First-order kinetics describes a reaction rate that is directly proportional to the concentration of a single reactant, meaning that as the concentration decreases, the rate of reaction decreases linearly. This kinetic model is commonly used to describe processes such as radioactive decay and the elimination of drugs from the body, where the rate constant remains unchanged over time.

First-order Kinetics

First-order kinetics

Reaction rate is a measure of how quickly reactants are converted into products in a chemical reaction, influenced by factors such as temperature, concentration, surface area, and catalysts. Understanding reaction rates is crucial for controlling industrial processes, optimizing reaction conditions, and studying reaction mechanisms in chemistry.

reaction rate

concentration of a single reactant

The rate of reaction measures how quickly reactants are converted into products in a chemical reaction, influenced by factors like concentration, temperature, and catalysts. Understanding this rate is crucial for optimizing industrial processes, controlling environmental impacts, and studying biological systems.

rate of reaction

Radioactive decay is the process by which an unstable atomic nucleus loses energy by emitting radiation, leading to the transformation of the original atom into a different element or a different isotope of the same element. This process occurs spontaneously and is characterized by a specific half-life, which is the time it takes for half of the radioactive atoms in a sample to decay.

radioactive decay

elimination of drugs

The rate constant is a proportionality factor in the rate equation of a chemical reaction, reflecting how quickly a reaction proceeds under specific conditions. It is influenced by factors such as temperature and the presence of a catalyst, and its units vary depending on the order of the reaction.

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