Dynamic equilibrium is a state where the ratio of products to reactants remains constant due to the equal rates of forward and reverse reactions. Reversible reactions favor both reactants and products, and Le Châtelier’s Principle explains how changes in variables can shift the equilibrium position. It is linked to the rate of chemical reactions and can be thought of as two distinct reactions settling into equilibrium.
Dynamic equilibrium is a state in which the ratio of products to reactants in a chemical reaction remains constant. The constant ratio of products to reactants does not mean that the reaction is completely static or that the reactants do not react to form products and vice versa. This type of equilibrium is “dynamic” because there is a constant exchange between reactants and products as the reaction continues to consume reactants to form products and consume products to form reactants. The ratio of products to reactants does not change because the rate of the reaction favoring the products and the rate of the reaction favoring the reactants are the same. The rates themselves cause no change in the product-reactant ratio over time, so the reaction is said to be at equilibrium or steady state.
A reaction must be reversible if it is to achieve any form of dynamic equilibrium. A reversible reaction is a chemical reaction in which the reactants can react to form products which can react with each other to form the original reactants. Reversible reactions often favor both reactants and products, so while it’s possible for the reaction to go both ways, the reaction tends to produce more of one than the other. This means that the “position” of a dynamic equilibrium can result in a greater amount of both products and reactants. An “equilibrium constant” is used to describe and make calculations relating to the equilibrium position of a given reaction.
Many different changes in the variables related to a chemical reaction can shift the position of the dynamic equilibrium. Le Châtelier’s Principle provides a general way for chemists to think about changes in dynamic equilibrium. The principle states, in general, that when an equilibrium reaction is elicited, the reaction will move in the direction that minimizes the change in equilibrium. If more reactant is added to an equilibrium reaction, the equilibrium will shift towards products and reach a new equilibrium based on the new reactant and product concentrations.
Dynamic equilibrium is intrinsically linked to the rate at which chemical reactions occur. A dynamic equilibrium can be thought of as two distinct chemical reactions. One occurs in the forward direction, with the reactants forming the products, while the other occurs in the reverse direction, with the products of the first reaction forming the reactants. Eventually, these two reactions settle into an equilibrium based on their equilibrium constants. In equilibrium, the forward reaction and the reverse reaction occur at the same rate.
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