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Galvanic (Voltaic) Electrochemical Cells

Key Concepts

Galvanic (Voltaic) Cell: converts chemical energy of oxidants and reductants into electrical energy
Electrodes: are conductors used to permit the flow of electrons in an electrochemical cell.
One electrode is the anode, the other is the cathode.
Anode: Oxidation occurs at anode
Anode is negative
Anode disintegrates
Cathode:Reduction occurs at cathode
Cathode is positive
Solid deposits on cathode
Salt bridge: allows for migration of ions to complete the electrical circuit
Electron Flow: from anode to cathode
Electrons flow from negative to positive
Spontaneous Reaction: E⁰ for the galvanic cell is positive

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Example : The Daniell Cell

A galvanic (voltaic) cell is a device that uses REDOX reactions to produce electricity.

In 1836 Professor John Daniell adopted a two-cell approach to produce electricity.
The Daniell Cell is divided into 2 half-cells connected by a wire and a salt bridge to complete the electrical circuit.

Anode: Zn ---> Zn²⁺ + 2e E^o = +0.76V

Cathode: Cu²⁺ + 2e ---> Cu E^o = +0.35V

Cell: Zn + Cu²⁺ ---> Zn²⁺ + Cu E^o_cell = +1.11V

At the negative anode, zinc is oxidised to zinc ions.
The zinc anode disintegrates in time.
At the positive cathode, copper ions are reduced to copper atoms.
Copper is deposited on the copper cathode in time.
Electrons flow from the zinc anode to the copper cathode.
In the overall REDOX reaction zinc is donating electrons to copper ions.
This REDOX reaction occurs spontaneously, E^o is positive.
This REDOX reaction produces 1.11V of electricity.

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