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Voltalic cell
Original price was: $ 19.50.$ 19.35Current price is: $ 19.35.
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A Voltaic Cell, also known as a galvanic cell, is an electrochemical device that converts chemical energy into electrical energy through spontaneous redox reactions. It consists of two different metals or metal compounds (electrodes) immersed in electrolyte solutions, connected by a salt bridge or porous membrane to complete the circuit. Widely used in educational, research, and industrial laboratories, the Voltaic Cell demonstrates fundamental principles of electrochemistry, battery operation, and electron flow. Its robust design and clear setup make it essential for experiments involving voltage generation, electrochemical potentials, and energy conversion.
Description
Voltalic cell
Primary Uses
- Laboratory and Educational Applications
- Demonstrates basic principles of electrochemistry and redox reactions in chemistry and physics labs.
- Used in teaching environments to illustrate the conversion of chemical energy to electrical energy.
- Supports experiments measuring electrode potentials and cell voltages.
- Facilitates studies on corrosion, electroplating, and battery chemistry.
- Employed in calibrating and testing electrodes and sensors in analytical laboratories.
Secondary Uses
- Research and Industrial Applications
- Used in research to develop and test new battery materials and designs.
- Supports industrial processes requiring electrochemical reactions, such as metal finishing and refining.
- Utilized in environmental monitoring involving electrochemical sensors.
- Applied in electrochemical synthesis and energy storage research.
KEY PRODUCT FEATURES
1.Basic Identification Attributes
- Components: Two electrodes (metals or metal compounds), electrolytes, salt bridge or membrane
- Output: Produces a measurable voltage from spontaneous redox reactions
- Configuration: Typically consists of two half-cells connected externally and internally
2.Physical & Chemical Properties
- Electrochemical Behavior: Generates electrical current through redox reactions
- Materials: Common electrode metals include zinc, copper, and graphite
- Electrolytes: Solutions such as sulfuric acid, copper sulfate, or salt solutions depending on the cell type
3.Safety & Hazard Attributes
- Handle acidic or basic electrolytes with care to prevent chemical burns.
- Risk of electrical shock from cell voltage, though generally low in typical lab cells.
- Proper disposal of electrolyte solutions to avoid environmental harm.
4.Storage & Handling Attributes
- Store electrodes and electrolytes separately when not in use to prevent degradation.
- Handle with gloves and protective eyewear during assembly and disassembly.
- Dispose of used electrolytes and materials according to laboratory chemical waste protocols.
5.Regulatory & Compliance Attributes
- Manufactured and used in compliance with laboratory safety and chemical handling standards.
- Suitable for use in GLP and educational laboratories.
6.Environmental & Health Impact
- Electrolyte solutions may be hazardous; proper disposal is necessary to minimize environmental impact.
- Electrodes may contain metals requiring recycling or special disposal.
SAFETY HANDLING PRECAUTIONS
Safety Handling Precautions
- Use PPE including gloves and eye protection when preparing or handling electrolytes.
- Avoid direct contact with electrolyte solutions and metal electrodes.
First Aid Measures
- In case of electrolyte contact with skin or eyes, rinse immediately with plenty of water and seek medical advice if irritation persists.
- If ingested or inhaled, seek immediate medical attention.
Firefighting Measures
- Not flammable; use appropriate extinguishing media for surrounding fire.
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