The standard electrode potential of a half-cell is the voltage measured under standard conditions when the half-cell is connected to a standard hydrogen electrode.
An example of an electrochemical cell with a standard hydrogen electrode:
- Pt | H2(aq) || Zn,2+(aq) | Zn(s)
The standard hydrogen electrode is always shown on the left - it doesn't matter if the other half-cell is more negative.
Standard hydrogen electrodes can be used to calculate standard electrode potentials because the standard hydrogen electrode half-cell has an electrode potential of 0.00 V.
The whole cell potential is: E*cell = (E*right - E*left)
The E*left is zero so the voltage reading will be equal to E*right = E*cell.
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