Explain nerst equation., Chemistry

The tendency to metal to lose electrons or tendency of its ions to gain electrons depends upon the concentration of the ions in solution. At the same time, the tendency to lose or gain electrons is expressed in terms of electrode potentials. The value of electrode potential, thus, varies with the variation in the concentration of the ions. The quantitative relationship between the concentration of ions and electrode potentials is given by Nerst equation. For a common electrode reaction:

Mn+ + ne-  2085_nerst equation.png  M

The nerst equation can be written in the two ways as

1027_nerst equation1.png  + (RT/nF) In [Mn+]/[M]

Or, 1027_nerst equation1.png - (RT/nF) In [Mn+]/[M]

In the present aspect, only the first form will be used in the further discussion. Converting natural logarithm (In) to log10 in the first expression, we get

1027_nerst equation1.png  + (2.303 RT/nF) log [Mn+]/[M],

Where, 1872_nerst equation2.png = electrode potential

714_electrochemical3.png  = standard electrode potential with reference to SHE when concentration of Mn+ is 1 mol L-1

R = 8.314 JK-1 mol-1;

T = temperature

[Mn+] = molar concentration of ions;

n = number of electrons gained

F = Faraday constant 96500 C mol-1;

[M] = concentration of metal

Substituting these values, we get

632_nerst equation3.png  log [Mn+]/[M]

1868_electrochemical3.png =  + (0.059/n) log [Mn+]/[M]

In general, for any electrode,

Ered = 2015_nerst equation4.png + (0.059/n) log [oxidized state]/[reduced state]










Posted Date: 6/26/2012 1:59:03 AM | Location : United States

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