The potential difference between the anode and cathode in a cell that allows electrons to flow in one direction (from higher to lower potential energy).

Also called cell potential

Designated as E^o_cell.

Measured in volts (1V = 1J/C)

Reactions that occur at cathode and anode

Concentrations of reactants and products

Temperature

The reduction potential for hydrogen is 0V:
2 H⁺ + 2e^- ---> H₂

From anode (high potential energy) to cathode (low potential energy).

Standard half-cell potentials tabulated for reduction reactions.

Denoted as E^o_red

Whenever we assign an electrical potential to a half-reaction, we write the reaction as a reduction.

Because cell potential is based on the potential energy per unit of charge, it is an intensive property (does not depend on size/amount of substances)

Thus, changing the stoichiometric coefficient in a half-reaction does not affect the value of the standard reduction potential.

Accounts for

Concentration of reactants and products: 1 atm for gasses, 1M for aqueous solutions

Temperature: 25^oC

E^o_cell = E^o_red(cathode) - E^o_red(anode)

Cell potential is always positive; E^o_red value for cathode is always more positive than E^o_red of anode.

The half-reaction with the most negative reduction potential is the one most easily reversed and run as an oxidation.

The strongest oxidizers have the most positive reduction potentials

The strongest reducers have the most negative reduction potentials