The following equation shows the equilibrium reaction between two cobalt complex

Question

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

Explanation / Answer

n the direction that you have written the equilibrium: CoCl4 2-(Blue) + 6H2O(l) => Co(H2O)6 2+(pink) + 4Cl-(aq) & HEAT released it is an exothermic reaction , so the sign of ?H for the reaction is negative favored directions are ones that release energy, that is your equation as you wrote it, so pink would be favored adding excess heat to the equilib will shift it back to the left to rid us of the added heat... into blue, as would adding excess Cl- removing heat to the equilib will shift it to the right to restore lost heat... into pink, as would removing Cl- by adding Ag+ ions

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