In an aqueous chloride solution cobalt(II) exists in equilibrium with the complexion CoCl,?. Co2"(aq) is pink and CoCl,²(aq) is blue.At Low Temperature the pink colorpredominates.At High Temperature the bluecolor is strong.If we represent the equilibrium as: CoCl, (ag)=Co**(aq) + 4Cl(aq)We can conclude that:| 1. This reaction is:A. ExothermicB. EndothermicC. NeutralD. More information is needed to answer this question.| 2. When the temperature is decreased the equilibrium constant, K:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question.When the temperature is decreased the equilibrium concentration|3. of Co2+:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question.

Given , colour ofCoCl42-= blue colour of Co2+= pink equilibrium reaction : CoCl42-(aq)⇌Co2+(aq)+4Cl-

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl,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 equilibrium as: CoC1,²"(aq) : Co*(aq) + 4CI'(aq)

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl,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 equilibrium as: CoC1,²"(aq) : Co*(aq) + 4CI'(aq)

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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Question

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex
ion CoCl,?. 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 equilibrium as: CoCl, (ag)=Co**(aq) + 4Cl(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
|3. of Co2+:
A. Increases
B. Decreases
C. Remains the same
D. More information is needed to answer this question.

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