The Nernst equation calculates the electrode potential of an electrochemical cell under non-standard conditions (non-unit concentrations). E = E° − (RT/nF) × ln(Q). At 25°C it simplifies to E = E° − (0.0592/n) × log(Q).
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Did You Know?
The Nernst equation explains why a battery's voltage drops as it discharges — as reactants are consumed, Q increases, reducing E until E=0 at full discharge.
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