Textbook Question
What products are obtained in the electrolysis of a molten mixture of KI and KBr?
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Ch.19 - Electrochemistry
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving107
- Ch.2 - Atoms & Elements100
- Ch.3 - Molecules, Compounds & Chemical Equations127
- Ch.4 - Chemical Quantities & Aqueous Reactions114
- Ch.5 - Gases103
- Ch.6 - Thermochemistry92
- Ch.7 - Quantum-Mechanical Model of the Atom50
- Ch.8 - Periodic Properties of the Elements89
- Ch.9 - Chemical Bonding I: The Lewis Model84
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory74
- Ch.11 - Liquids, Solids & Intermolecular Forces60
- Ch.12 - Solids and Modern Material50
- Ch.13 - Solutions90
- Ch.14 - Chemical Kinetics111
- Ch.15 - Chemical Equilibrium65
- Ch.16 - Acids and Bases135
- Ch.17 - Aqueous Ionic Equilibrium145
- Ch.18 - Free Energy and Thermodynamics92
- Ch.19 - Electrochemistry100
- Ch.20 - Radioactivity and Nuclear Chemistry68
- Ch.21 - Organic Chemistry121
Chapter 19, Problem 96b,c
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. b. KCl(aq) c. CuBr2(aq)
Verified step by step guidance1
Step 1: Identify the ions present in the aqueous solution of KCl. In KCl(aq), the ions are K⁺ and Cl⁻. Water (H₂O) is also present and can participate in the electrolysis reactions.
Step 2: Determine the possible half-reactions at the anode for KCl(aq). At the anode, oxidation occurs. The possible reactions are the oxidation of Cl⁻ to Cl₂ gas and the oxidation of water to oxygen gas.
Step 3: Write the half-reaction for the oxidation of Cl⁻ at the anode: 2Cl⁻(aq) → Cl₂(g) + 2e⁻. This reaction is more favorable than the oxidation of water under standard conditions.
Step 4: Identify the ions present in the aqueous solution of CuBr₂. In CuBr₂(aq), the ions are Cu²⁺ and Br⁻. Water is also present.
Step 5: Determine the possible half-reactions at the cathode for CuBr₂(aq). At the cathode, reduction occurs. The possible reactions are the reduction of Cu²⁺ to Cu(s) and the reduction of water to hydrogen gas. Write the half-reaction for the reduction of Cu²⁺ at the cathode: Cu²⁺(aq) + 2e⁻ → Cu(s). This reaction is more favorable than the reduction of water under standard conditions.
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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 elements. The reactions occur at two electrodes: the anode (positive electrode) and the cathode (negative electrode), where oxidation and reduction reactions take place, respectively.
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Half-Reactions
Half-reactions are the individual oxidation or reduction reactions that occur at the electrodes during electrolysis. Each half-reaction shows the transfer of electrons and the change in oxidation states of the species involved. By writing half-reactions, one can clearly identify what is being oxidized at the anode and what is being reduced at the cathode, which is essential for understanding the overall electrochemical process.
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Electrolyte Solutions
Electrolyte solutions are aqueous solutions that contain ions, which are necessary for conducting electricity. The nature of the electrolyte affects the products formed during electrolysis. For example, in KCl(aq), chloride ions can be oxidized at the anode, while in CuBr2(aq), copper ions can be reduced at the cathode, leading to different half-reactions based on the specific ions present in the solution.
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Related Practice
Textbook Question
Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag+(aq) + e– → Ag(s) What mass of silver would plate onto the cathode if a current of 6.8 A flowed through the cell for 72 min?
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Textbook Question
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. a. NaBr(aq) b. PbI2(aq) c. Na2SO4(aq)
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Textbook Question
Make a sketch of an electrolysis cell that electroplates copper onto other metal surfaces. Label the anode and the cathode and indicate the reactions that occur at each.
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Textbook Question
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each aqueous solution. a. Ni(NO3)2(aq)
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