Textbook Question
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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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 19, Problem 38
Sketch a cell with inert electrodes suitable for electrolysis of aqueous CuBr2. (b) Indicate the direction of electron and ion flow.
Verified step by step guidance1
insert step 1: Identify the components of the electrolysis cell. You will need an electrolyte solution, which is aqueous CuBr2, and inert electrodes, such as platinum or graphite, to conduct electricity.
insert step 2: Sketch the electrolysis cell. Draw a container to represent the electrolyte solution, and place the two inert electrodes into the solution. Label one electrode as the anode and the other as the cathode.
insert step 3: Determine the reactions at each electrode. At the anode, oxidation occurs, and at the cathode, reduction occurs. For CuBr2, copper ions (Cu^2+) will be reduced at the cathode, and bromide ions (Br^-) will be oxidized at the anode.
insert step 4: Indicate the direction of electron flow. Electrons flow from the anode to the cathode through the external circuit.
insert step 5: Indicate the direction of ion flow. In the solution, Cu^2+ ions move towards the cathode to gain electrons, and Br^- ions move towards the anode to lose electrons.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 into its constituent ions. For aqueous CuBr2, electrolysis will lead to the formation of copper and bromine at the respective electrodes.
Recommended video:
Guided course
01:21
The Electrolytic Cell
Inert Electrodes
Inert electrodes, such as platinum or graphite, do not participate in the chemical reactions occurring during electrolysis. Their primary function is to conduct electricity and facilitate the transfer of electrons to the ions in the electrolyte. This allows the electrochemical reactions to occur without the electrode material being consumed or altered.
Ion and Electron Flow
During electrolysis, ions move towards the electrodes of opposite charge: cations (positive ions) migrate to the cathode (negative electrode) to gain electrons, while anions (negative ions) move to the anode (positive electrode) to lose electrons. This flow of ions and electrons is essential for the electrochemical reactions that lead to the production of elements or compounds from the electrolyte.
Recommended video:
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00:35Anion Electron Configuration
Related Practice
Textbook Question
How are standard reduction potentials defined?
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Textbook Question
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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Textbook Question
Classify each of the following unbalanced half-reactions as either an oxidation or a reduction. (b) H2O2(aq) → O2(g)
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Textbook Question
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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Textbook Question
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.
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