Thermodynamics and Electrochemistry Cheat Sheet

The core ideas of Thermodynamics and Electrochemistry distilled into a single, scannable reference — perfect for review or quick lookup.

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Quick Reference

Measure of energy dispersal or microstates. Increases with more particles, higher T, or greater volume.

G=H-TS. delta-G<0: spontaneous. delta-G>0: non-spontaneous. delta-G=0: equilibrium.

E-cell = E-cathode - E-anode. Positive E-cell means spontaneous galvanic cell.

Electrochemical cell where spontaneous redox reaction produces electric current.

Uses external current to drive non-spontaneous redox reaction.

E=E0-(RT/nF)lnQ adjusts cell potential for non-standard conditions.

Mass deposited = (ItM)/(nF). Links charge to moles of substance.

Total entropy of universe increases for spontaneous processes.

Entropy (S):Thermodynamic quantity measuring energy dispersal; units J/(mol K).

Gibbs Free Energy (G):G = H - TS; criterion for spontaneity at constant T and P.

Spontaneous Process:Process that occurs without continuous external input; delta-G < 0.

Standard Cell Potential (E0):Voltage of an electrochemical cell under standard conditions (1M, 1atm, 25C).

Galvanic (Voltaic) Cell:Cell producing electricity from a spontaneous redox reaction.

Electrolytic Cell:Cell using external electricity to drive a non-spontaneous reaction.

Anode:Electrode where oxidation occurs.

Cathode:Electrode where reduction occurs.

Nernst Equation:E = E0 - (RT/nF)lnQ; relates cell potential to non-standard conditions.

Faraday Constant (F):96485 C/mol; charge of one mole of electrons.

Standard Reduction Potential:Voltage for a half-reaction written as reduction, relative to SHE.

Salt Bridge:Connection allowing ion flow between half-cells to maintain electrical neutrality.

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