Scoring Scheme: 3-2-1-1 Part IV. The chemical system in the study of the temperature effects on equilibria contains two complex ions of cobalt: Co(EtOH)2CI2(aq)(blue) + 6 H2O 2 EtOH + 2 Cl- + Co(H2O)62+(red-pink) + H2O(l) + heat. As written, the chemical system is exothermic. How does adding and removing heat from the system affect equilibrium?

Adding the heat to the system will shift the reaction in backward direction that is towards reactant side.

Removing the heat from the system will shift the reaction in forward direction that is towards product side.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For exothermic reaction:

A + B → C + Heat

Treat heat as a product on removing the product from equilibrium will shift the equilibrium in forward direction to make more product and to reestablish the equilibrium.

Treat heat as a product ,on adding the product on an equilibrium will shift the equilibrium in backward direction to make more reactant and to reestablish the equilibrium.

For Endothermic  reaction:

A + B + Heat → C

Treat heat as a reactant and on removing the reactant from equilibrium will shift reaction in backward direction to make more reactant and to reestablish the equilibrium.

Treat heat as a reactant and on adding the reactant on an equilibrium will shift the reaction in forward direction to make more reactant and to reestablish the equilibrium.

Now according to question the given  chemical reaction is an exothermic reaction, so on "

Adding the heat to the system will shift the reaction in backward direction that is towards reactant side.

Removing the heat from the system will shift the reaction in forward direction that is towards product side.

- both b and d.

-since b and d are the closest coastlines then that makes it the most affected.

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