First Law: mass deposited is proportional to charge passed. m = ZIt = $\frac{MIt}{nF}$. Z = $\frac{M}{nF}$ is the electrochemical equivalent. Second Law: for same charge through different electrolytes, masses deposited are proportional to equivalent weights $\frac{M}{n}$. 1 Faraday (F) = 96485 C = charge carried by 1 mole of electrons. 1 F deposits: 108 g Ag (n=1), 31.75 g Cu (n=2), 9 g Al (n=3). Charge Q = It (current x time). Always convert time to seconds. For series electrolytic cells (same current), compare masses using equivalent weights. For parallel cells (same voltage), currents may differ.