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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.20 - ElectrochemistryProblem 47a
Chapter 20, Problem 47a

(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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1
Identify the standard reduction potentials for each species under acidic conditions from a standard reduction potential table.
Recall that a higher (more positive) standard reduction potential indicates a stronger oxidizing agent.
List the standard reduction potentials for each species: \( \text{Cr}_2\text{O}_7^{2-} \), \( \text{H}_2\text{O}_2 \), \( \text{Cu}^{2+} \), \( \text{Cl}_2 \), and \( \text{O}_2 \).
Arrange the species in order of increasing standard reduction potential based on the values obtained.
The species with the lowest standard reduction potential is the weakest oxidizing agent, and the one with the highest is the strongest.

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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 can facilitate the oxidation of other substances more effectively. Understanding the relative strengths of different oxidizing agents is crucial for predicting the outcomes of redox reactions.
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Oxidizing and Reducing Agents

Standard Conditions

Standard conditions refer to a set of agreed-upon parameters for conducting experiments, typically defined as 1 atm pressure and a temperature of 25°C (298 K). These conditions provide a consistent basis for comparing the reactivity and properties of chemical species. When discussing oxidizing agents, standard conditions ensure that the comparisons made are relevant and applicable to real-world scenarios.
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Standard Reduction Potentials

Acidic Solution

An acidic solution is one where the concentration of hydrogen ions (H+) is higher than that of hydroxide ions (OH-), typically with a pH less than 7. The presence of H+ ions can influence the behavior of oxidizing agents, as some species may be more reactive or stable in acidic environments. Understanding how acidity affects redox reactions is essential for accurately determining the strength of oxidizing agents.
Related Practice
Textbook Question

By using the data in Appendix E, determine whether each of the following substances is likely to serve as an oxidant or a reductant: (a) Cl2(g), (b) MnO4- (aq, acidic solution), (c) Ba(s)

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Textbook Question

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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Textbook Question

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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Textbook Question

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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