Oxidation Reduction Reaction Calculator

Redox Reaction Potential Calculator

Calculation Results

Standard Cell Potential (E°_cell):

Gibbs Free Energy (ΔG°):

Reaction Spontaneity:

function calculateRedox() { var eCathode = parseFloat(document.getElementById('cathodePotential').value); var eAnode = parseFloat(document.getElementById('anodePotential').value); var n = parseFloat(document.getElementById('electronsTransferred').value); var faraday = 96485; // C/mol if (isNaN(eCathode) || isNaN(eAnode) || isNaN(n) || n 0) { spontaneityBox.innerText = "Spontaneous"; spontaneityBox.style.backgroundColor = "#d4edda"; spontaneityBox.style.color = "#155724"; } else if (eCell < 0) { spontaneityBox.innerText = "Non-Spontaneous"; spontaneityBox.style.backgroundColor = "#f8d7da"; spontaneityBox.style.color = "#721c24"; } else { spontaneityBox.innerText = "Equilibrium"; spontaneityBox.style.backgroundColor = "#fff3cd"; spontaneityBox.style.color = "#856404"; } document.getElementById('redoxResult').style.display = "block"; }

Understanding Oxidation-Reduction (Redox) Reactions

Oxidation-Reduction reactions, commonly known as Redox reactions, are chemical processes that involve the transfer of electrons between two species. These reactions are fundamental to electrochemistry, battery technology, and biological processes like cellular respiration.

Key Components of Redox Calculations

• Oxidation: The loss of electrons. This occurs at the Anode.
• Reduction: The gain of electrons. This occurs at the Cathode.
• Standard Reduction Potential (E°): A measure of the tendency of a chemical species to be reduced, measured in Volts (V).
• Cell Potential (E°_cell): The electromotive force (EMF) produced by the electrochemical cell.

The Formulas Used

This calculator utilizes standard electrochemical equations to determine the viability of a reaction:

1. Cell Potential Formula: E°cell = E°cathode - E°anode
2. Gibbs Free Energy Formula: ΔG° = -nFE°cell
   Where n is the moles of electrons, and F is Faraday's constant (96,485 C/mol).

Practical Example: The Daniell Cell

In a typical Daniell Cell (Zinc-Copper battery):

• Cathode (Copper): E° = +0.34 V
• Anode (Zinc): E° = -0.76 V
• Electrons (n): 2

Calculations:
E°_cell = 0.34 – (-0.76) = 1.10 V
Because E°_cell is positive, the reaction is spontaneous, meaning it can generate an electrical current naturally.

Spontaneity and ΔG°

The spontaneity of a reaction tells us if it will proceed without external energy input:

E°cell Value	ΔG° Value	Result
Positive (+)	Negative (-)	Spontaneous (Galvanic/Voltaic)
Negative (-)	Positive (+)	Non-Spontaneous (Electrolytic)
Zero (0)	Zero (0)	Equilibrium