Domanda del libro di testo
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (b) Pt2+ (aq) → Pt(s)
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Ch.19 - Electrochemistry
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 19, Problema 40a
Porous pellets of TiO2 can be reduced to titanium metal at the cathode of an electrochemical cell containing molten CaCl2 as the electrolyte. When the TiO2 is reduced, the O2-ions dis-solve in the CaCl2 and are subsequently oxidized to O2 gas at the anode. This approach may be the basis for a less expensive process than the one currently used for producing titanium.
(a) Label the anode and cathode, and indicate the signs of the electrodes.
Guida verificata passo dopo passo1
Identify the cathode and anode in the electrochemical cell. The cathode is where reduction occurs, and the anode is where oxidation occurs.
In this process, TiO2 is reduced to titanium metal at the cathode. Therefore, the cathode is the site of reduction.
The O2- ions are oxidized to O2 gas at the anode. Therefore, the anode is the site of oxidation.
In an electrochemical cell, the cathode is typically the negative electrode because it attracts cations (positive ions) and provides electrons for reduction.
Conversely, the anode is typically the positive electrode because it attracts anions (negative ions) and is the site where electrons are released during oxidation.
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Electrochemical Cells
Electrochemical cells consist of two electrodes, the anode and cathode, where oxidation and reduction reactions occur. The anode is where oxidation takes place, losing electrons, while the cathode is where reduction occurs, gaining electrons. Understanding the flow of electrons and the reactions at each electrode is crucial for analyzing the cell's function.
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02:46
Electrochemical Cells
Oxidation and Reduction
Oxidation refers to the loss of electrons, while reduction is the gain of electrons. In the context of the electrochemical cell described, the TiO2 is reduced to titanium at the cathode, and the O2- ions are oxidized to O2 gas at the anode. Recognizing these processes is essential for identifying the roles of the electrodes in the cell.
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01:53Oxidation and Reduction Reactions
Electrode Sign Convention
In electrochemical cells, the anode is conventionally assigned a positive sign in galvanic cells and a negative sign in electrolytic cells, while the cathode is the opposite. In this case, since the process involves electrolysis (reduction of TiO2), the cathode will be negative, and the anode will be positive. Understanding this convention helps in correctly labeling the electrodes.
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01:34Electron Affinity
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Porous pellets of TiO2 can be reduced to titanium metal at the cathode of an electrochemical cell containing molten CaCl2 as the electrolyte. When the TiO2 is reduced, the O2-ions dis-solve in the CaCl2 and are subsequently oxidized to O2 gas at the anode. This approach may be the basis for a less expensive process than the one currently used for producing titanium.
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