Domanda del libro di testo
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?
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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 148
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
Guida verificata passo dopo passo1
Identify the two half-reactions involved in the electrochemical cell and their respective standard reduction potentials (E°).
Write the balanced overall cell reaction by combining the two half-reactions, ensuring that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction.
Calculate the standard cell potential (E°_cell) by subtracting the standard reduction potential of the anode (oxidation) from the standard reduction potential of the cathode (reduction): E°_cell = E°_cathode - E°_anode.
Use the Nernst equation to calculate the standard Gibbs free energy change (∆G°) for the reaction: ∆G° = -nFE°_cell, where n is the number of moles of electrons transferred and F is the Faraday constant (approximately 96485 C/mol).
Calculate the equilibrium constant (K) for the reaction at 25 °C using the relationship between ∆G° and K: ∆G° = -RTlnK, where R is the universal gas constant (8.314 J/mol·K) and T is the temperature in Kelvin (298 K).
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Electrode Potential (E°)
Electrode potential, denoted as E°, is a measure of the tendency of a chemical species to be reduced, expressed in volts. It is determined under standard conditions (1 M concentration, 1 atm pressure, and 25 °C). The more positive the E° value, the greater the species' ability to gain electrons and undergo reduction, which is crucial for predicting the direction of electron flow in electrochemical cells.
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Percorso guidato
02:43
Relationship between ∆E°, ∆G°, and K
Gibbs Free Energy (∆G°)
Gibbs free energy change (∆G°) is a thermodynamic quantity that indicates the spontaneity of a reaction at standard conditions. It is calculated using the equation ∆G° = -nFE°, where n is the number of moles of electrons transferred, F is Faraday's constant, and E° is the cell potential. A negative ∆G° indicates a spontaneous reaction, while a positive value suggests non-spontaneity.
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01:51Gibbs Free Energy of Reactions
Equilibrium Constant (K)
The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is related to the Gibbs free energy change by the equation ∆G° = -RT ln(K), where R is the universal gas constant and T is the temperature in Kelvin. A larger K value indicates a reaction that favors product formation, while a smaller K suggests reactants are favored.
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01:14Equilibrium Constant K
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Chlorine can be prepared in the laboratory by the reaction of hydrochloric acid and potassium permanganate. (a) Use data in Appendix D to write a balanced equation for the reaction. The reduction product is Mn2+.
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Domanda del libro di testo
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?
Domanda del libro di testo
Chlorine can be prepared in the laboratory by the reaction of hydrochloric acid and potassium permanganate.
(b) Calculate E° and ∆G° for the reaction
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Domanda del libro di testo
The sodium–sulfur battery has molybdenum electrodes with anode and cathode compartments separated by b-alumina, a ceramic through which sodium ions can pass. Because the battery operates at temperatures above 300 °C, all the reactants and products are present in a molten solution. The cell voltage is about 2.0 V.
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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). (b) How many coulombs of electrical charge are needed?
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