MathLiveNernst equation
The Nernst equation gives the electrochemical cell potential under non-standard conditions, correcting the standard potential for temperature and reaction quotient. It is used to calculate electrode and cell voltages when concentrations differ from standard values.
E_{\mathrm{cell}}=E_{\mathrm{cell}}^\ominus-\frac{RT}{zF}\ln Q_{\mathrm{r}}What the symbols mean
| cell potential under the actual conditions (V) | |
| standard cell potential (V) | |
| molar gas constant (J·mol⁻¹·K⁻¹) | |
| thermodynamic temperature (K) | |
| number of electrons transferred in the reaction | |
| Faraday constant (C·mol⁻¹) | |
| reaction quotient |
About this formula
- FieldChemistry
- TopicElectrochemistry
- LevelUniversity
- Also calledNernst equation electrochemistry, cell potential under non-standard conditions, electrode potential formula, Nernst potential, reaction quotient cell voltage, E cell Nernst
- SourceWikidata Q751124
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