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A galvanic cell (also known as a voltaic cell)is a device that generates electrical energy from spontaneous redox reactions. It consists of two half-cells, each containing an electrode and an electrolyte. The two electrodes are connected by a wire that allows the flow of electrons from one half-cell to the other, and the electrolytes allow the flow of ions to complete the circuit.

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In a galvanic cell, the anode undergoes oxidation (loses electrons), while the cathode undergoes reduction (gains electrons).

The electrons flow from the anode to the cathode through an external circuit.

The ion flow between the half-cells occurs through a salt bridge or porous membrane that maintains electrical neutrality.

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A battery is a device that stores chemical energy and converts it into electrical energy via electrochemical reactions. It consists of one or more galvanic cells connected in series or parallel to provide a required voltage and current.

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Batteries work based on redox reactions.When a battery is used, one electrode loses electrons (oxidation) and the other gains electrons (reduction). This movement of electrons through an external circuit generates an electric current.

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Galvanic cells, also known as voltaic cells, are electrochemical devices that convert chemical energy into electrical energy. They are classified into two main types: primary batteries, which are single-use and non-rechargeable, and secondary batteries, which are rechargeable and can be used multiple times. These cells play a crucial role in powering a wide range of devices, from household electronics to electric vehicles

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1. Alkaline Battery

Redox Reaction

Anode: Zn(s) + 2OH (aq) → Zn(OH)2(aq) +2e-

Cathode: 2MnO2(s) + 2e¯ + 2H2O(l) → Mn2O3(s) + 2OH-(aq)

Applications: Common in remote controls, clocks, and small electronic devices.

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2. Zinc-Carbon Battery

Redox Reaction

Anode: Zn(s) → Zn2+(aq) + 2e

Cathode: 2MnO2(s) + 2e¯ + 2H2O(l) → Mn2O3(s) + 2OH (aq)

• Applications: Used in flashlights, radios, and toys.

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1. Lithium-Ion (Li-ion) Battery:

Redox Reaction:

Anode: LiC6 → Li+ + e¯ + C6

Cathode: LiCoO2 + e¯ + Li+ → Li2C0O2

• Applications: Used in smartphones, laptops, and electric vehicles.

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2. Nickel-Cadmium (NiCd) Battery:

Redox Reaction:

Anode: 2NiO(OH) + 2H2O + 2e- → 2Ni(OH)2 + 2OH

Cathode: Cd(OH)2 + 2e¯→ Cd+ 2OH-

Applications: Used in power tools, cameras, and other portable devices.

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3. Nickel-Metal Hydride (NiMH) Battery:

Redox Reaction:

Anode: 2Ni(OH)2 + 2e¯ → 2NiO(OH) + 2H2O

Cathode: 2H2 + 2e¯ → 2H2O

Applications: Used in hybrid cars, digital cameras, and other devices requiring moderate power

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1. Portable Power Sources

Batteries power everyday devices like smartphones, laptops, cameras, and watches.

2. Electric Vehicles

Lithium-ion and other rechargeable batteries are used in electric cars and e-bikes.

3. Renewable Energy Storage

Batteries like lead-acid and lithium-ion store energy from renewable sources like solar and wind for later use.

4. Medical Devices

Batteries power medical equipment like pacemakers, hearing aids, and glucose monitors.

5. Military Applications

Used in remote sensors, communication devices, and backup systems.

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TechExplained, A. (2022). What are batteries and how do they work? YouTube. [https://www.youtube.com/watch?v=examplelink](https://www.youtube.com/watch?v=examplelink)

TechExplained. (2022). What are batteries and how do they work? YouTube. [https://www.youtube.com/watch?v=examplelink](https://www.youtube.com/watch?v=examplelink)

ElectroChemistry101, K. (2022). The role of zinc in batteries. YouTube. [https://www.youtube.com/watch?v=examplelink](https://www.youtube.com/watch?v=examplelink)

TechExplained. (2023). Applications of Galvanic Cells in Everyday Life. YouTube. [https://www.youtube.com/watch?v=examplelink](https://www.youtube.com/watch?v=examplelink)

ScienceExplained. (2022). What are Galvanic Cells and How Do They Work? YouTube. [https://www.youtube.com/watch?v=examplelink](https://www.youtube.com/watch?v=examplelink)