From each of the following pairs of substances, use data in Appendix E to choose the one that is the stronger reducing agent: (d) BrO3-1aq2 or IO3-1aq2

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Identify the half-reactions for both BrO3- (bromate ion) and IO3- (iodate ion) in their reduction forms. This involves finding the reactions where these ions gain electrons to form their respective reduced states.

Consult Appendix E or a standard reduction potential table to find the standard reduction potentials (E°) for both BrO3- and IO3-. These values indicate the tendency of each ion to gain electrons.

Compare the standard reduction potentials of the two half-reactions. The substance with the more negative E° value is the stronger reducing agent, as it indicates a greater tendency to donate electrons.

Remember that a stronger reducing agent has a greater ability to reduce other substances, meaning it is more easily oxidized itself.

Conclude which ion, BrO3- or IO3-, is the stronger reducing agent based on the comparison of their standard reduction potentials.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Reducing Agents

A reducing agent is a substance that donates electrons in a chemical reaction, thereby reducing another substance. The strength of a reducing agent is determined by its ability to lose electrons easily. Stronger reducing agents have a greater tendency to undergo oxidation, which is the loss of electrons.

Standard Reduction Potentials

Standard reduction potentials (E°) are measured values that indicate the tendency of a species to gain electrons and be reduced. These values are typically found in tables and are used to compare the strength of different oxidizing and reducing agents. A more negative E° value indicates a stronger reducing agent, as it is more likely to lose electrons.

Oxidation States

Oxidation states (or numbers) represent the degree of oxidation of an atom in a compound. They help in determining how many electrons are gained or lost during a reaction. Understanding the oxidation states of the elements in the substances being compared is crucial for identifying which one acts as the stronger reducing agent.

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Textbook Question

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate ∆G° at 298 K, and calculate the equilibrium constant K at 298 K. (c) In basic solution, Cr1OH231s2 is oxidized to CrO42-1aq2 by ClO-1aq2.

Textbook Question

Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for each of the following reactions at 298 K:

(a) Fe(s) + Ni²⁺(aq) → Fe²⁺(aq) + Ni(s)

(b) Co(s) + 2 H⁺(aq) → Co²⁺(aq) + H₂(g)