By making reference to your observations, explain whether the equilibrium studied in Part C is exothermic or endothermic, and explain how temperature shifts the equilibrium of the reaction you are studying. Show reactions in both cases (when the system was heated and when it was cooled).

PART C: Investigation of the Effect of Changing Temperature on a System at Equilibrium Cobalt (II) salts form complex compounds readily. The pink aqueous solutions of Co (II) salts are characteristic of the complex ion [Co(H2O)6]2+ in which the Co2+ ion is bonded to six water molecules in an octahedral arrangement. If Clions are present in sufficient concentration, they will compete effectively with the water molecules for bonding to the Co2+ to form a deep blue solution of CoCl42. The unbalanced reaction is: [Co(H2O)6]2+(aq)+Cl(aq)?? Experimental Procedure: 1. In a small beaker, 10mL of 0.1MCo2+ solution is mixed with 9mL of concentrated HCl to produce a violet solution (halfway between the original pink and bright blue). If necessary, the color was adjusted by adding distilled water or concentrated HCl a drop at a time. 2. The violet solution is then divided into three large test tubes. One is reserved at room temperature for comparison; the second is placed in an ice bath; and the third is placed in a beaker of boiling water. Observe any color changes that occur. 3. The process is then determined if color changes are reversible