# Nernst Equation Calculator

Free and user-friendly Nernst Equation determines the reduction potential of a cell in a split of seconds along with the step by step solution guide. All you need to do is give standard reduction potential, electron transfer, temperature and activity in reduced form and oxidised form as input and hit the calculate button.

Standard red. potential (E₀)
Temprature
Electron Transferred
Activity(reduced form)
Activity(oxidised form)

Online Nernst Equation Calculator: Need to solve reduction potential of a half cell or full cell quickly? Then, you can use this handy equation calculator nernst tool. It accepts the required inputs and gives the exact result easily. Moreover, you will also learn about what is reduction potential, the Nernst equation, steps to find cell reduction potential and solved example questions from this page.

## Steps to Calculate Reducation Potential

Go through the simple guidelines and instructions to compute the reduction potential of a cell reaction effortlessly.

• Obtain the number of electrons transferred, standard reduction potential, temperature, activity in reduced form, oxidized form.
• Get the cell potential equation.
• Place these values in the formula and solve it.

### What is Reducation Potential?

The reduction potential of a dell reaction is also known as the redox potential or reduction/oxidation potential. It measures the tendency of molecules to acquire electrons and be reduced.

The standard reduction potential is the redox potential measured under the standard conditions. The reduction potential means a solution with higher potential will have a tendency to gain electrons, with lower potential have a tendency to lose electrons.

### Cell Potential Equation

The cell potential equation or Nernst equation relates the reduction potential to the standard electrode potential, activities of molecules and temperature.

The Nernst equation for a half cell or fill cell reaction is E = E₀ - RT/zF * ln([red]/[ox])

The cell potential equation at 25°C or 300 K is E = E° - 0.0592/n log10 Q

Where,

E₀ is the standard reduction potential

E is the reduction potential

F is the Faraday constant 96,485.3 C/mol

R is the gas constant, 8.314 J/K mol

z is the number of moles of electrons transferred in the reaction

T is the temperature

[red] is the chemical activity of the molecule in the reduced form

[ox] is the chemical activity of the molecule in the oxidized form

Example:

Question: The standard electrode potential of zinc ions is 0.76 V. What will be the potential of a 2M solution at 300K?

Given that

Standard reducation potential E° = 0.76 V

n = 2

[Mn+] = 2 M

T = 300K

The nernst equation is E = E° - [(2.303RT)/nF] × log 1/[Mn+]

E = 0.76 - [(0.2303 x 8.314 x 300)/(2 x 965000] x log 1/2

= 0.76 - [0.0298 x -0.301]

= 0.76 + 0.009 = 0.769 V

Therefore, the potential of 2M solution is 0.769 V.

Make use of our website Onlinecalculator.guru and learn the difficult concepts that you never seemed to understand in a simple way using free tools available. ### Frequently Asked Question's on Calculator Nernst Equation

1. How to calculate the reduction potential of a cell reaction?

You have to enter the standard reduction potential, temperature, electron transferred, activity in reduced form and oxidised form. Click the calculate button of the calculator to obtain the result instantly.

2. What is the cell potential equation?

The Nernst equation is also called the cell potential equation. The formula is E = Eo - RT/zF * ln([red]/[ox]. The parameters of the cell potential equation are reduction potential, standard reduction potential, temperature, chemical activity of the molecule in oxidized form and reduced form.

3. What is the Nernst equation?

Nernst equation is the equation that relates the Gibbs free energy, reduction potential of an electrochemical cell. It is useful to determine the cell potential, equilibrium constant and so on.

4. What is the Nernst equation at 25°C?

The Nernst equation at 25°C is E = E° - 0.0592/n log10 Q. The overall potential of the electrochemical cell depends on the reaction quotient.