$word_{count}$: 170

$E_{cell}$ = $E_{cathode}$ - $E_{anode}$ (reduction potentials). Nernst: E = $E_{standard}$ - $\frac{0.0592}{n}$log(Q) at 25 C. At equilibrium: E = 0, $E_{standard}$ = $\frac{0.0592}{n}$log(K). Thermodynamics: $delta_G$ = -nFE, delta_G_{standard} = -$nFE_{standard}$ = -RTln(K). Entropy: $delta_S$ = nF$\frac{dE}{dT}$. Faraday: m = $\frac{MIt}{nF}$, 1 F = 96485 C. Conductance: G = 1/R (S), kappa = G*$\frac{l}{A}$ $\frac{S}{cm}$. $Lambda_m$ = kappa*1000/C (S.$cm^2$/mol). Kohlrausch: Lambda_m_{infinity} = nu+*lambda+ + nu-*lambda-. Dissociation: alpha = \frac{Lambda_m}{Lambda_m_infinity}. Concentration cell: E = $\frac{0.0592}{n}$log$\frac{C_high}{C_low}$. Quick conversions: 1 F deposits 108 g Ag, 31.75 g Cu, 9 g Al. Volume at STP: 1 mol gas = 22.4 L. 0.0592/n gives the voltage change per decade of Q.