How can I solve the Nernst equation?

1 Answer
May 14, 2016

Answer:

#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.