A secondary current distribution model considers:

- Ohm’s law resistance, and
- kinetic charge-transfer resistance

while resistance related to concentration variations is ignored. Beginning with the equations given in Modeling porous electrodes: Part 1, the following can be written:

Eq 1 is conservation of charge; Eq 2 is some expression of electrochemical reaction kinetics; and Eqs 3 & 4 are Ohm’s law for the solid and liquid phases. The boundary conditions are such that a current density of *I* is being produced by the electrode. The liquid phase potential *φ*_{2} is arbitrarily set to 0 V at x = 0. The specific expression for the electrode kinetics (Eq 2) needs to be specified. The concentration-independent Butler-Volmer expression can be used:

The left hand side of this expression is the transfer current, with units of A/cm^{3}, and gives the amount of electrochemical reaction occurring at any point. The right hand side has two components: the anodic and cathodic kinetic terms. The downside of the Butler-Volmer equation is its complexity. Finding an analytical solution to the above set of differential equations requires a more simplified kinetic expression. One possible simplification is to assume the overpotential (*φ*_{1 }– *φ*_{2}) is highly negative. This means only the cathodic term in the Butler-Volmer equation need be considered:

The right hand side of this expression is a form of the Tafel equation. (An analogous anodic form can be used when overpotential is highly positive.) Another possible simplification is to assume the overpotential (*φ*_{1} – *φ*_{2}) is small. In this case both anodic and cathodic terms are important. Substituting the first two terms of a Taylor series for the exponentials results in:

This linear kinetic expression is valid only at low currents. Which approximation of the kinetic expression is appropriate depends on the conditions of interest. Choosing the following values for physical parameters:

- electrode area per volume,
*a*= 23,300 cm^{-1} - transfer coefficients,
*α*_{a}=*α*_{c}= 0.5 - exchange current density,
*i*_{0}= 2 x 10^{-7}A/cm^{2} - current density,
*I*= 0.1 A/cm^{2} - length,
*L*= 1 cm - electrolyte conductivity,
*κ*= 0.06 S/cm - electrode conductivity,
*σ*= 20 S/cm

we assume that the Tafel approximation for kinetics will be valid, because the current density is much larger than the exchange current density. Solving the set of equations 1-4 for both Tafel and linear kinetics gives the results below:

The Tafel kinetic expression predicts that current exchange from liquid to solid phases (ionic current to electronic current) will be concentrated near x = 0, the location closest to the counter electrode. There (*φ*_{1} – *φ*_{2}) will be near 300 mV, falling away further into the electrode. In contrast, the linear kinetic expression predicts a more even exchange of current through the electrode, and much higher values of (*φ*_{1} – *φ*_{2}). This is because the linear expression is a softer function of overpotential than the exponential one. The Tafel approximation is clearly the more appropriate in this case because (*φ*_{1} – *φ*_{2}) » RT/F which is 25.7 mV at room temperature.

Plotting the transfer current di_{2}/dx shows that in reality the electrochemical reaction is concentrated in the front 10% of the electrode. Linear kinetics tend to result in more uniform current distributions, but for this to be the case *i*_{0} > *I* will need to hold.