Redox Reactions & Electrochemistry: 5-Bullet Final Revision

Cell EMF: E°cell = E°cathode − E°anode (cathode minus anode); E°cell > 0 → spontaneous ( $\Delta G$ ° < 0); Daniell cell: E°cell = 0.34 − (−0.76) = 1.10 V.
Nernst equation: E = E° − (0.0592/n) log Q at 25°C; at equilibrium E = 0 → E° = (0.0592/n) log K; $\Delta G$ ° = −nFE°; F = 96500 C/mol.
Faraday's law: w = MIt/(nF); t in seconds; n = 1 ( $Ag^{+}$ ), n = 2 ( $Cu^{2+}$ , $Zn^{2+}$ ), n = 3 ( $Al^{3+}$ ); 2 A × 1 hr through $CuSO_{4}$ deposits 2.37 g Cu.
Conductance: Λm = Λ°m − A√C (strong); α = Λm/Λ°m (weak); Kohlrausch: Λ°m( $CH_{3}COOH$ ) = Λ°m( $CH_{3}COONa$ ) + Λ°m(HCl) − Λ°m(NaCl).
Cell polarity trap: Anode = NEGATIVE in galvanic; Anode = POSITIVE in electrolytic. In BOTH: oxidation at anode, reduction at cathode ("AN OX RED CAT").