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.
A student determines [FeSCN2+] is 0.00016 M at equilibrium. If the initial concentration of Fe3+ was 0.00080 M and the initial SCN- concentration was 0.0012 M, what is the measured value of Kc?
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hello, i submitted this question before but the answers were not correct. Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction: I-(aq) + I2(aq)= I3-(aq) K = 710. For each of the following cases calculate the equilibrium ratio of [I3-] to [I2]. 1a) 6.00×10-2 mol of I2 is added to 1.00 L of 6.00×10-1 M KI solution. 1b)The solution above is diluted to 11.00 L.
Given these initial concentrations: [SCN-] = 0.000644 M, [Fe3+] = 0.000505 M, and [Fe(SCN)2+] = 0.000 M, determine the value for K if the [Fe(SCN)2+] at equilibrium is 0.0000856 M.
Iodine is sparingly soluble in pure water. However, it does `dissolve' in solutions containing excess iodide ion because of the following reaction: I-(aq) + I2(aq)= I3-(aq) K = 693. For each of the following cases calculate the equilibrium ratio of [I3-] to [I2]. A) 3.00×10-2 mol of I2 is added to 1.00 L of 3.00×10-1 M KI solution. B)The solution above is diluted to 5.50 L.
Calculate the equillibrium constant using the balanced chemical equation and the concentration of he substances at equilibrium. Based on the calculated value of K which is favored for the reaction products (fwd) or reactants (rev)? 2NO2 (g)= N2O4 (g) [NO2]=.0760 M [N2O4]=1.26 M