In an aqueous chloride solution cobalt(II) exists in equilibrium with the comple

Question

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl_4^2-.Co^2+ (aq) is pink and CoCl_4^2-(aq) is blue. If we represent the equilibrium as: Co^2+ (aq) + 4Cl^- (aq) CoCl_4^2-(aq) We can conclude that: This reaction is: Exothermic Endothermic Neutral More information is needed to answer this question. When the temperature is increased the equilibrium constant, K: Increases Decreases Remains the same More information is needed to answer this question. When the temperature is increased the equilibrium concentration of CoCl_4^2-: Increases Decreases Remains the same More information is needed to answer this question.

Explanation / Answer

As temperature increases, blue color becomes strong, ie. more CoCl42- is formed, ie. High temperature favors forward reaction. The reaction is endothermic.

Kc = ([CoCl4-2)]/([Cl-]4[Co+2]), As temperature increases, concentration of CoCl42- increases. Hence Kc increases.

An increases in temperature favors endothermic reaction, ie concentration of CoCl42- increases.

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