Half-Life of First-Order Reaction
It is the time taken for the concentration of a reactant to reduce to half its initial value. First-order reactions exhibit a constant half-life, irrespective of the initial concentration of the reactant. The half life of the reaction is represnted as
t1/2 = ln 2 /k
Now, ln 2 = 0.693
t1/2 = 0.693 /k
Where
- t 1/2 Represnts Half Life
- k Represents Rate Constant
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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