Domanda del libro di testo
Sketch a cell with inert electrodes suitable for electrolysis of aqueous CuBr2.
(b) Indicate the direction of electron and ion flow.
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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 37
Consider a Daniell cell with 1.0 M ion concentrations: 
Does the cell voltage increase, decrease, or remain the same when each of the following changes is made? Explain.
(a) Write a balanced equation for each cell reaction.
Guida verificata passo dopo passo1
Identify the half-reactions occurring at the anode and cathode. The anode is where oxidation occurs, and the cathode is where reduction occurs.
Write the oxidation half-reaction at the anode: Zn(s) → Zn²⁺(aq) + 2e⁻.
Write the reduction half-reaction at the cathode: Cu²⁺(aq) + 2e⁻ → Cu(s).
Combine the half-reactions to write the overall balanced cell reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s).
Analyze how changes in ion concentrations or other conditions would affect the cell voltage based on the Nernst equation.
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Electrochemical Cells
Electrochemical cells, such as the Daniell cell, convert chemical energy into electrical energy through redox reactions. In a Daniell cell, zinc acts as the anode where oxidation occurs, while copper acts as the cathode where reduction takes place. The flow of electrons from the anode to the cathode generates an electric current, which can be measured as voltage.
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Percorso guidato
02:46
Electrochemical Cells
Half-Reactions
Half-reactions represent the individual oxidation and reduction processes occurring in an electrochemical cell. For the Daniell cell, the oxidation half-reaction involves zinc losing electrons to form zinc ions (Zn → Zn²⁺ + 2e⁻), while the reduction half-reaction involves copper ions gaining electrons to form solid copper (Cu²⁺ + 2e⁻ → Cu). Balancing these half-reactions is essential for understanding the overall cell reaction.
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01:49First-Order Half-Life
Nernst Equation
The Nernst equation relates the cell potential to the concentrations of the reactants and products in an electrochemical reaction. It shows how changes in ion concentration affect the voltage of the cell. For a Daniell cell, increasing the concentration of reactants (like Zn²⁺ or Cu²⁺) can lead to an increase in cell voltage, while decreasing their concentrations can lower the voltage, illustrating the dynamic nature of electrochemical systems.
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01:17The Nernst Equation
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How are standard reduction potentials defined?
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Domanda del libro di testo
The silver oxide–zinc battery used in watches delivers a voltage of 1.60 V. Calculate the free-energy change (in kilo-joules) for the cell reaction
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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.
(c) Write balanced equations for the anode, cathode, and overall cell reactions.
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Domanda del libro di testo
Calculate the standard cell potential and the standard free-energy change (in kilojoules) for the reaction below. (See Appendix D for standard reduction potentials.) <QUESTION REFERENCES APPENDIX D>
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Domanda del libro di testo
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.
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