Pre-exponential factor

This article needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. Find sources: "Pre-exponential factor" – news · newspapers · books · scholar · JSTOR (June 2018) (Learn how and when to remove this message)

In chemical kinetics, the pre-exponential factor or A factor is the pre-exponential constant in the Arrhenius equation (equation shown below), an empirical relationship between temperature and rate coefficient. It is usually designated by A when determined from experiment, while Z is usually left for collision frequency. The pre-exponential factor can be thought of as a measure of the frequency of properly oriented collisions. It is typically determined experimentally by measuring the rate constant ${\displaystyle k}$ at a particular temperature and fitting the data to the Arrhenius equation. The pre-exponential factor is generally not exactly constant, but rather depends on the specific reaction being studied and the temperature at which the reaction is occurring.^[1]

$${\displaystyle A={\frac {k}{e^{-{\frac {E_{a}}{RT}}}}}=ke^{\frac {E_{a}}{RT}}}$$

The units of the pre-exponential factor A are identical to those of the rate constant and will vary depending on the order of the reaction. For a first-order reaction, it has units of s⁻¹. For that reason, it is often called frequency factor.

According to collision theory, the frequency factor, A, depends on how often molecules collide when all concentrations are 1 mol/L and on whether the molecules are properly oriented when they collide. Values of A for some reactions can be found at Collision theory.

According to transition state theory, A can be expressed in terms of the entropy of activation of the reaction.

• IUPAC Gold Book definition of pre-exponential factor

This chemical reaction article is a stub. You can help Wikipedia by expanding it.

• v
• t
• e