# Nernst's Equation

(1) **Nernst’s equation for electrode potential**

The potential of the electrode at which the reaction,

_{}

takes place is described by the equation, _{}

or_{}

above eq. is called the **Nernst equation**.

Where,

** _{}**=the potential of the electrode at a given concentration,

_{} = the standard electrode potential

R = the universal gas constant, _{}

T= the temperature on the absolute scale,

n = the number of electrons involved in the electrode reaction,

F = the Faraday constant : (96500 C),

_{}= the concentration of the deposited metal,

_{}= the molar concentration of the metal ion in the solution,

The concentration of pure metal M(s) is taken as unity. So, the Nernst equation for the _{} electrode is written as,

_{}

At 298 K, the Nernst equation for the _{} electrode can be written as,

_{}

For an electrode (half - cell) corresponding to the electrode reaction,

Oxidised form _{}Reduced form

The Nernst equation for the electrode is written as,

_{}

At 298 K, the Nernst equation can be written as,

_{}