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In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion COCI,2". Co2"(aq) is pink and CoCl,2 (aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilbrium as: Cocl, (aq)=Co*"(aq) + 4CI'(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. When the temperature is decreased the equilibrium concentration of CoCI,?: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion COCI,2". Co2"(aq) is pink and CoCl,2 (aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilbrium as: Cocl, (aq)=Co*"(aq) + 4CI'(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. When the temperature is decreased the equilibrium concentration of CoCI,?: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...
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In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion COCI,2". Co2"(aq) is pink and CoCl,2 (aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilbrium as: Cocl, (aq)=Co*"(aq) + 4CI'(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. When the temperature is decreased the equilibrium concentration of CoCI,?: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
Transcribed Image Text:In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion COCI,2". Co2"(aq) is pink and CoCl,2 (aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilbrium as: Cocl, (aq)=Co*"(aq) + 4CI'(aq) We can conclude that: 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. When the temperature is decreased the equilibrium concentration of CoCI,?: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
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