Electrochemistry Calculator
Calculate cell potential using Nernst equation. Find standard reduction potentials and Gibbs free energy.
Cell Potential
1.1000 V
Standard Cell Potential (E°cell)
-212.27 kJ/mol
Gibbs Free Energy (ΔG)
Yes
Spontaneous?
Galvanic Cell Diagram
Calculation Steps

Cell Potential: E°cell = E°cathode - E°anode

E°cathode (reduction) = 0.34 V

E°anode (reduction potential) = -0.76 V

E°cell = 0.34 - -0.76 = 1.1000 V

Gibbs Free Energy: ΔG = -nFE

ΔG = -2 × 96485 × 1.1000

ΔG = -212267.00 J/mol = -212.2670 kJ/mol

Reaction is SPONTANEOUS (E > 0)

Half-Reactions

Cathode (Reduction):

Cu2+ + 2e- -> Cu

E° = 0.34 V

Anode (Oxidation):

Zn -> Zn2+ + 2e-

E° = 0.76 V (reversed)

Standard Reduction Potentials
SpeciesHalf-ReactionE° (V)
LithiumLi+ + e- -> Li-3.04
PotassiumK+ + e- -> K-2.93
CalciumCa2+ + 2e- -> Ca-2.87
SodiumNa+ + e- -> Na-2.71
MagnesiumMg2+ + 2e- -> Mg-2.37
AluminumAl3+ + 3e- -> Al-1.66
ZincZn2+ + 2e- -> Zn-0.76
IronFe2+ + 2e- -> Fe-0.44
NickelNi2+ + 2e- -> Ni-0.26
TinSn2+ + 2e- -> Sn-0.14
LeadPb2+ + 2e- -> Pb-0.13
Hydrogen2H+ + 2e- -> H20
Copper(II)Cu2+ + 2e- -> Cu+0.34
IodineI2 + 2e- -> 2I-+0.54
SilverAg+ + e- -> Ag+0.8
BromineBr2 + 2e- -> 2Br-+1.07
ChlorineCl2 + 2e- -> 2Cl-+1.36
Gold(III)Au3+ + 3e- -> Au+1.5
FluorineF2 + 2e- -> 2F-+2.87

Key Formulas

E°cell = E°cathode - E°anode
Nernst: E = E° - (RT/nF)ln(Q)
At 25°C: E = E° - (0.0592/n)log(Q)
Gibbs: ΔG = -nFE
R = 8.314 J/(mol·K)
F = 96485 C/mol

Tips:

  • Higher E° means stronger oxidizing agent (more likely to be reduced)
  • Spontaneous reactions have positive E°cell and negative ΔG
  • The anode is where oxidation occurs (loses electrons)
  • The cathode is where reduction occurs (gains electrons)

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