Editing Electrochemical cell (section)

==== Cell potential ====
The cell potential can be predicted through the use of [[electrode potential]]s (the voltages of each half-cell). These half-cell potentials are defined relative to the assignment of 0 [[volt]]s to the [[standard hydrogen electrode]] (SHE). (See [[table of standard electrode potentials]]). The difference in voltage between electrode potentials gives a prediction for the potential measured. When calculating the difference in voltage, one must first rewrite the half-cell reaction equations to obtain a balanced oxidation-reduction equation.{{cn|date=December 2024}}

# Reverse the reduction reaction with the smallest potential (to create an oxidation reaction/overall positive cell potential)
# Half-reactions must be multiplied by integers to achieve electron balance.

Cell potentials have a possible range of roughly zero to 6 volts. Cells using water-based electrolytes are usually limited to cell potentials less than about 2.5 volts due to high reactivity of the powerful oxidizing and reducing agents with water which is needed to produce a higher voltage. Higher cell potentials are possible with cells using other [[solvent]]s instead of water. For instance, [[Lithium battery|lithium cells]] with a voltage of 3 volts are commonly available.{{cn|date=December 2024}}

The cell potential depends on the [[concentration]] of the reactants, as well as their type. As the cell is discharged, the concentration of the reactants decreases and the cell potential also decreases.{{cn|date=December 2024}}