Master Thermodynamics and Electrochemistry: 129 Flashcards from Gibbs Free Energy to the Nernst Equation
Study thermodynamics and electrochemistry with 129 real flashcards: Gibbs free energy, entropy, redox, the Daniell cell, Nernst equation and corrosion.
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Two chapters that look separate are one equation seen twice. Thermodynamics & Electrochemistry on Flip It (deck code GE8638, 129 cards) merges them on purpose: the first half asks whether a reaction can happen, the second half makes it happen inside a cell and reads the answer in volts. The bridge is one card — ΔG = −nFE.
Study this deck: Thermodynamics & Electrochemistry
1 / 10Chemical thermodynamics
Tap the card for the answer · swipe right if you knew it, left if not
Ten cards from the deck
| Front | Back |
|---|---|
| Second law of thermodynamics (universal form) | In any spontaneous process, there is always an increase in entropy of the universe |
| Third law of thermodynamics | The entropy of a perfect crystal (well ordered) at 0 Kelvin is zero |
| Gibbs function (G) | A thermodynamic potential that measures the maximum reversible work that may be performed by a system at constant temperature and pressure |
| Chemical affinity | The quantity ∂G/∂ξ, symbolized by A, introduced by Théophile de Donder in 1923 |
| What does dG equal at thermodynamic equilibrium? | Zero |
| How is electrical work related to Gibbs free energy? | ΔG = −nFE, where n is moles of electrons, F is Faraday's constant, and E is cell potential |
| How do you calculate standard cell potential? | E°cell = E°red (cathode) − E°red (anode) |
| Nernst equation at 25°C (simplified) | E = E° − (0.0592/n) log Q |
| Anode half-reaction in a Daniell cell | Zn(s) → Zn²⁺(aq) + 2 e⁻ |
| Standard emf for iron rusting | 1.67 V (E° = 1.23 V − (−0.44 V)) |
Everything the 129 cards cover
- State functions and laws: internal energy (U), enthalpy (H), entropy (S), Gibbs free energy (G), the first, second and third laws, conservation of energy, the fundamental thermodynamic relation, extensive vs intensive properties, open and closed systems, thermodynamic equilibrium.
- Energy accounting: bomb calorimetry at constant volume, enthalpy change at constant pressure, enthalpy of formation, heat of combustion, bond energy, thermochemistry, phase transitions, isothermal and isobaric processes.
- The Gibbs machinery: dG = −SdT + VdP + Σμᵢ dNᵢ, chemical potential, the Gibbs-Duhem equation, extent of reaction ξ, stoichiometric coefficients, Legendre transformations, Massieu functions, entropy production, dissipative systems and Prigogine.
- Cells and potentials: galvanic vs electrolytic cells, anode, cathode, electrolyte, salt bridge, emf, the standard hydrogen electrode, E° for copper (+0.34 V) and zinc (−0.76 V), Faraday's constant (96,485 C/mol), concentration cells, thermal voltage RT/F.
- Redox and real devices: oxidation, reduction, oxidizing and reducing agents, the ion-electron balancing method, half-reactions, the Leclanché cell, zinc-carbon dry cells, lead-acid batteries, ATP and ADP, electrolysis, the Downs cell.
- Corrosion: rust as Fe₂O₃·xH₂O, salt water as an accelerant, copper patina, silver sulfide tarnish, passivating oxide layers on titanium and aluminium, sacrificial anodes.
Two tactics for this deck
Fix the signs before you memorise anything else. Spontaneous means ΔG negative, which via ΔG = −nFE means E positive. Every direction card in the deck resolves from that one line: a negative ΔG is a working battery, a positive one needs electrolysis. Say it out loud as you flip.
Use AN OX and RED CAT alongside OIL RIG. The deck gives you OIL RIG for the electron bookkeeping; add ANode = OXidation, REDuction = CAThode for the geometry. Drill the Daniell cell as the reference case — zinc dissolving, copper plating, salt bridge closing the circuit — and the rest of the cells become variations on it.
Pair this with Chemistry Lab Skills once the sign conventions are solid.
Get the deck
Sign in at flip-it.app and open Thermodynamics & Electrochemistry (deck code GE8638) from the library.
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