Question

Explain Le Châtelier's principle. How can this principle help us maximize the yields of reactions?

Short answer

Le Châtelier's principle states that if a system at equilibrium is disturbed, the system will adjust to minimize that disturbance. The principle is applied to maximize the yields of reactions by manipulating the conditions of the reaction, such as temperature, pressure, and concentration to 'force' the reaction towards producing more of the desired product.

Step-by-step solution

Understanding of Le Châtelier's Principle

Le Châtelier's principle states that if a dynamic equilibrium is disturbed by changing conditions, the system adjusts to restore the equilibrium. In the context of chemical reactions, it means if any change is made to a system in equilibrium, such as temperature, pressure, or concentration changes, the system will react to relieve the change.

Working Mechanism of Le Châtelier's Principle

To illustrate this, consider a system in chemical equilibrium, and then one of the reactants' concentration is increased. According to Le Châtelier's principle, the system will react by consuming the added reactant, shifting the equilibrium towards the 'product' side of the reaction. Similarly, if a product is removed from the system, the equilibrium will shift to replace the lost product.

Application of Le Châtelier's Principle in Maximizing Yields

The principle is widely used in industry to increase the yield of reactions. By manipulating the factors under control, like temperature, pressure, and concentration, it's possible to 'force' the reaction to produce more of the desired results. For instance, if a reaction releases heat (exothermic), it can be shifted toward the products by cooling the system. Similarly, in a reaction where reducing pressure favors the formation of the product, using a large vessel can increase the yield. Hence, understanding and manipulating the equilibrium conditions allows us to maximize yield.