Question

In the equation ${\mathrm{G}}_{°}={\mathrm{nFE}}_{°\mathrm{cell}}$ F is__________.

Answer 1

Gibbs energy:

1. It is defined as the electrical work performed by the cell.
2. When a reaction is non-spontaneous, its value is positive, when it is spontaneous, it is negative, and when it is in equilibrium, its value is zero.
3. When both reactants and products are in their standard states Gibbs energy is given by ${\mathrm{G}}_{°}=-{\mathrm{nFE}}_{°\mathrm{cell}}$ where n$=$ number of moles of electron involved, F$=$Faraday constant which is equal to $96500$ Coulombs and ${\mathrm{E}}_{°\mathrm{cell}}=$emf of the cell.
4. The magnitude of electric charge per mole of electrons is represented by the Faraday constant.
5. It is equal to the Avogadro constant multiplied by the charge of an electron's elementary charge. F$=6.022\times {10}^{23}\times 1.6022\times {10}^{-19}\mathrm{C}\Rightarrow 96484.6\mathrm{C}{\mathrm{mol}}^{-1}\approx 96500\mathrm{C}{\mathrm{mol}}^{-1}$

Therefore, Gibbs energy is the product of the number of moles of electron involved, Emf of the cell, and Faraday constant.