Question

How can I solve the Nernst equation?

Answer 1

`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.