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

Explanation:

Le Chatelier, in his principle explains changes that happens to a system at equilibrium. These principle states that;

If a dynamic equilibrium of a system is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change to reestablish an equilibrium. If a chemical reaction is at equilibrium and experiences a change in pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to offset the change.

In this problem the conditioned changed, is the temperature. To understand how temperature changes affect equilibrium conditions, the sign of the reaction enthalpy must be known.

The system is exothermic as mentioned in the question already.

Adding heat - Increasing the temperature.

If the temperature is increased, then the position of equilibrium will move so that the temperature is reduced again. Suppose the system is in equilibrium at 400°C, and the temperature is increased 700°C. To cool down, it needs to absorb the extra heat added. In the case, the back reaction is that in which heat is absorbed. The position of equilibrium therefore moves to the left. The new equilibrium mixture contains more reactants and less products.

Remving heat - Decreasing the temperature

The equilibrium will move in such a way that the temperature increases again. Suppose the system is in equilibrium at 700°C and the temperature is reduced to 500°C. The reaction will tend to heat itself up again to return to the original temperature by favoring the exothermic reaction. The position of equilibrium will move to the right with more reactants converted into products at the lower temperature: