Metals and Equilibria: Dynamic Equilibrium

Dynamic equilibrium is a state reached in a reversible reaction where the forward and reverse reactions take place at the same rate. Therefore, the concentration of the reactants and products does not change over time.
Understand that equilibrium is possible only in a closed system where no reactants or products can escape or be added.
A reversible reaction is indicated by the use of forward and reverse arrows instead of the usual one-way arrow.
The equilibrium symbol is used (double arrow: ⇌) to indicate that a reaction can proceed in both the forward and reverse directions.
In terms of chemical equations, a reversible reaction could be represented as A + B ⇌ C + D.
Learning the concept of Le Chatelier’s principle, which states that if a dynamic equilibrium is disrupted by changing the conditions, the position of equilibrium moves to counteract the change, is also necessary.
For instance, if the concentration of a reactant is increased, the equilibrium will shift to decrease it (making more product). Conversely, decreasing the concentration of a product or increasing the temperature (for an endothermic reaction) will shift the equilibrium to make more of that product.
Also, note that changing the temperature or pressure will have an impact on the equilibrium of a reaction. For high pressure, the reaction will favour the side with fewer gaseous molecules and for high temperature, it will favour the endothermic reaction.
It’s essential to familiarise yourself with diagrams and graphs that represent the changes in concentration over time in a reversible reaction to understand the concept of dynamic equilibrium.
Revisit and understand examples of real-world scenarios where dynamic equilibrium is crucial, such as the Haber-Bosch process for ammonia synthesis or the production of methanol, as these are often used in questions.