Identify the two half-cells and their standard reduction potentials
Write the oxidation half-reaction and the reduction half-reaction
Determine the anode and cathode
Use the formula: EMF = E(cathode) – E(anode)
If standard conditions are given, use standard electrode potentials: E°cell = E°cathode – E°anode
If non-standard conditions are given, use the Nernst equation: Ecell = E°cell – (RT/nF) ln Q
At 25°C, use: Ecell = E°cell – (0.0591/n) log Q
Substitute the reaction quotient Q into the Nernst equation
Calculate the cell potential in volts
Check the sign of EMF
A positive EMF indicates a spontaneous cell reaction