Zero-Order Reaction
| Formula / Notation | rate = k |
|---|---|
| Also Known As | Zero-order kinetics, zero-order rate law, concentration-independent reaction |
What is Zero-Order Reaction?
A zero-order reaction is a reaction whose rate is independent of the concentration of the reactant(s). The rate is constant and equal only to the rate constant k. This occurs when a reaction is limited by something other than reactant concentration, such as catalyst surface area, enzyme concentration (when fully saturated), or light intensity. As the reaction proceeds, concentration decreases linearly with time.
Formula & Notation
Other Names / Synonyms: Zero-order kinetics, zero-order rate law, concentration-independent reaction
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A zero-order reaction is a reaction whose rate is independent of the concentration of the reactant(s). The rate is constant and equal only to the rate constant k. This occurs when a reaction is limited by something other than reactant concentration, such as catalyst surface area, enzyme concentration (when fully saturated), or light intensity. As the reaction proceeds, concentration decreases linearly with time.
Understanding enzyme kinetics (Vmax in Michaelis-Menten = zero-order). Drug release from controlled-release formulations. Heterogeneous catalysis analysis. Surface reaction kinetics. Pharmaceutical dosing calculations.
Conceptual classification — safety depends on specific reaction. Zero-order reactions may proceed at a constant rate even as reactant is depleted — important consideration in industrial reactor safety.
The formula or notation for Zero-Order Reaction is: rate = k