CHAPTER 21: Electrode Potentials
- Standard Electrode Potential
- Measuring Standard Electrode Potential
- Using E° Values
- Cells and Batteries
- Quantitative Electrolysis
- define the terms:
- standard electrode (redox) potential
- standard cell potential
- describe the standard hydrogen electrode
- describe methods used to measure the standard electrode potentials of:
- metals or non-metals in contact with their ions in aqueous solution
- ions of the same element in different oxidation states
- calculate a standard cell potential by combining two standard electrode potentials
- use standard cell potentials to:
- explain/deduce the direction of electron flow from a simple cell
- predict the feasibility of a reaction
- construct redox equations using the relevant half-equations.
- predict qualitatively how the value of an electrode potential varies with the concentration of the aqueous ion
- state the possible advantages of developing other types of cell, g. the H2/O2 fuel cell and improved batteries (as in electric vehicles) in terms of smaller size, lower mass and higher voltage.
- state the relationship, F = Le, between the Faraday constant, the Avogadro constant and the charge on the electron
- predict the identity of the substance liberated during electrolysis from the state of electrolyte (molten or aqueous), position in the redox series (electrode potential) and concentration
- calculate:
- the quantity of charge passed during electrolysis
- the mass and/or volume of substance liberated during electrolysis, including those in the electrolysis of H2SO4(aq), Na2SO4(aq).
- describe the determination of a value of the Avogadro constant by an electrolytic method