# How can I solve the Nernst equation?

May 14, 2016

${E}_{c e l l} = {E}_{c e l l}^{\circ} - \frac{R T}{n F} \ln Q$

#### Explanation:

The Nernst Equation is the following:

${E}_{c e l l} = {E}_{c e l l}^{\circ} - \frac{R T}{n F} \ln Q$

Where,
$n$ is the number of mole electrons exchanged during the redox reaction,
$F = 96485 \frac{C}{\text{mol } {e}^{-}}$ is Faraday's constant.
$R = 8.3145 \frac{J}{K \cdot m o l}$ is the ideal gas law constant,
$T$ is the Kelvin temperature,
and $Q$ is the reaction quotient.

For example, consider the following reaction:

$2 A l \left(s\right) + 3 M {n}^{2 +} \left(a q\right) \to 2 A {l}^{3 +} \left(a q\right) + 3 M n \left(s\right)$

the Nernst equation would be:

${E}_{c e l l} = {E}_{c e l l}^{\circ} - \frac{R T}{n F} \ln \left(\frac{{\left[A {l}^{3 +}\right]}^{2}}{{\left[M {n}^{2 +}\right]}^{3}}\right)$

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