Standard Electrode Potential Notes

Describe the standard hydrogen electrode.

Standard Hydrogen Electrode: A reference half‑cell made of H₂ gas at 1 atm bubbled over a platinum electrode in 1.0 M H⁺, assigned 0.00 V to provide the standard for measuring all other electrode potentials.

Explain the term standard electrode (reduction) potential, 𝐸o.

Standard Electrode (Reduction) Potential E^o: The measured voltage of a half‑cell under standard conditions (1.0 M, 1 atm, 25 °C) relative to the standard hydrogen electrode, showing how readily the species is reduced.

Identify the limitations associated with standard electrode (reduction) potentials, 𝐸o.

Calculate cell potential, 𝐸cell o (Formula: 𝐸cell o o =𝐸reduction half−cell o −𝐸oxidation half−cell )

Formula: 𝐸cell o o =𝐸reduction half−cell o −𝐸oxidation half−cell.

Apply standard electrode potentials to determine the relative strength of oxidising and reducing agents.

Higher E-naught Value: stronger oxidising agents because they are more easily reduced

Lower E-naught Value: stronger reducing agents because they are more easily oxidised.

Analyse data, including standard electrode potentials, to make predictions about the spontaneity of a reaction and to compare electrochemical cells.

How to Know if Spontaneous Reaction WIll Occur: If a postive E-naught value is produced from the formula.