In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2 (aq) is pink and CoCl42-(aq) is blue. At

Question

In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCl42-. Co2 (aq) is pink and CoCl42-(aq) is blue. At Low Temperature the pink color pre-dominates. At High Temperature the blue color is strong. If we represent the equilibrium as:
CoCl4^2-(aq) <–> Co2+(aq) + 4Cl-(aq)
We can conclude that:___.
1. This reaction is:___.
A. Exothermic
B. Endothermic
C. Neutral
2. When the temperature is decreased the equilibrium constant, K:____.
A. Increases
B. Decreases
C. Remains the same.
3. When the temperature is decreased the equilibrium concentration of Co2:______.
A. Increases
B. Decreases
C. Remains the same.

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Sapo 4 years 2021-08-04T02:17:09+00:00 1 Answers 221 views 0

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  1. minhkhang
    -1
    2021-08-04T02:19:02+00:00
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    Answer:

    1. This reaction is (A) Exothermic .

    2. When the temperature is decreased the equilibrium constant, K: (A) Increases

    3.When the temperature is decreased the equilibrium concentration of Co2: (A) Increases

    Explanation:

    CoCl4^2-(aq) <--> Co_2+(aq) + 4Cl^-(aq)

    1. The pink color predominates at low temperatures, indicating that the commodity is preferred.

    This is a reaction that is exothermic.

    2. As the decrease in the temperature , the equilibrium constant , K ;

          equilibrium constant = \frac{product}{reactant} =\frac{[CO^2^+][Cl^-^4]}{CoCl^2^-_4}

    As the temperature drops, the concentration ofCl^- and CO^2^+ rises, and K rises as well , thus it increases .

    3. The equilibrium concentration of CO^2^+ decreases as the temperature decreases:

    When the temperature is lowered, the equilibrium shifts to the right , that is it increases.

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