What is a First-Order Reaction?
First-Order Reaction is a chemical process where the rate of transformation of a substance is directly proportional to its concentration. As the concentration decreases, the rate of the reaction diminishes at a corresponding rate. These reactions are vital in various natural and artificial phenomena, like radioactive decay and specific chemical changes.
Examples of First-Order Reactions
Some examples of the First-Order Reactions are,
- Radioactive Decay: Isotopes such as carbon-14 decay at a rate proportional to their concentration.
- Chemical Decomposition: Decomposition of hydrogen peroxide into water and oxygen follows first-order kinetics.
Some other examples of first order reactions are,
- 2N2O5 → O2 + 4NO2
- 2H2O2 → 2H2O + O2
First-Order Reactions
First-Order Reactions describe chemical processes where the transformation rate directly depends on the concentration of a single substance. We define first-order reactions as reactions where the initial concentration of the initial element doubles then its rates also doubles.
In this article, we will learn about, First-Order Reaction Definition, Differential Rate Law for the First-Order Reaction, Integrated Rate Law for a First-Order Reaction, a Graphical Representation of a First-Order Reaction, Pseudo First-Order Reaction, and others in detail.
Table of Content
- What is a First-Order Reaction?
- Differential Rate Law for a First-Order Reaction
- Integrated Rate Law for a First-Order Reaction
- Graphical Representation of a First-Order Reaction
- Pseudo First-Order Reaction