Integrated Rate Law

Integrated rate law is a fundamental concept in chemical kinetics that describes the concentration of reactants or products over time during a chemical reaction. It provides a mathematical relationship between the concentration of a reactant or product and time, thereby allowing for the determination of reaction kinetics and rate constants.

Zero-Order Reaction Rate

In a zero-order reaction, the reaction rate is independent of the concentration of the reactant. The integrated rate equation for a zero-order reaction is:

[A]_t = −k.t+[A]₀

First-Order Reaction Rate

In a first-order reaction, the reaction rate is directly proportional to the concentration of the reactant. The integrated rate equation for a first-order reaction is:

ln[A]_t = −k.t +ln[A]₀

Second-Order Reaction Rate

In a second-order reaction, the reaction rate is proportional to the square of the concentration of the reactant. The integrated rate equation for a second-order reaction is:

1/[A]_t= k.t+1/[A]₀

​​Where,

• [A]_t is the concentration of the reactant at time t,
• k is the rate constant,
• [A]₀ is the initial concentration of the reactant.

Read More about Integrated Rate Laws.

Half-Life of a Reaction

In chemical kinetics, the concept of half-life represents the time required for the concentration of a reactant to decrease to half of its initial value. The half-life is particularly useful in understanding the kinetics of first-order reactions, where the reaction rate is directly proportional to the concentration of the reactant.

For a first-order reaction, the relationship between the half-life (t_1/2), the rate constant k, and the initial concentration of the reactant [A₀]can be expressed as

t_1/2=0.693/k

This equation indicates that the half-life of a first-order reaction is inversely proportional to the rate constant k. As the rate constant increases, the half-life decreases, indicating a faster rate of reaction.

Chemical Kinetics is a part of physical chemistry that focuses on the rate of chemical reactions and the reasons behind them. It involves figuring out the speed and details of chemical reactions, studying the factors that affect how fast they happen, and how molecules interact during these changes.

This field is important in various scientific areas, from improving industrial processes to understanding complicated reactions in biological systems. By focusing on how molecules interact, chemical kinetics helps us to understand the complex movements of atoms and molecules in the world of chemistry.