Question

What are the real-world applications of Le Chatelier

Answer 1

One easy to understand example is the equilibrium that exists in our blood between water, carbon dioxide and carbonic acid. The equation for this reaction is H₂O + CO₂ <==> H₂CO₃.

In our blood, near our cells, where the concentration of CO2 is relatively high, the forward reaction produces carbonic acid, binding up the CO₂ that is a waste product of cellular respiration. In the lungs, where the concentration of CO₂ is relatively lower, the reverse reaction occurs, breaking up the carbonic acid and creating carbon dioxide, which we exhale.

The cooling of food with refrigerators, along with means of food preservation that do not involve changes in temperature, maintains chemical equilibrium in the foods and thereby prevents or at least retards spoilage. Even more important is the maintenance of equilibrium in reactions between hemoglobin and oxygen in human blood.

The cooling of food in refrigerators or preservating food with preservatives without changing the temperature also needs this principle. The equilibrium has to be maintained to keep food from spoilage.

Alse the equilibrium in the reaction between hemoglobin and oxygen in the blood is maintaines by the same principle.

It is the main feature of any phase change reaction such as liquid <=>vapour or ice <=> water. Also in many manufacturing processes in the chemical industries such as in the manufacturing of Ammonia which is called the Haber's Process.