Predict the anode, cathode, and overall cell reactions when an aqueous solution of each of the following salts is electrolyzed in a cell having inert electrodes. (a) Ag2SO4

Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In an electrolytic cell, an external voltage is applied to facilitate the movement of ions in an electrolyte solution, leading to the oxidation and reduction reactions at the electrodes. The anode is where oxidation occurs, while the cathode is where reduction takes place.

Inert electrodes, such as platinum or graphite, do not participate in the chemical reactions occurring during electrolysis. Their primary function is to provide a surface for the oxidation and reduction reactions to occur without themselves being consumed or altered. This allows for the accurate observation of the reactions involving the electrolyte.

Half-reactions are the individual oxidation and reduction processes that occur at the electrodes during electrolysis. For the electrolysis of Ag2SO4, the half-reaction at the anode involves the oxidation of sulfate ions, while at the cathode, silver ions are reduced to form metallic silver. Understanding these half-reactions is crucial for predicting the overall cell reactions.