system is suddenly decreased : The value of K. A. Increases B. Decreases C. Remains 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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Question

Consider the following system at equilibrium where AH = -198 kJ, and K. = 34.5 , at 1.15×103 K:
2 S02 (g) + 02 (g) 2 S03 (g)
If the TEMPERATURE on the equilibrium system is suddenly decreased:
The value of K.
A. Increases
B. Decreases
C. Remains the same
The value of Qc
A. Is greater than K.
B. Is equal to K.
C. Is less than K.
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 0, will:
A. Increase.
B. Decrease.
C. Remain the same.

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