Domanda del libro di testo
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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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 37c
Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (c) Fe1s2 + 2 Fe3+1aq2 ¡ 3 Fe2+1aq2
Guida verificata passo dopo passo1
Identify the half-reactions involved in the overall reaction. For the given reaction, the half-reactions are: \( \text{Fe} \rightarrow \text{Fe}^{2+} + 2e^- \) and \( \text{Fe}^{3+} + e^- \rightarrow \text{Fe}^{2+} \).
Look up the standard reduction potentials for each half-reaction from Appendix E. The standard reduction potential for \( \text{Fe}^{3+} + e^- \rightarrow \text{Fe}^{2+} \) is typically given, and you will need to reverse the sign for the oxidation half-reaction \( \text{Fe} \rightarrow \text{Fe}^{2+} + 2e^- \).
Calculate the standard emf (electromotive force) for the overall reaction by using the formula: \( E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \).
Substitute the values of the standard reduction potentials into the formula. Remember that the cathode is where reduction occurs and the anode is where oxidation occurs.
Sum the potentials to find the standard emf for the overall reaction. Ensure that the stoichiometry of the electrons is balanced in the half-reactions before calculating the emf.
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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, which can be calculated using the standard reduction potentials of the half-reactions involved. The overall EMF can be determined by subtracting the reduction potential of the anode from that of the cathode.
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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 the oxidation and reduction half-reactions, balancing the number of electrons transferred, and adjusting the coefficients of the reactants and products accordingly. Properly balanced reactions are essential for accurate calculations of standard EMF.
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01:04Balancing Basic Redox Reactions
Pratica correlata
Domanda del libro di testo
The standard reduction potentials of the following halfreactions are given in Appendix E:
Ag+(aq) + e- → Ag(s)
Cu2+(aq) + 2 e- → Cu(s)
Ni2+(aq) + 2 e- → Ni(s)
Cr3+(aq) + 3 e- → Cr(s)
(a) Determine which combination of these half-cell reactions leads to the cell reaction with the largest positive cell potential and calculate the value.
(b) Determine which combination of these half-cell reactions leads to the cell reaction with the smallest positive cell potential and calculate the value.
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Domanda del libro di testo
A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow
Domanda del libro di testo
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
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Domanda del libro di testo
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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