Electrochemistry Formulas - Gibbs Free Energy, Equilibrium K, Cell Potential, Nernst Equation

Electric potential is the work per unit of charge, measured in joules, while voltage is the electric potential difference between two points, measured in volts.

The cell potential is the cell potential of the cathode minus the cell potential of the anode. The negative sign for the anode is because you need to reverse the standard reduction potential for the anode, as oxidation occurs at the anode.

The negative sign is there because the standard reduction potential for the anode must be reversed to represent an oxidation reaction, which occurs at the anode.

Oxidation occurs with a loss of electrons, while reduction occurs with a gain of electrons.

Copper 2+ gaining two electrons turns into copper metal, with a cell potential of 34 volts.

Zinc gives up two electrons to turn into zinc 2+, with a standard reduction potential of 0.76 volts when the reaction is written in reverse.

Using the equation ΔG = -nFE, where n is the number of electrons transferred, F is Faraday's constant, and E is the cell potential.

ΔG = -RT Ln K, where R is the gas constant, T is the temperature in Kelvin, and K is the equilibrium constant.

E = RT Ln K / NF, where R is the gas constant, T is the temperature in Kelvin, K is the equilibrium constant, N is the number of moles of electrons transferred, and F is Faraday's constant.

E = E° - 0.0591 log Q/n, where E° is the standard cell potential, Q is the reaction quotient, and n is the number of moles of electrons transferred.

Q is calculated in a similar way to the equilibrium constant K, as products over reactants, but it does not include solids in its expression.

Q = [Zn 2+]/[Cu 2+], as zinc metal and copper metal are in the solid state and are not included in the expression.

E = E° - (RT/NF) * ln Q, where R is the gas constant, T is the temperature in Kelvin, and Q is the reaction quotient.

Faraday's constant is 96,485 coulombs per mole of electrons transferred.

One mole of electrons is equal to 96485 coulombs.

One coulomb is equal to 1 amp times 1 second, based on the equation Q = It, where Q is the charge, I is the electric current, and t is the time in seconds.

The work done by a charge is equal to the magnitude of the charge times the voltage, where 1 volt is equal to 1 joule per coulomb.

Electric potential is the work per unit of charge, measured in joules, while voltage is the electric potential difference between two points, measured in volts.

The cell potential is the cell potential of the cathode minus the cell potential of the anode. The negative sign for the anode is because you need to reverse the standard reduction potential for the anode, as oxidation occurs at the anode.