The Nernst equation is used to calculate the electromotive force (EMF) of a cell at any given moment. It is represented as:
Ecell = E°cell - (RT/nF) * ln(Q)
Where:
- Ecell is the EMF of the cell
- E°cell is the standard electrode potential of the cell
- R is the gas constant (8.314 J/(mol*K))
- T is the temperature in Kelvin
- n is the number of moles of electrons transferred in the cell reaction
- F is Faraday's constant (96,485 C/mol)
- Q is the reaction quotient, which is the ratio of the concentrations of products to reactants raised to their stoichiometric coefficients
This equation shows the relationship between the EMF of a cell and the concentrations of the reactants and products involved in the cell reaction. It is a fundamental equation in electrochemistry and is used to determine the potential of a cell under non-standard conditions.
derive nernst equation for emf of cell
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