Galvanic Cells - Full Explanation
Galvanic Cells - Full Explanation
Introduction to Galvanic Cells
A Galvanic cell (also called a voltaic cell) is an electrochemical cell that generates electrical energy
from a
spontaneous redox reaction. It is the basis of batteries used in everyday applications.
Components of a Galvanic Cell:
1. Two Electrodes: Anode (negative) and Cathode (positive).
2. Electrolytes: Solutions that conduct ions.
3. Salt Bridge: Maintains electrical neutrality by allowing ion flow.
4. External Circuit: Connects the electrodes, allowing electrons to flow.
Working Principle:
- The anode undergoes oxidation (loses electrons).
- The cathode undergoes reduction (gains electrons).
- Electrons flow from the anode to the cathode through an external circuit, generating electricity.
Example: Daniell Cell
- Anode Reaction (Zinc Electrode in ZnSO4 Solution):
Zn -> Zn2+ + 2e-
- Cathode Reaction (Copper Electrode in CuSO4 Solution):
Cu2+ + 2e- -> Cu
- Overall Reaction:
Zn + Cu2+ -> Zn2+ + Cu
Applications of Galvanic Cells:
- Batteries (e.g., alkaline, lithium-ion, lead-acid).
- Corrosion prevention.
- Powering electronic devices.
Conclusion:
Galvanic cells are essential for converting chemical energy into electrical energy efficiently.
Understanding their
Galvanic Cells - Full Explanation
Introduction to Galvanic Cells
A Galvanic cell (also called a voltaic cell) is an electrochemical cell that generates electrical energy
from a
spontaneous redox reaction. It is the basis of batteries used in everyday applications.
Components of a Galvanic Cell:
1. Two Electrodes: Anode (negative) and Cathode (positive).
2. Electrolytes: Solutions that conduct ions.
3. Salt Bridge: Maintains electrical neutrality by allowing ion flow.
4. External Circuit: Connects the electrodes, allowing electrons to flow.
Working Principle:
- The anode undergoes oxidation (loses electrons).
- The cathode undergoes reduction (gains electrons).
- Electrons flow from the anode to the cathode through an external circuit, generating electricity.
Example: Daniell Cell
- Anode Reaction (Zinc Electrode in ZnSO4 Solution):
Zn -> Zn2+ + 2e-
- Cathode Reaction (Copper Electrode in CuSO4 Solution):
Cu2+ + 2e- -> Cu
- Overall Reaction:
Zn + Cu2+ -> Zn2+ + Cu
Applications of Galvanic Cells:
- Batteries (e.g., alkaline, lithium-ion, lead-acid).
- Corrosion prevention.
- Powering electronic devices.
Conclusion:
Galvanic cells are essential for converting chemical energy into electrical energy efficiently.
Understanding their
