In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl4². co2+(aq) is pink and CoCl42-(aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilibrium as: CoClą2 (aq) = co2+(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 increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of Co2*: 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 CoCl4². co2+(aq) is pink and CoCl42-(aq) is blue. At Low Temperature the pink color predominates. At High Temperature the blue color is strong. If we represent the equilibrium as: CoClą2 (aq) = co2+(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 increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of Co2*: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

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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