Nernst Equation

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= Nernst Equation<br>  =
 
 
 
'''Nernst Equation''' is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).<br>  
 
'''Nernst Equation''' is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).<br>  
  
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R is the universal gas constant; R = 8.314471 J K<sup>-1</sup> mol<sup>-1</sup>  
 
R is the universal gas constant; R = 8.314471 J K<sup>-1</sup> mol<sup>-1</sup>  
  
T is the thermodynamics temperature, in ''Kelvin''; 0 K = -273.15<sup>o</sup>C<br>
+
T is the thermodynamics temperature, in ''Kelvin''; 0 K = -273.15<sup>o</sup>C<br>  
  
z is the number of moles of electrons transferred between cells (defined by the valency of ions)<br>
+
z is the number of moles of electrons transferred between cells (defined by the valency of ions)<br>  
  
F is the Faraday's constant; F = 96,485.3415 C mol<sup>-1</sup><br>
+
F is the Faraday's constant; F = 96,485.3415 C mol<sup>-1</sup><br>  
  
[red] is the concentration of ion that gained electrons (reduction)<br>
+
[red] is the concentration of ion that gained electrons (reduction)<br>  
  
[oxi] is the concentration of ion that lost electrons (oxidation)<br>
+
[oxi] is the concentration of ion that lost electrons (oxidation)<br>  
  
<br>
+
<br>  
  
== Membrane Potential<br> ==
+
== Membrane Potential<br> ==
  
Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:<br>
+
Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:<br>  
  
 +
<br>
  
 +
[[Image:Nernst equation2.png|304x107px]]
  
[[Image:Nernst_equation2.png|304x107px]]
+
<br>
  
 +
or
  
 +
<br>
  
or
+
[[Image:Nernst equation3.png|439x115px]]  
 
+
 
+
 
+
[[Image:Nernst_equation3.png|439x115px]]
+
 
+
  
 +
<br>
  
 
where
 
where

Revision as of 21:38, 14 November 2010

Nernst Equation is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).


Equation

Nernst equation can be expressed as follows:


Nernst equation1.png


where


Ecell is the half-cell potential difference

Eθcell is the standard half-cell potential

R is the universal gas constant; R = 8.314471 J K-1 mol-1

T is the thermodynamics temperature, in Kelvin; 0 K = -273.15oC

z is the number of moles of electrons transferred between cells (defined by the valency of ions)

F is the Faraday's constant; F = 96,485.3415 C mol-1

[red] is the concentration of ion that gained electrons (reduction)

[oxi] is the concentration of ion that lost electrons (oxidation)


Membrane Potential

Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:


Nernst equation2.png


or


Nernst equation3.png


where

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