E°cell = E°cathode - E°anode
ΔG° = -nFE°cell
ΔG° = -RT ln K
E°cell = (RT / nF) * ln K
K = exp(nFE°cell / RT)
Ecell = E°cell - 0.0591/n * log(Q)
Ecell = E°cell - (RT / nF) * ln(Q)
Q = [Zn²⁺] / [Cu²⁺]
Q = I × t
Work = Q × Voltage
| Formula | Description | |------------------------------------------------|-------------------------------------------------| | E°cell = E°cathode - E°anode | Standard cell potential | | ΔG° = -nFE°cell | Gibbs free energy from cell potential | | ΔG° = -RT ln K | Gibbs free energy from equilibrium constant | | E°cell = (RT / nF) × ln K | Cell potential in terms of K | | K = exp(nFE°cell / RT) | Find K from cell potential | | Ecell = E°cell - 0.0591/n * log(Q) | Nernst at 25°C | | Ecell = E°cell - (RT / nF) × ln(Q) | General Nernst | | Q = I × t | Charge from current and time | | Work = Q × V | Work from charge and voltage |
Note: These are the key formulas and principles required for typical electrochemistry problems and calculations in academic contexts.