Electrochemical cell
An electrochemical cell is a device that uses redox (reduction-oxidation) reactions to either produce or consume electrical energy.
These cells come in two main types:
To understand how a voltaic cell operates, let’s break it down into its key components:
Electrodes
Electrodes are solid surfaces where the redox reactions occur
Salt bridge
The salt bridge is a tube or porous material filled with an ionic solution (e.g., KNO₃ or Na₂SO₄). It allows ions to flow between the two half-cells, maintaining electrical neutrality and completing the circuit.
Without a salt bridge, the buildup of charges in the half-cells would prevent the flow of electrons, effectively stopping the redox reaction.
Each half-cell contains a solution with ions of the metals involved in the redox reaction.
In a zinc-copper cell, the anode is immersed in a solution of Zn²⁺ ions (e.g., ZnSO₄), and the cathode is immersed in a solution of Cu²⁺ ions (e.g., CuSO₄).
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