Omni Calculator logo

Nernst Equation Calculator

Created by Bogna Szyk
Reviewed by Steven Wooding
Last updated: Jun 05, 2023

This Nernst equation calculator presents the fundamental formula of electrochemistry — the Nernst equation, also known as the cell potential equation. It is a formula that allows you to calculate the reduction potential of a half-cell or full cell reaction. If you don't know what the reduction potential is, don't worry — we will explain all the terms, describe in detail how to calculate the cell potential, and finish with a Nernst equation example that best presents its application.

What is the reduction potential?

The reduction potential of a half-cell or full-cell reaction is also called the redox potential or oxidation/reduction potential. It measures the tendency of molecules (or atoms, ions, etc.) to acquire electrons and hence be reduced. This value is measured in volts (V) — the same units that are used by our Ohm's law calculator.

Why exactly is it called oxidation/reduction potential? Oxidation occurs when electrons are removed — for example when a free radical steals an electron from a cell. Reduction, on the other hand, means receiving or gaining electrons, for instance, when an antioxidant donates an electron to a free radical.

What does it mean in terms of reduction potential? A solution with a higher potential will have a tendency to gain electrons (be reduced), and a solution with a lower potential — to lose electrons (be oxidized). Note that a high reduction potential doesn't mean that the reaction will occur — the reaction still requires some activation energy to be supplied.

It is difficult to measure the absolute potential of a solution. That's why the reduction potentials are usually defined relative to a reference electrode.

The standard reduction potential is the redox potential measured under standard conditions: 25 °C, activity equal to 1 per ion, and pressure of 1 bar per gas participating in the reaction. The standard reduction potential is defined relative to a standard hydrogen electrode (SHE), which is arbitrarily given a potential of 0 volts.

What is the cell potential equation?

The Nernst equation (cell potential equation) relates the reduction potential to the standard electrode potential, temperature, and activities of molecules. Activities can be substituted by concentrations for an approximate result. For a half-cell or full cell reaction, the Nernst equation is:

E = E₀ - RT/zF × ln([red]/[ox])


  • E — Reduction potential, expressed in volts (V);
  • E₀ — Standard reduction potential, also expressed in volts (V);
  • R — Gas constant, equal to 8.314 J/(K·mol);
  • T — Temperature at which the reaction would occur, measured in Kelvins (K);
  • z — Number of moles of electrons transferred in the reaction (mol);
  • F — Faraday constant, equal to the number of coulombs per mole of electrons (96,485.3 C/mol);
  • [red] — Chemical activity of the molecule (atom, ion…) in the reduced form. It can be substituted by concentration; and
  • [ox] — Chemical activity of the molecule (atom, ion…) in the oxidized form. It also can be substituted by concentration.

How to calculate reduction potential: a Nernst equation example

We will use the Nernst equation calculator to find the reduction potential of a cell basing on the following reactions:

  • Mg → Mg2+ + 2e-, where E₀ = +2.38 V

  • Pb2+ + 2e- → Pb, where E₀ = -0.13 V

  1. First, we need to write down the total reaction and calculate the total standard redox potential:

    Pb2+(aq) + Mg(s) → Mg2+(aq) + Pb(s)

    E₀(cell) = 2.38 V + -0.13 V = 2.25 V

  2. The next step is to determine the temperature and number of moles of electrons transferred. We can assume the temperature to be equal to 25 °C. 2 moles of electrons were transferred in this reaction.

  3. Now, we need to decide which molecules are oxidized and which reduced. The ones that gain electrons — that is, lead (Pb) molecules — are reduced. The magnesium (Mg) molecules are oxidized.

  4. The last step before performing calculations is to determine the proportion of activity or concentration. If we know the concentration of Pb molecules to be 0.200 M and of magnesium to be 0.020 M, the concentration proportion is [red]/[ox] = [Mg2+]/[Pb2+] = 0.020/0.200 = 0.1.

  5. Now we can combine all of these results and introduce them into the Nernst equation calculator. The final value of reduction potential is equal to 2.28 V.

Are you interested in the fundamentals of electrochemistry? Learn the other building block of this field with our electrolysis calculator!

Bogna Szyk
Standard red. potential (E₀)
Electrons transferred
Activity (reduced form)
Activity (oxidized form)
Reduction potential (E)
Check out 4 similar electrochemistry calculators 🔋
Cell EMFElectrolysisIonic strength… 1 more
People also viewed…

Beer-Lambert law

Use Omni's Beer-Lambert law calculator to calculate the absorbance of light as it passes through any substance. You can also use this calculator to determine the concentration of a solution using Beer's law.


This millionaire calculator will help you determine how long it will take for you to reach a 7-figure saving or any financial goal you have. You can use this calculator even if you are just starting to save or even if you already have savings.

Solution dilution

The solution dilution calculator tells you how to dilute a stock solution of known concentration.

Test grade

With this test grade calculator, you'll quickly determine the test percentage score and grade.
Copyright by Omni Calculator sp. z o.o.
Privacy, Cookies & Terms of Service