Redox Reaction Calculator

Calculate cell potentials, Gibbs free energy, and equilibrium constants for redox reactions. Perfect for electrochemistry, battery chemistry, and oxidation-reduction calculations.

Redox Reaction Calculator

About Redox Reactions

Formula

E°cell = E°cathode - E°anode

Where F = Faraday's constant (96,485 C/mol), R = Gas constant (8.314 J/mol·K)

Key Concepts

  • Redox Reaction: Oxidation-reduction reaction involving electron transfer
  • Anode: Site of oxidation (loses electrons)
  • Cathode: Site of reduction (gains electrons)
  • Cell Potential: Driving force for electron flow
  • Standard Conditions: 1 M concentration, 1 atm pressure, 298.15 K

Spontaneity Rules

  • E°cell > 0: Reaction is spontaneous (galvanic cell)
  • E°cell < 0: Reaction is non-spontaneous (electrolytic cell)
  • E°cell = 0: Reaction is at equilibrium

Common Standard Potentials

Li+ + e- → Li-3.04 V
K+ + e- → K-2.93 V
Ca2+ + 2e- → Ca-2.87 V
Na+ + e- → Na-2.71 V
Mg2+ + 2e- → Mg-2.37 V
Al3+ + 3e- → Al-1.66 V
Zn2+ + 2e- → Zn-0.76 V
Fe2+ + 2e- → Fe-0.44 V
Cd2+ + 2e- → Cd-0.40 V
Co2+ + 2e- → Co-0.28 V
Ni2+ + 2e- → Ni-0.25 V
Sn2+ + 2e- → Sn-0.14 V
Pb2+ + 2e- → Pb-0.13 V
2H+ + 2e- → H20.00 V
Cu2+ + 2e- → Cu0.34 V
Cu+ + e- → Cu0.52 V
I2 + 2e- → 2I-0.54 V
Fe3+ + e- → Fe2+0.77 V
Ag+ + e- → Ag0.80 V
Hg2+ + 2e- → Hg0.85 V
Br2 + 2e- → 2Br-1.07 V
O2 + 4H+ + 4e- → 2H2O1.23 V
Cl2 + 2e- → 2Cl-1.36 V
Au3+ + 3e- → Au1.50 V
F2 + 2e- → 2F-2.87 V

How to Use

  1. Select the calculation type you want to perform
  2. Enter the required values based on your calculation
  3. Use standard reduction potentials from the table
  4. Click Calculate to get the result

Common Applications

  • Battery and fuel cell design
  • Corrosion prevention
  • Electroplating processes
  • Biological redox reactions
  • Environmental chemistry

Important Notes

  • More positive potentials indicate stronger oxidizing agents
  • More negative potentials indicate stronger reducing agents
  • Standard potentials are measured at 298.15 K
  • Cell potential is independent of cell size
  • Nernst equation accounts for concentration effects