2+In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC142. Co²+ (aq) is pink and CoCl2(aq) is blue.At low temperature the pink color predominates. At high temperature the blue color is strong.If we represent the equilibrium as:2+CoCl2(aq) Co²+ (aq) + 4C1¯ (aq)We can conclude that:1. This reaction isO exothermic.O endothermic.Oneutral.O More information is needed to answer this question.2. When the temperature is decreased the equilibrium constant, K:O increases.decreases.remains the same.O More information is needed to answer this question.3. When the temperature is decreased the equilibrium concentration of Co²+:Prev

Step 1: As we see the product of the reaction is pink colour Cobalt ions , so pink colour is…

Answered: 2+ In an aqueous chloride solution…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 13.101PAE

See similar textbooks

Similar questions

Chromium(VI) forms two different oxyanions, the orange dichromate ion, Cr2O72 , and the yellow chromate ion, CrO42 . (See the following photos.) The equilibrium reaction between the two ions is Cr2O72(aq)+H2O(l)2CrO42(aq)+2H+(aq) Explain why orange dichromate solutions turn yellow when sodium hydroxide is added.
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoClą2-. 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 CoCl². Co²+ (aq) is pink and CoC14² (aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: Co²+ (aq) + 4C1 (aq) = CoCl₂² (aq) We can conclude that: 1. This reaction O exothermic. O endothermic. Oneutral. O More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: O increases. Odecreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of Co²+: O increases. Odecreases. O remains the same. OMore information is needed to answer this question. Previc
In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCL42. Co²+ (aq) is pink and CoC14²(aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: CoC14²(aq) Co²+ (aq) + 4Cl¯ (aq) We can conclude that: 1. This reaction is O exothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of CoC₁4²: O increases. O decreases. O remains the same. O More information is needed to answer this question.
The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe3+(aq) ++ SCN−(aq) ↽−−⇀↽−−⇀ Fe(SCN)2+(aq) increasing the concentration of Fe3+ decreasing the concentration of Fe(SCN)2 increasing the temperature of the system Answer Bank ↑↑ ↓↓
The formation of the iron(III) thiocyanate complex ion is an exothermic equilibrium system. For each change to the system, indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium. An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. Fe (aq) + SCN (aq) = Fe(SCN)²+* (aq) increasing the concentration of Fe³+ decreasing the concentration of Fe(SCN)²+ increasing the temperature of the system Answer Bank about us carten privacy polic terms of use contact us help
The equation below shows the equilibrium that exists between the two ions of copper. A mixture of the two lons has an intermediate blue-green color. Cu(H₂O) (aq) + 4C (aq) CuCl(aq) + 4H₂O(1) blue yellow Predict what color the mixture above will have as a result of the following changes in the space provided below indicate your prediction and explain why the resulting colors appear. [Explanations must be specific and relate to concepts learned in this class) Al Sodium chloride (NaCl) is added to the mixture, b Water is added to the mixture
For the aqueous [Ag (NH3)2] complex K, =1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0072 M AgNO3 solution and 0.72M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. м x10 X
In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC14². Co²+ (aq) is pink and CoC14² (aq) is blue. At low temperature the pink color predominates. At high temperature the blue color is strong. If we represent the equilibrium as: Co²+ (aq) + 4Cl¯¯(aq) ⇒ CoCl² (aq) We can conclude that: 1. This reaction is O exothermic. O endothermic. O neutral. O More information is needed to answer this question. 2. When the temperature is decreased the equilibrium constant, K: O increases. O decreases. O remains the same. O More information is needed to answer this question. 3. When the temperature is decreased the equilibrium concentration of Co²+: O increases. O decreases. O remains the same. O More information is needed to answer this question.
Consider the following equilibrium system: Ag+(aq) + 2NH3(aq) D Ag(NH3)2+(aq) + energy If the equilibrium concentrations are as follows, what is the value of Keq? [Ag+] = 2.0M , [NH3] = 6.0 M , [Ag(NH3)2+] = 8.0M
The fictitious complex M(SCN)2 can be produced from an aqueous equilibrium in which the M2+ ion is mixed with the thiocyanate ion. A solution containing initial concentrations of M2+ and SCN- are 0.000100 M and 0.000300 M respectively has an equilibrium concentration of M(SCN)2 of 2.00 x 10-5 M. What are the equilibrium concentrations of the two starting ions and what is the value of the equilibrium constant? [M2+] = ___ x 10__ M [SCN-]= ___ x 10__ M Kc = ___ x 10 __

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry for Engineering Students

Chemistry

ISBN:

9781337398909

Author:

Lawrence S. Brown, Tom Holme

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS