Explanation: An electrochemical cell that converts the chemical energy of spontaneous redox reactions into electrical energy is known as a galvanic cell
A galvanic cell harnesses the redox reactions occurring in the half-cells to generate an electric current. It is commonly used in batteries and other portable power sources.
A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts chemical energy into electrical energy through a redox (reduction-oxidation) reaction. It consists of two half-cells connected by a conductive pathway.
1. Half-cells: A galvanic cell consists of two half-cells, each containing an electrode and an electrolyte solution. The two half-cells are connected by a salt bridge or a porous membrane, which allows for the flow of ions.
2. Electrodes: Each half-cell has an electrode, which can be made of different materials depending on the specific galvanic cell. One electrode is called the anode, and the other is the cathode. The anode is where oxidation occurs, and it is negatively charged. The cathode is where reduction occurs, and it is positively charged.
3. Electrolyte Solution: The electrodes are immersed in an electrolyte solution that contains ions. The electrolyte solution allows for the flow of ions and completes the circuit. The ions in the solution participate in the redox reaction.
4. Redox Reaction: In a galvanic cell, a redox reaction takes place. Oxidation occurs at the anode, where the electrode loses electrons and forms positive ions. Reduction occurs at the cathode, where the electrode gains electrons and forms negative ions. This transfer of electrons generates an electric current.
5. Salt Bridge or Porous Membrane: The salt bridge or porous membrane connects the two half-cells while preventing the mixing of the electrolyte solutions. It allows for the flow of ions to maintain charge balance during the redox reaction.
6. Electrical Energy: The flow of electrons from the anode to the cathode through the external circuit creates an electric current. This electric current can be harnessed to do work or power electronic devices.
One example of a galvanic cell is the zinc-copper cell. In this cell, the zinc electrode serves as the anode, and it undergoes oxidation. The copper electrode serves as the cathode, and it undergoes reduction. The zinc electrode loses electrons and forms zinc ions, while the copper electrode gains electrons and forms copper ions. The flow of electrons from the zinc electrode to the copper electrode through the external circuit produces an electric current.
In summary, a galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through a redox reaction. It consists of two half-cells with electrodes and electrolyte solutions, connected by a salt bridge or a porous membrane. The redox reaction at the electrodes generates an electric current, which can be used to power devices or do work.
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Answer:
Galvanic cell
Explanation: An electrochemical cell that converts the chemical energy of spontaneous redox reactions into electrical energy is known as a galvanic cell
Explanation:
A galvanic cell harnesses the redox reactions occurring in the half-cells to generate an electric current. It is commonly used in batteries and other portable power sources.
A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts chemical energy into electrical energy through a redox (reduction-oxidation) reaction. It consists of two half-cells connected by a conductive pathway.
1. Half-cells: A galvanic cell consists of two half-cells, each containing an electrode and an electrolyte solution. The two half-cells are connected by a salt bridge or a porous membrane, which allows for the flow of ions.
2. Electrodes: Each half-cell has an electrode, which can be made of different materials depending on the specific galvanic cell. One electrode is called the anode, and the other is the cathode. The anode is where oxidation occurs, and it is negatively charged. The cathode is where reduction occurs, and it is positively charged.
3. Electrolyte Solution: The electrodes are immersed in an electrolyte solution that contains ions. The electrolyte solution allows for the flow of ions and completes the circuit. The ions in the solution participate in the redox reaction.
4. Redox Reaction: In a galvanic cell, a redox reaction takes place. Oxidation occurs at the anode, where the electrode loses electrons and forms positive ions. Reduction occurs at the cathode, where the electrode gains electrons and forms negative ions. This transfer of electrons generates an electric current.
5. Salt Bridge or Porous Membrane: The salt bridge or porous membrane connects the two half-cells while preventing the mixing of the electrolyte solutions. It allows for the flow of ions to maintain charge balance during the redox reaction.
6. Electrical Energy: The flow of electrons from the anode to the cathode through the external circuit creates an electric current. This electric current can be harnessed to do work or power electronic devices.
One example of a galvanic cell is the zinc-copper cell. In this cell, the zinc electrode serves as the anode, and it undergoes oxidation. The copper electrode serves as the cathode, and it undergoes reduction. The zinc electrode loses electrons and forms zinc ions, while the copper electrode gains electrons and forms copper ions. The flow of electrons from the zinc electrode to the copper electrode through the external circuit produces an electric current.
In summary, a galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through a redox reaction. It consists of two half-cells with electrodes and electrolyte solutions, connected by a salt bridge or a porous membrane. The redox reaction at the electrodes generates an electric current, which can be used to power devices or do work.
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