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. (b) CuCl₂

Key Concepts

Electrolysis

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. Understanding electrolysis is crucial for predicting the products formed during the electrolysis of compounds like CuCl2.

Anode and Cathode Reactions

In electrolysis, the anode is the electrode where oxidation occurs, while the cathode is where reduction takes place. For CuCl2, at the anode, chloride ions (Cl-) are oxidized to chlorine gas (Cl2), and at the cathode, copper ions (Cu2+) are reduced to solid copper (Cu). Identifying these reactions is essential for predicting the overall cell reaction.

Inert Electrodes

Inert electrodes, such as platinum or graphite, do not participate in the chemical reactions occurring during electrolysis. Their primary role is to provide a surface for the oxidation and reduction reactions without interfering with the electrolyte's chemistry. Understanding the function of inert electrodes helps clarify how the electrolysis process proceeds without altering the composition of the electrodes themselves.