Domanda del libro di testo
By using the data in Appendix E, determine whether each of the following substances is likely to serve as an oxidant or a reductant: (d) Zn(s)
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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 47b
(b) Arrange the following in order of increasing strength as reducing agents in acidic solution: Zn, I-, Sn2+, H2O2, Al.
Guida verificata passo dopo passo1
Understand the concept of reducing agents: A reducing agent is a substance that donates electrons to another substance, reducing it. The strength of a reducing agent is determined by its ability to lose electrons easily.
Consider the standard reduction potentials: In acidic solutions, the standard reduction potential (E°) values can help determine the strength of reducing agents. A more negative E° value indicates a stronger reducing agent.
List the standard reduction potentials for each species: Look up the standard reduction potentials for Zn, I-, Sn2+, H2O2, and Al in a table of standard reduction potentials.
Compare the E° values: Arrange the species in order of increasing reduction potential. The species with the most negative E° value is the strongest reducing agent, and the one with the least negative (or most positive) E° value is the weakest.
Arrange the species: Based on the comparison of their standard reduction potentials, list the species in order of increasing strength as reducing agents.
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Reducing Agents
Reducing agents are substances that donate electrons in a chemical reaction, thereby reducing another species. Their strength as reducing agents is determined by their ability to lose electrons easily. In acidic solutions, the relative strength of reducing agents can vary based on their standard reduction potentials, which indicate how readily they can be oxidized.
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01:01
Oxidizing and Reducing Agents
Standard Reduction Potential
Standard reduction potential (E°) is a measure of the tendency of a chemical species to be reduced, expressed in volts. A higher E° value indicates a stronger oxidizing agent and a weaker reducing agent. Conversely, a lower E° value suggests a stronger reducing agent. This concept is crucial for comparing the reducing strengths of different substances in a given reaction environment.
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01:10Standard Reduction Potentials
Acidic Solution
An acidic solution is characterized by a higher concentration of hydrogen ions (H⁺) than hydroxide ions (OH⁻). In such environments, certain reactions may be favored, and the behavior of reducing agents can change. For example, some metals may react differently in acidic conditions compared to neutral or basic conditions, affecting their reducing power.
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01:39Solution Components
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(a) Assuming standard conditions, arrange the following in order of increasing strength as oxidizing agents in acidic solution: Cr2O72-, H2O2, Cu2+, Cl2, O2.
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Domanda del libro di testo
Given the following reduction half-reactions:
Fe3+(aq) + e- → Fe2+(aq) E°red = +0.77 V
S2O62-(aq) + 4 H+(aq) + 2 e- → 2 H2SO3(aq) E°red = +0.60 V
N2O(g) + 2 H+(aq) + 2 e- → N2(g) + H2O(l) E°red = -1.77 V
VO2+(aq) + 2 H+(aq) + e- → VO2+ + H2O(l) E°red = +1.00 V
(a) Write balanced chemical equations for the oxidation of Fe2+(aq) by S2O62-(aq), by N2O(aq), and by VO2+(aq).
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Domanda del libro di testo
Is each of the following substances likely to serve as an oxidant or a reductant: (a) Ce3+(aq) (b) Ca(s) (c) ClO3-(aq) (d) N2O5(g)?
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