In \(Cu - Ag\) electrochemical cell \(Cu\) acts as

Anode

In a copper-silver electrochemical cell, copper acts as the (1) anode.

An anode is the electrode where oxidation takes place. In this case, copper is oxidized to copper ions:

\(Cu (s) \longrightarrow Cu^{2+} (aq) + 2e^-\)

The electrons released from the oxidation of copper flow through the external circuit to the silver electrode, where they are reduced to silver atoms:

\(Ag^+ (aq) + e^- \longrightarrow Ag (s)\)

Therefore, the copper electrode is the anode in the copper-silver electrochemical cell.

The other options are incorrect:

• The cathode is the electrode where reduction takes place.
• The salt bridge is a device that connects the two half-cells and allows for the flow of ions.
• The electrolyte is the solution that contains the ions that are involved in the redox reaction.