QUESTION: When the pink equilibrium solution formed from CoCl 2 was placed in a

Question

QUESTION: When the pink equilibrium solution formed from CoCl2 was placed in a hot water bath, the solution turned blue. When placed into an ice bath, it turned back to pink. Cite specific observation results to identify the forward reaction in this equilibrium as an exothermic, or as an endothermic process. Write an equation for this equilibrium depicting heat as a reactant or producr of the reaction.

ATTEMPT AT AN ANSWER: In a forward reaction, blue Co ions and water maolecules combine to form pink Co(H2O)6 ions (endothermic process) AND in a reverse reaction, pink Co(H2O)6 ions break into blue Co ions and water molecules (exothermic process).

I feel like I am 100% incorrect / incomplete. Can someone help me please?

Explanation / Answer

we know that

according to Le Chatlier principle

the equilibrium will shift in such a direction to counter the change

now

assume the reaction to be

CoCl42- ( blue) + 6 H20 ---> Co (H20)62- ( pink) + 4 Cl- + heat

now

hot water is added

it is nothing but heat is added to the equilibrium

now

according to Le chatlier principle

the equilibrium will shift in such a direction to decrease the heat

so

the equilibrium will shift to the left

it means the solution will turn blue

now

ice bath is added , means heat is reduced at the equilibrium

as a result

the equilibrium will shift in a direction to increase the heat

so

the equilirbium will shift to the right side producing more pink color

So

our assumption is correct

So

the forward reaction is exothermic as it produces heat

the equation is

CoCl42- ( blue) + 6 H20 ---> Co (H20)62- ( pink) + 4 Cl- + heat

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