# 6.2.3.6: The Arrhenius Law - Pre-exponential Factors

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The pre-exponential factor (\(A\)) is an important component of the Arrhenius equation, which was formulated by the Swedish chemist Svante Arrhenius in 1889. The pre-exponential factor is also known as the* frequency factor,* and represents the frequency of collisions between reactant molecules at a standard concentration. Although often described as temperature independent, it is actually dependent on temperature because it is related to molecular collision, which is a function of temperature.

## Temperature Dependence of Reactions

The units of the pre-exponential factor vary depending on the order of the reaction. In first order reactions, the units of the pre-exponential factor are reciprocal time (e.g., 1/s). Because the pre-exponential factor depends on frequency of collisions, it is related to collision theory and transition state theory.

\[ k = A e^{E_a/RT} \label{eq1}\]

The Arrhenius equation introduces the relationships between rate and \(A\), \(E_a\), and \(T\), where \(A\) is the pre-exponential factor, \(E_a\) is the activation energy, and \(T\) is the temperature. The pre-exponential factor, \(A\), is a constant that can be derived experimentally or numerically. It is also called the **frequency factor** and describes how often two molecules collide. To first approximation, the pre-exponential factor is considered constant.

When dealing with the collision theory, the pre-exponential factor is defined as \(Z\) and can be derived by considering the factors that affect the frequency of collision for a given molecule. Consider the most elementary bimolecular reaction:

\[A + A \rightarrow Product\]

An underlying factor to the frequency of collisions is the space or volume in which this reaction is allowed to occur. Intuitively, it makes sense for the frequency of collisions between two molecules to be dependent upon the dimensions of their respective containers. By this logic, \(Z\) is defined the following way:

\[Z = \dfrac{(\text{Volume of the cylinder}) (\text{Density of the particles})}{\text{time}}\]

Using this relationship, an equation for the collision frequency, \(Z\), of molecule \(A\) with \(A\) can be derived:

\[Z_{AA} = 2N^2_Ad^2 \sqrt{\dfrac{\pi{k_{b}T}}{m_a}}\]

A similar reasoning is used for bimolecular reactions that involve the collisions of \(A\) and \(B\)

\[A + B \rightarrow Product\]

for deriving the collision frequency, \(Z\) between \(A\) and \(B\).

\(Z_{AB} = N_AN_Bd^2_{AB} \sqrt{\dfrac{8{k_{b}T}}{\mu}}\)

Substituting the collision factor back into the original Arrhenius equation yields:

\[\begin{align*} k &= Z_{AB}e^{\frac{-E_a}{RT}} \\[4pt] &= N_A\, N_B\, d^2_{AB} \sqrt{\dfrac{8{k_{b}T}}{\mu}}\,e^{\frac{-E_a}{RT}}\end{align*}\]

This equation produces a rate constant with the standard units of (M^{-1} s^{-1}); however, on a molecular level, a rate constant with molecular units would be more useful. To obtain this constant, the rate is divided by \(N_A\,N_B\). This produces a rate constant with units (m^{3} molecule^{-1} s^{-1}) and provides the following equation:

\[k = Z_{AB} e^{\frac{-E_a}{RT}}\]

Divide both sides by \(N_AN_B\)

\[\dfrac{k}{N_AN_B} = d^2_{AB} \sqrt{\dfrac{8 k_b T}{\mu}}e^{\frac{-E_a}{RT}}\]

\(Z_{AB}\) becomes \(z_{AB}\):

\[\dfrac{Z_{AB}}{N{_A}N{_B }} = z_{AB}\]

Substituting back into the Arrhenius equation (Equation \ref{eq1}):

\[k = z_{AB}e^{\frac{-E_a}{RT}}\]

The pre-exponential factor is now defined within the collision theory as the following:

\[d^2_{AB} \sqrt{\dfrac{8{k_{b}T}}{\mu}}\]

\(A\) and \(Z\) are practically interchangeable terms for collision frequency. The derivations for \(Z\) often ignores the steric effect of molecules. For a reaction to occur, two molecules must collide in the correct orientation. Not every collision results in the proper orientation, and thus some do not yield a corresponding product. To account for this steric effect, the variable \(P\), which represents the probability of two atoms colliding with the proper orientation, is introduced. The Arrhenius equation is as follows:

\[k = Pze^{\frac{-E_a}{RT}}\]

The probability factor, \(P\), is very difficult to asses and still leaves the Arrhenius equation imperfect.

## Transition State Theory Pre-exponential Theory

The collision theory deals with gases and neglects to account for structural complexities in atoms and molecules. Therefore, the collision theory estimation for probability is not accurate for species other than gases. The transition state theory attempts to resolve this discrepancy. It uses the foundations of thermodynamics to give a representation of the most accurate pre-exponential factor that yields the corresponding rate. The equation is derived through laws concerning Gibbs free energy, enthalpy and entropy:

\[k = \dfrac{k_bT}{h} e^{\frac{\Delta S^o}{R}} e^{\frac{-\Delta H^o}{RT}}(M^{1-m})\]

Factor |
Type |
---|---|

A | Empirical |

\(d^2_{AB} \sqrt{\dfrac{8{k_{b}T}}{\mu}}\) |
Collision Theory |

\(\dfrac{k_bT}{h}\) | Transition State Theory |

The pre-exponential factor is a function of temperature. As indicated in Table 1, the factor for the collision theory and the transition state theory are both responsive to temperature changes. The collision theory factor is proportional to the square root of \(T\), whereas that of the transition state theory is proportional to \(T\). The empirical factor is also sensitive to temperature. As temperature increases, molecules move faster; as molecules move faster, they are more likely to collide and therefore affect the collision frequency, \(A\).

## Sources

- Atkins, Peter, and Julio De Paula.
**Physical Chemistry for the Life Sciences.**Alexandria, VA: Not Avail, 2006. - Chang, Raymond.
**Physical Chemistry for the Biosciences.**Sausalito, CA: University Science, 2005.

## Contributors and Attributions

- Golshani (UCD)