Electrochemistry — Chemistry Lab

FPS: --

E°cell: --

Ecell: --

ΔG: --

Q: --

E°cell / Spontaneous

Presets

Parameters

Anode (Oxidation) Zn

Cathode (Reduction) Cu

Anode [ion] (M) 1.0

Cathode [ion] (M) 1.0

Temperature (K) 298

Show Math

Governing Equations


Cell Potential (Standard):
  E°cell = E°cathode - E°anode
  Spontaneous when E°cell > 0

Nernst Equation (at 298 K):
  Ecell = E°cell - (RT/nF) ln Q
  Ecell = E°cell - (0.0592/n) log Q

Reaction Quotient:
  Q = [products]^coeff / [reactants]^coeff

Gibbs Free Energy:
  ΔG = -nFEcell
  ΔG° = -nFE°cell
  Spontaneous when ΔG < 0

Concentration Cell:
  Ecell = -(RT/nF) ln([dilute]/[concentrated])
  Same metal, different concentrations

Real-World Connection: Electrochemical cells power batteries, fuel cells, and corrosion prevention systems. The Daniell cell was one of the earliest practical batteries, and modern lithium-ion batteries use the same fundamental principles of redox chemistry and ion transport to store and release energy efficiently.