Galvanic Cell Potential Calculator

Calculate the standard potential of an electrochemical cell by combining the reduction potentials of the cathode and anode.

E° Reduction (Cathode)

E° Reduction (Anode)

Standard Cell Potential (E°)

1.10 V

Cell TypeGalvanic / Voltaic (Produces Energy)

SpontaneitySpontaneous

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The Architecture of a Battery

A Galvanic Cell (also known as a Voltaic Cell) is a device that harnesses a spontaneous chemical reaction to generate electrical energy. It is the fundamental architecture behind every battery in the modern world.

To build a battery, you must connect two different metals. One metal must want to give away its electrons (oxidation at the Anode), and the other metal must want to accept those electrons (reduction at the Cathode).

Standard Reduction Potentials

Chemists rank every chemical element on a list based on how aggressively it wants to steal electrons. This is called the Standard Reduction Potential ( $E^\circ_{red}$ ), measured in Volts.

High positive voltages (like Fluorine or Gold) mean the element desperately wants to steal electrons.
Negative voltages (like Lithium or Zinc) mean the element hates electrons and wants to give them away.

To calculate the total voltage your battery will produce, you simply subtract the potential of the anode from the potential of the cathode.

The Equation

\begin{aligned} E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode} \end{aligned}

Where:

E^\circ_{cell}

Standard Cell Potential

E^\circ_{cathode}

Reduction Potential of Cathode

E^\circ_{anode}

Reduction Potential of Anode

The Rule of Spontaneity

For a battery to actually work (be spontaneous), the resulting $E^\circ_{cell}$ must be a positive number. If the result is negative, the reaction is non-spontaneous, meaning you have accidentally built an electrolytic cell and must plug it into the wall to force it to run backwards.

Frequently Asked Questions

In a spontaneously operating galvanic cell, the chemical with the higher (more positive) reduction potential will automatically act as the cathode and force the other metal to be the anode.

Never! Voltage is an intensive property. It does not matter if the balanced equation requires 1 mole of zinc or 5 moles of zinc; the physical voltage generated by a single zinc atom dropping an electron remains exactly the same.

It indicates 'Standard Conditions'. It guarantees the textbook value was measured at exactly 1.0 Molar concentration, 1 atmosphere of pressure, and typically 25°C.

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