Textbook Question
What conditions must be met for a cell potential E to qualify as a standard cell potential E°?
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Ch.19 - Electrochemistry
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 19, Problem 76
Consider the following substances: I2(s), Fe2+(aq), Cr2O72-(aq). Which is the strongest oxidizing agent? Which is the weakest oxidizing agent?
Verified step by step guidance1
insert step 1> Identify the oxidation states of the elements in each substance: I2(s), Fe2+(aq), and Cr2O72-(aq).
insert step 2> Recall that an oxidizing agent is a substance that gains electrons and is reduced in a chemical reaction.
insert step 3> Compare the standard reduction potentials (E°) for each substance to determine their ability to act as oxidizing agents.
insert step 4> The substance with the highest standard reduction potential is the strongest oxidizing agent, while the one with the lowest is the weakest.
insert step 5> Rank the substances based on their standard reduction potentials to identify the strongest and weakest oxidizing agents.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Oxidizing Agents
An oxidizing agent is a substance that gains electrons in a chemical reaction, causing another substance to be oxidized. The strength of an oxidizing agent is determined by its ability to accept electrons; stronger oxidizers have a higher reduction potential. Understanding the relative strengths of different oxidizing agents is crucial for predicting the outcomes of redox reactions.
Recommended video:
Guided course
01:01
Oxidizing and Reducing Agents
Standard Reduction Potentials
Standard reduction potentials (E°) are measured values that indicate the tendency of a species to be reduced. These values are typically listed in tables, allowing for easy comparison between different oxidizing agents. A higher E° value corresponds to a stronger oxidizing agent, as it indicates a greater likelihood of gaining electrons.
Recommended video:
Guided course
01:10Standard Reduction Potentials
Half-Reaction Method
The half-reaction method involves separating oxidation and reduction processes to analyze redox reactions. By writing the half-reactions for each species involved, one can determine which species is oxidized and which is reduced. This method is essential for identifying the strongest and weakest oxidizing agents among the given substances.
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01:49Method 1 of Radioactive Half-Life
Related Practice
Textbook Question
Consider the following substances: Fe2+(aq), Sn2+(aq), I-(aq). Identify the strongest reducing agent and the weakest reducing agent.
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Textbook Question
Arrange the following oxidizing agents in order of increasing strength under standard-state conditions: Br2(aq), MnO4+(aq), Sn4+(aq).
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Textbook Question
The following cell reactions occur spontaneously: (c) Which of the three cell reactions delivers the highest voltage?
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Textbook Question
Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq).(d) Which substances can be oxidized by Cu2+(aq)? Which can be reduced by H2O2(aq)?
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