Domanda del libro di testo
Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (c) Fe1s2 + 2 Fe3+1aq2 ¡ 3 Fe2+1aq2
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Ch.20 - Electrochemistry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 20, Problema 37a
Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (a) Cl21g2 + 2 I-1aq2 ¡ 2 Cl-1aq2 + I21s2
Guida verificata passo dopo passo1
Identify the half-reactions involved in the overall reaction. For the given reaction, the half-reactions are: \( \text{Cl}_2(g) + 2e^- \rightarrow 2\text{Cl}^-(aq) \) and \( 2\text{I}^-(aq) \rightarrow \text{I}_2(s) + 2e^- \).
Look up the standard reduction potentials for each half-reaction in Appendix E. The standard reduction potential for \( \text{Cl}_2(g) + 2e^- \rightarrow 2\text{Cl}^-(aq) \) is typically positive, while for \( \text{I}_2(s) + 2e^- \rightarrow 2\text{I}^-(aq) \) it is less positive.
Reverse the oxidation half-reaction to match the direction of the given reaction. This means reversing \( 2\text{I}^-(aq) \rightarrow \text{I}_2(s) + 2e^- \) to \( \text{I}_2(s) + 2e^- \rightarrow 2\text{I}^-(aq) \) and changing the sign of its standard reduction potential.
Calculate the standard electromotive force (emf) of the reaction by adding the standard reduction potential of the reduction half-reaction (\( \text{Cl}_2(g) + 2e^- \rightarrow 2\text{Cl}^-(aq) \)) to the reversed oxidation potential (\( \text{I}_2(s) + 2e^- \rightarrow 2\text{I}^-(aq) \)).
The standard emf of the reaction is the sum of the potentials from step 4. This value indicates the tendency of the reaction to occur spontaneously under standard conditions.
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Standard Reduction Potentials
Standard reduction potentials are measured voltages that indicate the tendency of a chemical species to gain electrons and be reduced. Each half-reaction has a specific potential, typically 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 overall cell potential.
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01:10
Standard Reduction Potentials
Electrochemical Cell and EMF
An electrochemical cell consists of two half-cells where oxidation and reduction reactions occur. The electromotive force (EMF) is the voltage generated by the cell when no current is flowing, representing the maximum potential difference between the two electrodes. The standard EMF can be calculated using the standard reduction potentials of the half-reactions involved.
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02:46Electrochemical Cells
Nernst Equation
The Nernst equation relates the cell potential to the concentrations of the reactants and products in a redox reaction. It allows for the calculation of the EMF under non-standard conditions, taking into account temperature and concentration changes. Understanding this equation is essential for accurately determining the cell potential in various scenarios.
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01:17The Nernst Equation
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Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (d) 2 NO3-1aq2 + 8 H+1aq2 + 3 Cu1s2 ¡ 2 NO1g2 + 4 H2O1l2 + 3 Cu2+1aq2
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Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (b) Ni1s2 + 2 Ce4+1aq2 ¡ Ni2+1aq2 + 2 Ce3+1aq2
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