Half-Life Time (t1/2) for Zero Order Reaction
For a zero-order reaction, the half-life (t1/2) is the time required for the concentration of the reactant to decrease to half of its initial value. The half-life for a zero-order reaction can be calculated using the following formula:
It is the time for half conversion of reactants into products.
t½ = [A]o/2k
Where,
- t1/2 is the half-life of the reaction,
- [A]o is the initial concentration of the reactant, and
- k is the rate constant of the zero-order reaction.
Differential and Integrated form of Zero Order Reaction
In the differential form, the rate of change of the concentration of the reactant with respect to time (d[A]/dt) is equal to the negative of the rate constant (−k) multiplied by the concentration of the reactant ([A]). This can be expressed as:
d[A]/dt = -k
To derive the integrated form of the zero-order reaction, we can integrate the differential rate equation. Assuming the initial concentration of the reactant ([A]o) is known, the integrated form is:
[A] = [A]o – kt
Where:
- [A] is the concentration of the reactant at time t,
- [A]o is the initial concentration of the reactant,
- k is the rate constant of the zero-order reaction, and
- t is the reaction time.
Zero Order Reaction
Zero Order Reaction is a type of chemical reaction where the reaction rate does not change with variations in the concentration of the reactants. In such reactions, the concentration rates remain constant over time. This type of reaction is characterized by the fact that the concentration of the reactants does not influence the reaction rate.
In this article, we look into What the order of the reaction is, what the zero-order reaction is, definition characteristics, rate law expression, etc.
Table of Content
- What is Order of Reaction?
- What is a Zero Order Reaction?
- Characteristics of Zero Order Reactions
- Rate Law for Zero Order Reactions
- Half-Life Time (t1/2) for Zero Order Reaction
- Zero, First and Second-Order Reactions
- Significance of Zero Order Reactions
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