The following equation shows the equilibrium reaction between twocobalt complexes: Co(H2O)6 2+ (aq) + 4Cl1- (aq) <-------->CoCl4 2- (aq) + 6H2O pink blue Equilibrium is established and theresulting solution is purple. When this solution is heated it turnsblue. What are the implications of this result? Answer a.Thereaction is exothermic as written b.The reaction is endothermic aswritten c. Heat was not the cause of the color change. d. Coolingthe solution will increase the value of Kc

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Studying the (CoCl4)^2 / (Co(H2O)6)^2+ Equilibrium.
-color of original equilibrium
dark-blue
-color change after addition of distilled water
lighter shade of dark blue
- color change after addition of 12M HCl
sky-blue
- color change after addition of distilled waster
lavender
-color change after heating mixture
light blue
- color change after cooling mixture
darker shade of purple.

(CoCl4)^2- (aq, blue) + 6H2O (l)= (Co(H2O)6)^2+ (aq, pink)+ 4Cl^-(aq)

6) Use Le Chateliers principle to account for the color change youobserved when you added 12M HCl to the equilibrium mixture
7)Based on your answer to question 6 , would you expect to observethe same color change if you added a saturated NaCl solutioninstead of adding the 12M HCl? Explain.
8) After the equilibrium mixture was cooled in the ice-water bathwhat was the predominant cobalt(II) species present in thesolution, (CoC14)^2 or (Co(H20)6)^2+. explain.
9) Based on your answer to question 8, is the forward reactionexothermic or endothermic? Rewrite the equilibrium reaction toinclude the heat term.

Tetrachlorocobalt (II) ion reacts with water to form hexaaquacobalt (II) ion according to the following net ionic equation:
[CoCl₄]²^-(aq, blue) + 6 H₂O(l) <=> [Co(H₂O)₆]²⁺(aq, pink) + 4 Cl^-(aq)

(A) A student doing this experiment placed a test tube containing a blue equilibrium mixture in an ice-water bath. The solution turned pink. When the student removed the test tube from the ice-water bath and placed it in the hot water bath, the solution turned blue. Is the forward reaction exothermic or endothermic? Give complete explanation.

(B) What change do you observe when you add concentrated hydrochloric acid, HCl, solution. HCl undergoes dissociation according the following equation: Give complete explanation.

HCl(aq) â H⁺(aq) + Cl^-(aq)

(C) What experimental evidence do you have that the equilibrium is affected by the addition of water. Give complete explanation.

Which of the following actions will cause the equilibrium to shift such that the concentration of NOgas will increase?

2NO(g) + 2H2(g) ? N2(g)+2H2O+heat

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Which of the following actions will cause the equilibrium to shift such that the concentration of gas will increase?

Decrease the concentration of N2(g)

Increase the concentration of H2O(g)

Increase the concentration of H2(g)

Lower the reaction temperature

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Part B