Topics: Fundamentals of electrochemistry; Electrochemical cells Use general chemistry rules for significant figures. 1. A cell is constructed to reduce the Ag+ in AgCl(s) to Ag(s) at the cathode when current is passed through the cell. At the anode, Cu(s) is oxidized to Cu2+. If current of 0.500 A is passed through the cell for 101 minutes, calculate the mass of Cu(s) dissolved and mass of Ag(s) deposited. Half-cell reactions: Cathode: AgCl(s) + e ⇌ Ag(s) + Cl– Anode: Cu(s) ⇌ Ce2+ + 2e

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.