Textbook Question
When the nickel–zinc battery, used in digital cameras, is recharged, the following cell reaction occurs: (a) How many grams of zinc are formed when 3.35 x 10-2 g of Ni(OH)2 are consumed?
Ch.19 - Electrochemistry
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- 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
Chapter 19, Problem 146a
In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO4(s) must be converted into PbO2(s) and Pb(s). (a) Does the reaction represent an electrolytic or galvanic cell?
Verified step by step guidance1
insert step 1> Identify the type of cell by understanding the process involved. In an electrolytic cell, electrical energy is used to drive a non-spontaneous chemical reaction, whereas in a galvanic cell, a spontaneous chemical reaction generates electrical energy.
insert step 2> Recognize that charging a battery involves reversing the discharge reaction, which is typically non-spontaneous and requires an external power source.
insert step 3> Recall that in a lead storage battery, during discharge, PbO_2 and Pb react with H_2SO_4 to form PbSO_4 and water. Charging the battery involves converting PbSO_4 back into PbO_2 and Pb.
insert step 4> Since the conversion of PbSO_4 to PbO_2 and Pb requires an input of electrical energy, this process is characteristic of an electrolytic cell.
insert step 5> Conclude that the reaction represents an electrolytic cell because it involves the input of electrical energy to drive the non-spontaneous conversion of PbSO_4 into PbO_2 and Pb.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electrolytic vs. Galvanic Cells
Electrolytic cells use electrical energy to drive a non-spontaneous chemical reaction, while galvanic cells generate electrical energy from spontaneous reactions. In electrolytic cells, an external power source is required to facilitate the reaction, whereas galvanic cells produce voltage as a result of the chemical reaction occurring spontaneously.
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The Electrolytic Cell
Lead Storage Battery Chemistry
A lead storage battery operates through the reversible reactions of lead dioxide (PbO2), lead (Pb), and lead sulfate (PbSO4). During discharge, PbSO4 is formed, and during charging, PbSO4 is converted back to PbO2 and Pb, illustrating the principles of redox reactions and energy storage in electrochemical systems.
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Redox Reactions
Redox reactions involve the transfer of electrons between two species, resulting in oxidation (loss of electrons) and reduction (gain of electrons). In the context of the lead storage battery, lead sulfate is reduced to lead and oxidized to lead dioxide, highlighting the importance of electron flow in energy conversion processes.
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Related Practice
Textbook Question
In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO4(s) must be converted into PbO2(s) and Pb(s). (c) If a current of 500 A is used, how long will it take?
Textbook Question
Electrolysis of a metal nitrate solution M(NO3)2(aq) for 325 min with a constant current of 20.0 A gives 111 g of the metal. Identify the metal ion M2+.
Textbook Question
In order to charge a lead storage battery (Section 19.10) 500.0 g of PbSO4(s) must be converted into PbO2(s) and Pb(s). (b) How many coulombs of electrical charge are needed?
Textbook Question
What constant current (in amperes) is required to produce aluminum by the Hall–Héroult process at a rate of 40.0 kg/h?
Textbook Question
Aluminum, titanium, and several other metals can be col-ored by an electrochemical process called anodizing. Anodizing oxidizes a metal anode to yield a porous metal oxide coating that can incorporate dye molecules to give brilliant colors. In the oxidation of aluminum, for instance, the electrode reactions are The thickness of the aluminum oxide coating that forms on the anode can be controlled by varying the current flow during the electrolysis. How many minutes are required to produce a 0.0100-mm thick coating of Al2O3 (density 3.97 g/cm^3) on a square piece of aluminum metal 10.0 cm on an edge if the current passed through the piece is 0.600 A?
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