Electrochemistry Formulas

relation between free energy difference and electric potential difference

∆G= free energy change

n= moles of e⁻

F= Faraday's constant (9.649 X 10⁴ C/mol)

E= Electric potential (volts)

SHE half reaction

Nerst Equation at standard conditions (25 C)

E= Electric potential (volts)

E°= standard reduction potential (ActA=ActB=1)

R= gas constant(8.314J/(K*mol)= 8.314(V*C)/(K*mol)

T= temperature (K)

n= number of electrons transferred in the half-reaction

Q= reaction quotient

Reaction Quotient

Q= reaction quotient

Nerst Equation at nonstandard conditions

E= Electric potential (volts)

R= 8.314 j/mol/K

Q= reaction quotient, defined as the ratio of product concentrations to reactant concentrations at any point in a reaction, each raised to the power of their coefficients in the balanced chemical equation.

T= Temperature in Kelvin

F= faradays constant 

E°= standard reduction potential (ActA=ActB=1)

n= number of electrons in the half-reaction

Finding E° from K

E°= standard reduction potential (ActA=ActB=1)

n= number of electrons in the half-reaction

K= equilibrium constant

reduction potential formula