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

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) in blue. If we represent equilibrium as: Co^2- (aq) + 4CI^-(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 decreased the equilibrium constant, K: Increases Decreases Remains the same More information is needed to answer this question. When the temperature is decreased the equilibrium concentration of Co^2-? Increases Decreases Remains the same More information is needed to answer this questions

Explanation / Answer

1. The answer is B) Endothermic because at high temperature CoCl4^2- is produced more i.e heat is used by the reaction

2.The answer is B) Decrease because the equilibrium expression is K = [CoCl4^2-]/[Co^2+][Cl^-]^4,as the temperature decreases[ CoCl4^2-] decrease and K decrease

3.The answer is A) Increase because as temperture decrease the reaction proceed reverse

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