Final answer:
An electrochemical cell with Cu2+/Cu and Ag/Ag+ involves copper undergoing oxidation at the anode and silver undergoing reduction at the cathode, with a salt bridge maintaining charge balance as electricity is generated.
Step-by-step explanation:
Understanding Electrochemical Cells
An electrochemical cell comprises two half-cells, each including a redox conjugate pair of a single reactant. In a cell involving copper and silver ions - Cu2+/Cu and Ag/Ag+ - copper acts as the anode where oxidation takes place, and silver acts as the cathode where reduction occurs. The circuit between the copper and silver electrodes permits the flow of electrons, thereby generating electricity.
The Cu/Cu2+ half-cell includes solid copper foil immersed in an aqueous solution of copper nitrate, undergoing oxidation reaction Cu(s) -> Cu2+(aq) + 2e-. Conversely, the Ag/Ag+ half-cell consists of solid silver foil in an aqueous silver nitrate solution, where the reduction reaction 2Ag+ + 2e- -> 2Ag(s) occurs. Both reactions are facilitated by a salt bridge, which maintains ionic balance by allowing the transfer of inert ions while preventing the direct mixing of reactants.
The spontaneous redox reaction produces Cu2+ at the anode and consumes Ag+ at the cathode, resulting in a flow of electrons through the external circuit and the movement of ions through the salt bridge to maintain charge neutrality.