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Consider the following system at equilibrium where AH° = -108 kJ, and Kc = 77.5, at 600 K: co (g) + Cl₂ (g) = COCl₂ (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 Kc 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 Cl₂ will: A. Increase. B. Decrease. C. Remain the same.

Consider the following system at equilibrium where AH° = -108 kJ, and Kc = 77.5, at 600 K: co (g) + Cl₂ (g) = COCl₂ (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 Kc 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 Cl₂ will: A. Increase. B. Decrease. C. Remain the same.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter16: Spontaneity Of Reaction
Section: Chapter Questions
Problem 61QAP: Consider the reaction CO(g)+H2O(g)CO2(g)+H2(g) Use the appropriate tables to calculate (a) G at 552C...
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Use the References to access important values if needed for this quest Consider the following system at equilibrium where AH° = -108 kJ, and Kc = 77.5, at 600 K: co (g) + Cl₂ (g) = CoCl₂ (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 Kc 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 Cl2 will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Try Another Version 9 item attempts remaining
Transcribed Image Text:Use the References to access important values if needed for this quest Consider the following system at equilibrium where AH° = -108 kJ, and Kc = 77.5, at 600 K: co (g) + Cl₂ (g) = CoCl₂ (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 Kc 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 Cl2 will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Try Another Version 9 item attempts remaining
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