Most chemical reactions end when the number of conductors ends. Some processes are not completed. The fact that this occurs can be explained by the reversibility of the reaction.
After forming the products, they again form the original reagents. If certain modifications are not made, these reactions will not come to an end. They tend to reach the chemical balance.
Chemical equilibrium is represented by inverse arrows: ↔
Be the generic reaction:
V1 and V2 are the speeds
At equilibrium, concentrations A, B, C, D are constant but not necessarily equal.
Reversible reaction It is one that occurs simultaneously in both directions. At the same time, reagents turn into products and products turn into reagents.
In the chart below, the conductors are represented by B and the products by A.
At the beginning of the reaction, there are a lot of reagents. As time goes on, this amount decreases and so does the speed.
Meanwhile, at the beginning of the reaction, there are no products, the amount is zero. In the course of the reaction, products are formed, the initial velocity is zero and increasing until it equals the reactant velocity.
At this time, the velocities will remain equal and constant. The concentrations will also be constant. When product and reagent speeds reach this point, we say that the reaction is in equilibrium.
We can classify the equilibria according to the phases of the substances involved in the chemical reaction.
It is one where all substances are in the same phase (physical state). They usually occur in gaseous and aqueous systems. Examples:
It is one where substances are in different phases. Usually involve solid and liquid substances. Examples: