How does equilibrium relate to reaction rates?

Equilibrium relates to reaction rates as it is the point where the rates of the forward and reverse reactions are equal.

In a chemical reaction, substances (reactants) are transformed into different substances (products). This process can often occur in both directions, meaning the reactants form products, but the products can also revert back to the original reactants. The rate at which these transformations occur is known as the reaction rate. When the rate of the forward reaction (reactants forming products) equals the rate of the reverse reaction (products forming reactants), the reaction is said to be in a state of equilibrium.

Equilibrium does not mean that the reaction has stopped. Instead, it means that the concentrations of the reactants and products have reached a balance and are no longer changing. This is because the rate at which the reactants are being consumed is equal to the rate at which they are being produced from the products. Similarly, the rate at which the products are being formed is equal to the rate at which they are reverting back to reactants.

The position of equilibrium can be influenced by changes in conditions such as temperature, pressure, or concentration. For example, if the concentration of a reactant is increased, the rate of the forward reaction will initially increase, disrupting the equilibrium. However, over time, the rates of the forward and reverse reactions will adjust, and a new equilibrium will be established.

In summary, equilibrium is a dynamic state where the forward and reverse reaction rates are equal, resulting in constant concentrations of reactants and products. Understanding this concept is crucial in predicting how changes in conditions can shift the position of equilibrium and influence the outcome of a reaction.