← Labs|

Electrochemistry & Nernst Equation Simulator

Galvanic Cell — Live
Anode: Zn²⁺ → Zn (oxidation)Cu²⁺ → Cu (reduction)
Cell EMF
1.100 V
✓ Spontaneous (galvanic)
Nernst Equation
E = E° − (RT/nF)·ln Q
E = 1.100 − 0.01284·ln(1.0e+0)
= 1.100 V
Thermodynamics
E°cell
Standard EMF
1.100 V
E cell
at T=298K, Q=1.0e+0
1.100 V
ΔG°
= −nFE°
-212.3 kJ/mol
ΔG
= −nFE
-212.3 kJ/mol
Kc
Equilibrium constant
1.62e+37
n (e⁻)
Electrons transferred
2

Cell EMF vs Reaction Quotient Q

Nernst equation — how EMF drops as Q increases

At equilibrium (E=0)
log(Kc) = 37.21
ΔG° = −nFE°
Standard Gibbs & EMF
ΔG° = −RT ln Kc
Gibbs & equilibrium
log Kc = nE°/0.0592
At 298K (simplified)