Electrochemical cells are crucial for converting chemical energy to electrical energy and vice versa. This overview discusses Galvanic and electrolytic cells, their anode and cathode functions, and applications like batteries and electrolysis. The role of these cells in sustainable energy, particularly hydrogen fuel production, is also highlighted.
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Galvanic cells generate electrical energy from spontaneous chemical reactions
Electrolytic cells consume electrical energy to drive nonspontaneous chemical reactions
Galvanic cells have a negative anode and positive cathode, while electrolytic cells have a positive anode and negative cathode
The anode is the source of electrons and the cathode is the electron acceptor in electrochemical cells
The anode releases electrons in oxidation reactions, while the cathode consumes electrons in reduction reactions
Diagrams show the source of electrical energy and the direction of electron flow in electrochemical cells
Galvanic cells are used in disposable batteries and can power electronic devices
Electrolytic cells are used in rechargeable batteries and in processes such as electrolysis of water for hydrogen production
Electrochemical cells, particularly electrolytic cells, play a crucial role in producing clean energy and reducing reliance on nonrenewable sources
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Purpose of Galvanic vs. Electrolytic Cells
Galvanic cells convert chemical energy to electrical energy; electrolytic cells use electrical energy to drive chemical reactions.
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Anode and Cathode in Galvanic Cells
In Galvanic cells, anode is negative and supplies electrons; cathode is positive and accepts electrons.
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Anode and Cathode in Electrolytic Cells
In electrolytic cells, anode is positive due to external current; cathode is negative and receives electrons.
