What defines a chemical reaction's rate?

The rate of a chemical reaction is fundamentally defined by the speed at which reactants are consumed or products are formed. This is a core concept in chemistry, as it quantifies how quickly the transformation between reactants and products takes place over time. The measurement of reaction rate often involves monitoring changes in concentration, pressure, or volume, providing a clear indication of how fast the reaction is progressing.

In addition, several factors can affect this rate, such as temperature, presence of a catalyst, and the identity of reactants. While temperature can influence molecular collisions and energy levels, and catalysts can speed up reactions without being consumed, these factors are secondary to the fundamental definition of the reaction rate itself. The type of reactants can also play a role in determining the reactivity and rate; however, they do not define it. The core essence of the reaction rate remains rooted in the changes of the reactants and products through time.