Some Chemistry key terms and definitions related to the electrolysis of aqueous solutions:
1. Electrolysis: A chemical process that uses electrical energy to drive a non-spontaneous chemical reaction. This process involves the decomposition of a compound into its elements or simpler compounds using electricity.
2. Electrolyte: A substance that dissociates into ions when dissolved in water, allowing the solution to conduct electricity. Common electrolytes include salts, acids, and bases.
3. Electrode: A conductor through which electricity enters or leaves an electrolyte solution. There are two types of electrodes:
• Anode: The positive electrode where oxidation occurs (loss of electrons).
• Cathode: The negative electrode where reduction occurs (gain of electrons).
4. Ions: Charged particles that result from the dissociation of electrolytes in solution. Cations are positively charged ions, while anions are negatively charged ions.
5. Oxidation: A chemical reaction that involves the loss of electrons by a substance. In electrolysis, oxidation occurs at the anode.
6. Reduction: A chemical reaction that involves the gain of electrons by a substance. In electrolysis, reduction occurs at the cathode.
7. Half-Reaction: A representation of either the oxidation or reduction process occurring at an electrode during electrolysis. Half-reactions show the transfer of electrons and can be combined to form the overall reaction.
8. Faraday's Laws of Electrolysis: Two laws that quantify the relationship between the amount of substance transformed during electrolysis and the quantity of electric charge passed through the electrolyte:
• First Law: The mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
• Second Law: The mass of different substances altered by the same quantity of electricity is proportional to their equivalent weights.
9. Electrolytic Cell: A device used to carry out electrolysis, consisting of two electrodes immersed in an electrolyte solution connected to a power source.
10. Conductivity: The ability of a solution to conduct electric current, which depends on the concentration and type of ions present in the solution.
11. Electroplating: A process that uses electrolysis to deposit a layer of metal onto a surface, often used for decorative purposes or to prevent corrosion.
12. Hydrolysis: A chemical reaction involving water that results in the breakdown of a compound into its constituent parts, often associated with electrolysis.
13. pH: A measure of the acidity or basicity of a solution, which can influence the products formed during electrolysis, especially in aqueous solutions.
14. Gas Evolution: The production of gases at the electrodes during electrolysis, such as hydrogen gas (H₂) at the cathode and oxygen gas (O₂) at the anode when water is electrolyzed.
15. Electrode Potential: The tendency of an electrode to gain or lose electrons, measured in volts. Standard electrode potentials are used to predict the direction of redox reactions.
16.Electrosynthesis: is the use of electrical energy to drive chemical reactions, resulting in the synthesis of organic or inorganic compounds.
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1. Electrolysis: A chemical process that uses electrical energy to drive a non-spontaneous chemical reaction. This process involves the decomposition of a compound into its elements or simpler compounds using electricity.
2. Electrolyte: A substance that dissociates into ions when dissolved in water, allowing the solution to conduct electricity. Common electrolytes include salts, acids, and bases.
3. Electrode: A conductor through which electricity enters or leaves an electrolyte solution. There are two types of electrodes:
• Anode: The positive electrode where oxidation occurs (loss of electrons).
• Cathode: The negative electrode where reduction occurs (gain of electrons).
4. Ions: Charged particles that result from the dissociation of electrolytes in solution. Cations are positively charged ions, while anions are negatively charged ions.
5. Oxidation: A chemical reaction that involves the loss of electrons by a substance. In electrolysis, oxidation occurs at the anode.
6. Reduction: A chemical reaction that involves the gain of electrons by a substance. In electrolysis, reduction occurs at the cathode.
7. Half-Reaction: A representation of either the oxidation or reduction process occurring at an electrode during electrolysis. Half-reactions show the transfer of electrons and can be combined to form the overall reaction.
8. Faraday's Laws of Electrolysis: Two laws that quantify the relationship between the amount of substance transformed during electrolysis and the quantity of electric charge passed through the electrolyte:
• First Law: The mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
• Second Law: The mass of different substances altered by the same quantity of electricity is proportional to their equivalent weights.
9. Electrolytic Cell: A device used to carry out electrolysis, consisting of two electrodes immersed in an electrolyte solution connected to a power source.
10. Conductivity: The ability of a solution to conduct electric current, which depends on the concentration and type of ions present in the solution.
11. Electroplating: A process that uses electrolysis to deposit a layer of metal onto a surface, often used for decorative purposes or to prevent corrosion.
12. Hydrolysis: A chemical reaction involving water that results in the breakdown of a compound into its constituent parts, often associated with electrolysis.
13. pH: A measure of the acidity or basicity of a solution, which can influence the products formed during electrolysis, especially in aqueous solutions.
14. Gas Evolution: The production of gases at the electrodes during electrolysis, such as hydrogen gas (H₂) at the cathode and oxygen gas (O₂) at the anode when water is electrolyzed.
15. Electrode Potential: The tendency of an electrode to gain or lose electrons, measured in volts. Standard electrode potentials are used to predict the direction of redox reactions.
16.Electrosynthesis: is the use of electrical energy to drive chemical reactions, resulting in the synthesis of organic or inorganic compounds.
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