BRAINCAKENon-Standard Conditions
The half equations are reversible reactions. The Eθ values depend on the position of equilibrium. Any factor that alters the position of equilibrium will alter the standard electrode potential in the direction predicted by Le Chatelier's principle. In the following equilibrium
MnO4-(aq) + 8H+ + 5e- &rlhar Mn2+(aq) + 4H2O(l)
The standard electrode potential Eθ is +1.52V. If the concentration of manganate (VII) ions or hydrogen ions is increased above 1.0 moldm-3 the position of equilibrium will move to the right to counteract the change according to Le Chatelier's principle. Fewer electrons will be released and the electrode potential will become more positive than the standard value.
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Key terms in this lesson
- le chatelier's principle
- If a system at equilibrium is subjected to a change in concentration, pressure or temperature, the position of equilibrium shifts to oppose that change.
More in Electrochemistry
- The Standard Hydrogen Half Cell
- Standard Electrode Potential Eθ and the Electrochemical Series
- Calomel Electrode
- Standard Cell Potentials Eθcell Values and Electrochemical Cells
- Cell Diagrams
- Thermodynamic Feasibility of a Reaction and the Extent of a Reaction
- Electrochemical Cells
- Rechargeable Batteries
All 14 lessons in Electrochemistry · All Edexcel A-level Chemistry topics