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
- standard electrode potential
- The e.m.f. of a half cell compared with a standard hydrogen half cell, measured under standard conditions.
More in Electrochemistry
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- Standard Cell Potentials Eθcell Values and Electrochemical Cells
- Cell Diagrams
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- Electrochemical Cells
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All 14 lessons in Electrochemistry · All OCR A-level Chemistry topics