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Questions and Answers
What role does the anode play in an electrical cell?
What role does the anode play in an electrical cell?
- It is the substance facilitating ion flow between electrodes.
- It is the positive electrode where ions flow through.
- It is the negative electrode where oxidation occurs. (correct)
- It is the positive electrode where reduction occurs.
What differentiates a galvanic cell from an electrolytic cell?
What differentiates a galvanic cell from an electrolytic cell?
- A galvanic cell drives a non-spontaneous reaction.
- A galvanic cell generates an electric current from a spontaneous reaction. (correct)
- A galvanic cell uses a salt bridge to facilitate ion flow.
- A galvanic cell requires an external electric current.
What is the function of the salt bridge in an electrical cell?
What is the function of the salt bridge in an electrical cell?
- To allow ions to flow between the two half-cells. (correct)
- To connect the anode and cathode directly.
- To provide a path for electrons between electrodes.
- To measure the potential difference between electrodes.
Which component of an electrical cell gains electrons during the reaction?
Which component of an electrical cell gains electrons during the reaction?
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What is measured in volts (V) in an electrical cell?
What is measured in volts (V) in an electrical cell?
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Why are electrical cells important in modern applications?
Why are electrical cells important in modern applications?
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Study Notes
Basics of Electrical Cells
- An electrical cell, also known as a voltaic cell, is a device that generates an electric current from chemical reactions.
- It consists of two half-cells: an anode (negative electrode) and a cathode (positive electrode) immersed in an electrolyte.
Types of Electrical Cells
- Galvanic Cell: A spontaneous reaction occurs between the anode and cathode, generating an electric current.
- Electrolytic Cell: An external electric current is applied to the cell, driving a non-spontaneous reaction.
Key Components of an Electrical Cell
- Anode: The negative electrode where oxidation occurs, releasing electrons.
- Cathode: The positive electrode where reduction occurs, gaining electrons.
- Electrolyte: A substance that facilitates the flow of ions between the anode and cathode.
- Salt Bridge: A U-shaped tube that connects the two half-cells, allowing ions to flow between them.
Cell Potential
- The potential difference between the anode and cathode, measured in volts (V).
- It is the driving force behind the electric current generated by the cell.
Importance of Electrical Cells
- Provide a portable source of electricity.
- Used in various applications, including batteries, fuel cells, and electrolysis.
Basics of Electrical Cells
- An electrical cell generates an electric current from chemical reactions between two half-cells.
- The half-cells consist of an anode (negative electrode) and a cathode (positive electrode) immersed in an electrolyte.
Types of Electrical Cells
- Galvanic cells generate an electric current through a spontaneous reaction between the anode and cathode.
- Electrolytic cells require an external electric current to drive a non-spontaneous reaction.
Key Components of an Electrical Cell
- Anodes are negative electrodes where oxidation occurs, releasing electrons.
- Cathodes are positive electrodes where reduction occurs, gaining electrons.
- Electrolytes facilitate the flow of ions between the anode and cathode.
- Salt bridges are U-shaped tubes that connect the two half-cells, allowing ions to flow between them.
Cell Potential
- Cell potential is the potential difference between the anode and cathode, measured in volts (V).
- It is the driving force behind the electric current generated by the cell.
Importance of Electrical Cells
- Electrical cells provide a portable source of electricity.
- They are used in various applications, including batteries, fuel cells, and electrolysis.
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