교과서 질문
Which metal cation is the best oxidizing agent? a. Pb2+ b. Cr3+ c. Fe2+ d. Sn2+
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Ch.19 - Electrochemistry
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
19장, 문제 66
Use tabulated electrode potentials to calculate ∆G°rxn for each reaction at 25 °C. a. 2 Fe3+(aq) + 3 Sn(s) → 2 Fe(s) + 3 Sn2+(aq) b. O2(g) + 2 H2O(l) + 2 Cu(s) → 4 OH–(aq) + 2 Cu2+(aq) c. Br2(l) + 2 I–(aq) → 2 Br–(aq) + I2(s)
검증된 단계별 안내1
Identify the half-reactions involved in the redox process. For the given reaction, the half-reactions are: \( \text{Br}_2(l) + 2e^- \rightarrow 2\text{Br}^-(aq) \) and \( 2\text{I}^-(aq) \rightarrow \text{I}_2(s) + 2e^- \).
Look up the standard electrode potentials (E°) for each half-reaction from a table of standard reduction potentials. Note that the potential for the oxidation half-reaction (\( 2\text{I}^-(aq) \rightarrow \text{I}_2(s) + 2e^- \)) will be the negative of the reduction potential.
Calculate the standard cell potential (E°cell) for the reaction by subtracting the anode potential (oxidation) from the cathode potential (reduction): \( E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \).
Use the Nernst equation to relate the standard cell potential to the standard Gibbs free energy change: \( \Delta G^\circ_{\text{rxn}} = -nFE^\circ_{\text{cell}} \), where \( n \) is the number of moles of electrons transferred (2 in this case) and \( F \) is the Faraday constant (approximately 96485 C/mol).
Substitute the values for \( n \), \( F \), and \( E^\circ_{\text{cell}} \) into the equation to calculate \( \Delta G^\circ_{\text{rxn}} \).
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주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
Electrode Potentials
Electrode potentials, measured in volts, indicate the tendency of a chemical species to be reduced. Standard electrode potentials (E°) are measured under standard conditions (1 M concentration, 1 atm pressure, and 25 °C). These values are crucial for predicting the direction of redox reactions and calculating the Gibbs free energy change (∆G°rxn) for reactions.
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가이드 코스
01:27
Standard Cell Potential
Gibbs Free Energy (∆G°rxn)
Gibbs free energy change (∆G°rxn) is a thermodynamic quantity that indicates the spontaneity of a reaction at standard conditions. It can be calculated using the equation ∆G°rxn = -nFE°cell, where n is the number of moles of electrons transferred, F is Faraday's constant, and E°cell is the cell potential derived from the electrode potentials of the half-reactions.
추천 영상:
가이드 코스
01:51Gibbs Free Energy of Reactions
Half-Reaction Method
The half-reaction method involves breaking down a redox reaction into its oxidation and reduction half-reactions. Each half-reaction can be assigned a standard electrode potential, which allows for the calculation of the overall cell potential (E°cell). This method is essential for determining the Gibbs free energy change and understanding the electron transfer processes in the reaction.
추천 영상:
가이드 코스
01:49Method 1 of Radioactive Half-Life