Redox disequilibrium

Redox Disequilibrium is part of a free web series, GWB Online Academy, by Aqueous Solutions LLC.

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At low temperature many redox reactions are unlikely to achieve equilibrium. Lindberg and Runnells (1984) demonstrated the generality of this problem. They compiled more than 600 water analyses that provided at least two measures of oxidation state and calculated species distributions for each sample. They then computed redox potentials for the various redox couples in the analysis, using the Nernst equation. Their results showed that redox couples in a sample generally failed to achieve equilibrium with each other.

Before this idea was widely accepted, the common approach in geochemical modeling was to assume that all redox reactions reached equilibrium. The user sets a single value for the system oxidation state, or a “Master Eh,” which controls the distribution of species among different oxidation states.

A more realistic approach is to allow for redox disequilibrium by disabling one or more redox coupling reactions. All coupled redox reactions still reflect the Master Eh for the system. Disabled redox couples, though, behave independently.

Any number of redox coupling reactions can be disabled.

For any disabled couple, you can write out an electron transfer reaction and calculate the Nernstian Eh. Where redox equilibrium is not achieved, each disabled couple would have a distinct Nernstian Eh.

In this lab we will consider how to construct chemical models that account for redox reactions that are not in thermodynamic equilibrium. The GWB programs allow you to interactively control which redox couples are to be held in equilibrium and which are not.

Disabling the redox couple between Fe+++ and Fe++, for example, eliminates any provision for equilibrium between ferrous and ferric iron. Species Fe+++ is available as a new entry in the basis, which you can constrain independently from Fe++. Going to the Basis pane, you will find that you can now add Fe+++ to the basis list.

This feature is quite useful—and commonly necessary—for modeling natural waters. You will likely find yourself decoupling sulfide from sulfate, methane from carbonate, ammonium and nitrite from nitrate, As(V) from As(III), and so on.

Task 1: Chemical energy in natural waters

Microbes take advantage of the redox disequilibrium found in the natural environment to derive energy. Respiring microbes trap energy released when electrons liberated by an electron-donating reaction are taken up by an electron-accepting reaction.

The difference ΔEh between the Eh for the accepting and donating reactions is a measure in volts or mV of the energy released. The value is given as

where n is the number of electrons transferred and F is the Faraday constant. Reactions with positive ΔEh values release energy.

Double-click on file “microbe.sp8”. When SpecE8 opens, move to the Basis pane

The input describes the analysis of a hypothetical groundwater, assuming equilibrium with ferric hydroxide and a soil gas in which f CO2 = 10−2. Note that constraints are provided for the distribution of several elements across differing redox states.

To see why, open the Config → Redox Couples… dialog

Several redox pairs have been disabled.

Move to the Results pane and click , then click

In SpecE8's output file, check the Nernst Eh values for the following redox couples:

Which couple is the most energetically favorable as an electron-donating reaction? Which is the best at accepting electrons?

It is useful to list the redox potential for each couple so that they are arranged in decreasing order

Reactions at the top of the list are most favored in this environment to accept electrons, and those at the bottom most prone to donate them.

The best electron donor in this environment, then, would be CH3COO, while O2 is the best electron acceptor.

For each of the following metabolisms, determine ΔEh. Which metabolisms are favorable for microbes living in contact with this groundwater?

  • Oxidation of acetate by ferric iron
  • Oxidation of methane by molecular O2
  • Reduction of sulfate by ferrous iron
  • Oxidation of H2 by nitrate

In considering energy availability, it is helpful to remember that “electrons fall up!” In other words, if the overall reaction is to liberate energy, the donating half-reaction in a list ordered as shown must appear below the accepting half-reaction, to give a positive ΔEh.

We can set up a table with the redox potentials of our electron accepting and donating half-reactions arranged in descending order (horizontal and vertical orientations, respectively), as shown below

We used a spreadsheet to calculate redox potentials (ΔEh = EhaccEhdon) in this groundwater for every possible pair of electron donating and accepting half-reactions. We listed those with positve redox potentials in the table and highlighted them in green.

Taking a closer look at the metabolisms mentioned above, we can calculate a redox potential for acetotrophic iron reduction (the oxidation of acetate by ferric iron) as follows: 322 − (−230) = 552 mV.

Similarly, for the oxidation of methane by molecular O2, the redox potential is 836 − (−187) = 1023 mV.

For the reduction of sulfate by ferrous iron, the redox potential is −126 − 322 = −448 mV.

Finally, the redox potential for the oxidation of H2 by nitrate depends on what form of nitrogen the nitrate is reduced to. If the nitrate is reduced to nitrite, the redox potential is 481 − (−199) = 680 mV. If the nitrate is reduced to ammonium, though, the redox potential is 443 − (−199) = 642 mV.

The examples are highlighted in red below

All of the above-mentioned metabolisms would be favorable for microbes in contact with this groundwater, except for the reduction of sulfate by ferrous iron, for which we calculated a negative redox potential.


Craig M. Bethke and Brian Farrell. © Copyright 2016–2021 Aqueous Solutions LLC. This lesson may be reproduced and modified freely to support any licensed use of The Geochemist's Workbench® software, provided that any derived materials acknowledge original authorship.


Bethke, C.M., 2008, Geochemical and Biogeochemical Reaction Modeling. Cambridge University Press, New York, 547 pp.

Bethke, C.M., B. Farrell, and M. Sharifi, 2021, The Geochemist's Workbench®, Release 15: GWB Essentials Guide. Aqueous Solutions LLC, Champaign, IL, 215 pp.

Lindberg, R.D. and D.D. Runnels, 1984, Groundwater redox reactions: an analysis of equilibrium state applied to Eh measurements and geochemical modeling. Science 225, 925–927.

Comfortable with redox disequilibrium?

Move on to the next topic, High-salinity Fluids, or return to the GWB Online Academy home.