Domanda del libro di testo
(b) What amperage is required to plate out 0.250 mol Cr from a Cr3+ solution in a period of 8.00 h?
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Ch.20 - Electrochemistry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 20, Problema 94d
(d) Why are active metals such as Al obtained by electrolysis using molten salts rather than aqueous solutions?
Guida verificata passo dopo passo1
Understand that active metals like aluminum (Al) are highly reactive and tend to form stable compounds.
Recognize that in aqueous solutions, water is present and can participate in redox reactions.
Consider the electrochemical series: water is more easily reduced than many metal ions, including Al³⁺, meaning water would preferentially undergo reduction to form hydrogen gas instead of reducing Al³⁺ to Al.
Realize that using molten salts allows the metal ions to be reduced without the interference of water, as there is no water present to compete in the reduction process.
Conclude that electrolysis of molten salts provides a more efficient and feasible method to obtain pure active metals like aluminum, as it avoids the side reactions that occur in aqueous solutions.
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Electrolysis
Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In this process, an electric current is passed through an electrolyte, causing the decomposition of the compound. This technique is essential for extracting metals from their ores, particularly for active metals that cannot be easily reduced by chemical means.
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Percorso guidato
01:21
The Electrolytic Cell
Molten Salts vs. Aqueous Solutions
Molten salts are ionic compounds that are heated until they become liquid, allowing ions to move freely. In contrast, aqueous solutions contain water as a solvent, which can introduce complications such as competing reactions with water. For active metals like aluminum, using molten salts prevents the formation of hydrogen gas and ensures a more efficient extraction process.
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01:11Types of Aqueous Solutions
Reactivity of Active Metals
Active metals, such as aluminum, have a strong tendency to lose electrons and form positive ions. This high reactivity makes them difficult to extract using traditional methods, as they readily react with water and other substances. Electrolysis of molten salts allows for the direct reduction of these metals without interference from other reactions, making it a preferred method for their extraction.
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02:02Activity Series Chart
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(a) A Cr3+(aq) solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out after 2.00 days?
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