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
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 20, Problema 41b
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
Guida verificata passo dopo passo1
Identify the half-reactions involved in the overall redox reaction. For the given reaction, the half-reactions are: \( \text{Ni} \rightarrow \text{Ni}^{2+} + 2e^- \) and \( \text{Ce}^{4+} + e^- \rightarrow \text{Ce}^{3+} \).
Look up the standard reduction potentials for each half-reaction in Appendix E. The standard reduction potential for \( \text{Ni}^{2+} + 2e^- \rightarrow \text{Ni} \) is \( E^\circ = -0.25 \text{ V} \), and for \( \text{Ce}^{4+} + e^- \rightarrow \text{Ce}^{3+} \) is \( E^\circ = +1.61 \text{ V} \).
Reverse the reduction potential for the oxidation half-reaction. Since \( \text{Ni} \rightarrow \text{Ni}^{2+} + 2e^- \) is the oxidation half-reaction, its potential becomes \( E^\circ = +0.25 \text{ V} \).
Calculate the standard emf (electromotive force) of the cell by adding the standard potentials of the oxidation and reduction half-reactions: \( E^\circ_{\text{cell}} = E^\circ_{\text{reduction}} + E^\circ_{\text{oxidation}} \).
Substitute the values into the equation: \( E^\circ_{\text{cell}} = 1.61 \text{ V} + 0.25 \text{ V} \).
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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) of the cell is the voltage generated by the spontaneous redox reaction, calculated as the difference between the reduction potentials of the cathode and anode. A positive EMF indicates a spontaneous reaction, while a negative EMF suggests non-spontaneity.
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02:46Electrochemical Cells
Balancing Redox Reactions
Balancing redox reactions involves ensuring that both mass and charge are conserved in the reaction. This is done by identifying oxidation and reduction half-reactions, balancing the number of electrons transferred, and adjusting coefficients accordingly. Properly balanced reactions are essential for accurate calculations of standard EMF and understanding the stoichiometry of the reaction.
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01:04Balancing Basic Redox Reactions
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