Nernst Equation
In
electrochemistry
, the
Nernst equation
gives the
electrode potential
(E)
, relative to the
standard electrode potential
,
(E
0
)
, of the electrode couple or, equivalently, of the half cells of a
battery
E = E^0 - \frac{RT}{nF} \ln\frac{a_{\mbox{red}}}{a_{\mbox{ox}}} At room temperature the following is true
E = E^0 - \frac{0.0591}{n} \log\frac{
\mbox{red}
}{
\mbox{ox}
}
R
is the
universal gas constant
, equal to 8.314570 J K
-1
mol
-1
T
the
temperature
in
kelvins
a
the chemical
activities
on the reduced and oxidized side, respectively
F
is the
Faraday constant
, equal to 96,485 C mol
-1
n
is the number of
electrons
transferred in the
half-reaction
.
red
is the concentration of
oxidizing agent
(the reduced species).
ox
is the concentration of
reducing agent
(the oxidized species).
History
The Nernst equation is named after the German physical chemist
Walther Nernst
who first formulated it.
See also
Electrodiffusion
.
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