Domanda del libro di testo
Consider the following half-reactions and E° values:
(c) Write the cell reaction for part (b), and calculate the values of E°, ∆G° (in kilojoules), and K for this reaction at 25 °C
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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 146b
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?
Guida verificata passo dopo passo1
Identify the balanced chemical reaction for the conversion of PbSO_4(s) to PbO_2(s) and Pb(s).
Determine the molar mass of PbSO_4 to convert the given mass (500.0 g) into moles.
Use stoichiometry to find the moles of electrons required for the conversion based on the balanced equation.
Calculate the total charge in coulombs using the relationship between moles of electrons and charge (1 mole of electrons = 96485 C).
Summarize the steps to ensure all conversions and calculations align with the stoichiometry of the reaction.
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Electrochemical Reactions
Electrochemical reactions involve the transfer of electrons between chemical species, which is fundamental in processes like charging a battery. In a lead storage battery, lead sulfate (PbSO4) is converted into lead dioxide (PbO2) and lead (Pb) through oxidation and reduction reactions, releasing or consuming electrons in the process.
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Percorso guidato
02:46
Electrochemical Cells
Faraday's Laws of Electrolysis
Faraday's Laws of Electrolysis quantify the relationship between the amount of substance transformed at an electrode and the quantity of electric charge passed through the electrolyte. The first law states that the mass of a substance altered at an electrode is directly proportional to the total electric charge passed, which is crucial for calculating the charge needed to convert PbSO4 to PbO2 and Pb.
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Percorso guidato
01:40Faraday's Constant in Electrochemistry
Coulombs and Charge Calculation
Coulombs (C) are the standard unit of electric charge in the International System of Units (SI). To determine the total charge required for the conversion of PbSO4 to PbO2 and Pb, one must calculate the moles of electrons involved in the reaction and then use Faraday's constant (approximately 96485 C/mol) to convert moles of electrons to coulombs.
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Percorso guidato
01:15Coulomb's Law Concept 2
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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?
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