# Nernst Equation Chemistry Tutorial

## Key Concepts

- The Nernst Equation allows us to calculate the voltage produced by any electrochemical cell given E
^{o}values for its electrodes and the concentrations of reactants and products. - The general Nernst Equation:
E = E

^{o}-(RT/nF)lnQE

^{o}= standard electrochemical cell potential (voltage)

R = ideal gas constant

T = temperature

n = moles of electrons

F = Faraday constant = 96,485 C mol^{-1}

Q = mass-action expression (approximated by the equilibrium expression) - At 25°C the Nernst Equation is simplified to:
E = E

^{o}-(0.0592/n)log_{10}QE

^{o}= standard electrochemical cell potential (voltage)

n = moles of electrons

Q = mass-action expression (approximated by the equilibrium expression) - For a system at equilibrium at 25°C, E = 0 and the Nernst Equation is simplified to:
E

^{o}= (0.0592/n)log_{10}K

E^{o}= standard electrochemical cell potential (voltage)

n = moles of electrons

K = equilibrium expression