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The free energy of an electrochemical cell is given by the equation:

$\frac{?}{{?}_{\frac{?}{?}}G}=-$nFE

Where:

$\frac{?}{{?}_{\frac{?}{?}}G}=$ Gibbs Free Energy change

$n=$ moles of electrons

$F=$ Faraday's constant

$E=$ cell voltage

NOTE: Write $G$ as $dG($with no spaces$)$ for the answers below.

In order to solve for the Faraday's constant, $F,$ you must multiply both sides of the equation by the same expression:

$\frac{?}{{?}_{\frac{?}{?}}G}=-$nFE$$

The resulting equation is:

$F=$