How can I solve the Nernst equation?

1 Answer
Dr. Hayek
May 14, 2016

#E_(cell)=E_(cell)^@-(RT)/(nF)lnQ#

Explanation:

The Nernst Equation is the following:

#E_(cell)=E_(cell)^@-(RT)/(nF)lnQ#

Where,
#n# is the number of mole electrons exchanged during the redox reaction,
#F=96485C/("mol "e^-)# is Faraday's constant.
#R=8.3145J/(K*mol)# is the ideal gas law constant,
#T# is the Kelvin temperature,
and #Q# is the reaction quotient.

For example, consider the following reaction:

#2Al(s)+3Mn^(2+)(aq)->2Al^(3+)(aq)+3Mn(s)#

the Nernst equation would be:

#E_(cell)=E_(cell)^@-(RT)/(nF)ln(([Al^(3+)]^2)/([Mn^(2+)]^3))#

Here is a video that explains more about the Nernst equation, I hope you find it helpful:
Electrochemistry | The Concentration Cell.

Related questions
See all questions in Calculating Energy in Electrochemical Processes
Impact of this question
4687 views around the world
You can reuse this answer
Creative Commons License