Reaction Kinetics Concept Map


Reaction kinetics is the study of how fast chemical reactions occur and the factors that affect their rates.


The rate of reaction is defined as the change in concentration of reactants or products over time.


Several factors affect the rate of a chemical reaction, including:

• Temperature


• Concentration


• Catalysts


• Surface area


• Pressure

The reaction order refers to the exponent of the concentration term in the rate equation.

• Zero-order reactions


• First-order reactions


• Second-order reactions

The rate law is an expression that relates the rate of a reaction to the concentrations of the reactants raised to their respective orders.

• Rate = k[A]^m[B]^n

Reaction mechanisms describe the sequence of steps that occur during a chemical reaction.

• Elementary steps


• Reaction intermediates


• Rate-determining step

Catalysts are substances that increase the rate of a chemical reaction without being consumed in the process.

• Heterogeneous catalysis


• Homogeneous catalysis


• Enzymatic catalysis

Reaction kinetics is a critical aspect of chemistry that helps us understand how chemical reactions occur and how they can be controlled. Understanding the factors that affect reaction rates and the mechanisms by which reactions occur is essential for developing new materials and improving existing processes.