19In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2+ (aq) is pinkand 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: CoCl42 (aq) Co2+ (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. DecreasesNextPrevious▲SONYDISPLAYWEBcokOFFOne Touch Web Access Without Booting UpF11F12Num LkScr LkPrt ScSys RaF10P4:18 AM4/30/2022VGN-NW350FBackspaceDeleteBreakHome At Low Temperature the pink color predominates.If we represent the equilibrium as: CoCl42 (aq) Co2+ (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.3. When the temperature is decreased the equilibrium concentration of CoC14²:A. IncreasesB. DecreasesC. Remains the sameD. More information is needed to answer this question.PreviousSONYWEBOFFOne Touch Web Access Without Booting UpAt High Temperature the blue color is strong.Next4:18 AM4/30/2022VGN-NW350F

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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: CoCl42 (aq) Co2+ (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. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases Previous SONY (--| | ه 4:18 AM 4/30/2022 VGN-NW350F

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: CoCl42 (aq) Co2+ (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. When the temperature is decreased the equilibrium constant, K: A. Increases B. Decreases Previous SONY (--| | ه 4:18 AM 4/30/2022 VGN-NW350F

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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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:... CoCl42-(aq) Co2+(aq) + 4Cl-(aq)We can conclude that: fill in the blank 1 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. fill in the blank 2 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. fill in the blank 3 3. When the temperature is increased the equilibrium concentration of CoCl42-: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
Which option is correct. And why
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K22.
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