Domanda del libro di testo
Consider the following table of standard electrode potentials for a series of hypothetical reactions in an aqueous solution: reduction half-reaction E °(V) (c) Which substance(s) can oxidize C2+?
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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 9
(a) What is an electrolytic cell? (b) The negative terminal of a voltage source is connected to an electrode of an electrolytic cell. Is the electrode the anode or the cathode of the cell? Explain.
Guida verificata passo dopo passo1
Step 1: Understand the concept of an electrolytic cell. An electrolytic cell is a type of electrochemical cell that uses electrical energy to drive a non-spontaneous chemical reaction. It consists of two electrodes (anode and cathode) immersed in an electrolyte solution.
Step 2: Identify the role of the electrodes in an electrolytic cell. In an electrolytic cell, the anode is the electrode where oxidation occurs, and the cathode is the electrode where reduction occurs.
Step 3: Determine the connection of the voltage source. In an electrolytic cell, the negative terminal of the voltage source is connected to the cathode, and the positive terminal is connected to the anode.
Step 4: Explain the reasoning. The negative terminal of the voltage source provides electrons, which flow to the cathode, causing reduction to occur at the cathode. Therefore, the electrode connected to the negative terminal is the cathode.
Step 5: Summarize the findings. In an electrolytic cell, the electrode connected to the negative terminal of the voltage source is the cathode, where reduction takes place.
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Electrolytic Cell
An electrolytic cell is a type of electrochemical cell that uses an external voltage source to drive a non-spontaneous chemical reaction. In this cell, electrical energy is converted into chemical energy, facilitating processes such as electrolysis. The cell consists of two electrodes immersed in an electrolyte solution, where oxidation occurs at the anode and reduction occurs at the cathode.
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01:21
The Electrolytic Cell
Electrode Designation
In an electrolytic cell, the electrodes are designated as anode and cathode based on the direction of electron flow. The anode is the electrode where oxidation occurs, and it is connected to the positive terminal of the voltage source. Conversely, the cathode is where reduction takes place and is connected to the negative terminal, attracting cations from the electrolyte.
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04:44Electron Geometry
Current Flow and Electrode Behavior
The behavior of electrodes in an electrolytic cell is influenced by the flow of current. When the negative terminal of a voltage source is connected to an electrode, that electrode becomes the cathode, where reduction occurs. This is because electrons flow from the negative terminal to the cathode, allowing cations in the electrolyte to gain electrons and be reduced.
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04:44Electron Geometry
Pratica correlata
Domanda del libro di testo
Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (a) What is the most common oxidation number for Mg when it is part of a salt?
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Domanda del libro di testo
The electrodes in a silver oxide battery are silver oxide 1Ag2O2 and zinc (b) Which battery do you think has an energy density most similar to the silver oxide battery: a Li-ion battery, a nickel– cadmium battery, or a lead–acid battery? [Section 20.7]
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Domanda del libro di testo
Consider the following voltaic cell:
(c) What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10?
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Domanda del libro di testo
Bars of iron are put into each of the three beakers as shown here. In which beaker—A, B, or C—would you expect the iron to show the most corrosion ? [Section 20.8]
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