How can I solve the Nernst equation?

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How can I solve the Nernst equation?

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Answer 1 · 2016-05-14T21:20:07

$E_{c e l l} = E_{c e l l}^{\circ} - \frac{R T}{n F} ln Q$ $E_(cell)=E_(cell)^@-(RT)/(nF)lnQ$

Explanation:

The Nernst Equation is the following:

$E_{c e l l} = E_{c e l l}^{\circ} - \frac{R T}{n F} ln Q$ $E_(cell)=E_(cell)^@-(RT)/(nF)lnQ$

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

For example, consider the following reaction:

$2 A l (s) + 3 M n^{2 +} (a q) \to 2 A l^{3 +} (a q) + 3 M n (s)$ $2Al(s)+3Mn^(2+)(aq)->2Al^(3+)(aq)+3Mn(s)$

the Nernst equation would be:

$E_{c e l l} = E_{c e l l}^{\circ} - \frac{R T}{n F} ln ⎛ ⎝ \frac{{[A l^{3 +}]}^{2}}{{[M n^{2 +}]}^{3}} ⎞ ⎠$ $E_(cell)=E_(cell)^@-(RT)/(nF)ln(([Al^(3+)]^2)/([Mn^(2+)]^3))$

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

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How can I solve the Nernst equation?

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