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Chapter 22: Problem 123

The best reducing agent of the following substances is (a) \(\mathrm{H}_{2} \mathrm{S} ;\) (b) \(\mathrm{O}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4} ;\) (d) \(\mathrm{NaF}\); (e) \(\mathrm{H}_{2} \mathrm{O}\).

Short Answer

Expert verified
The best reducing agent among the given substances is \(\mathrm{H}_{2}\mathrm{S}\).

Step by step solution

01

Identify the oxidations states of the substances

The substances given are \(\mathrm{H}_{2}\mathrm{S}\), \(\mathrm{O}_{3}\), \(\mathrm{H}_{2} \mathrm{SO}_{4}\), \(\mathrm{NaF}\) and \(\mathrm{H}_{2} \mathrm{O}\). Their oxidation states are -2, 0, +6, -1, and -2 respectively. Remember that the oxidation state indicates the degree of oxidation of an atom in a chemical compound. The most electronegative element in a compound is assigned the negative oxidation number.
02

Analyze the standard reduction potentials of the substances

Knowing the oxidation states, the standard reduction potentials of the substances can be checked from a standard reduction potentials table. The substance with the most positive standard reduction potential is the strongest oxidizing agent, while the one with the most negative standard reduction potential is the strongest reducing agent.
03

Identify the strongest reducing agent

By comparing the standard reduction potentials, the substance with the highest ability to lose electrons (i.e., the one with the most negative or least positive standard reduction potential) will be the best reducing agent. Among the given substances, \( \mathrm{H}_{2}\mathrm{S} \) is the best reducing agent as it has the most negative standard reduction potential compared to the others.

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Most popular questions from this chapter

Write a chemical equation for the hydrolysis in alkaline solution of \(\mathrm{XeF}_{6}\) that yields \(\mathrm{XeO}_{6}^{4-}, \mathrm{Xe}, \mathrm{O}_{2}, \mathrm{F}^{-}\) and \(\mathrm{H}_{2} \mathrm{O}\) as products.

Show by calculation whether the disproportionation of chlorine gas to chlorate and chloride ions will occur under standard-state conditions in an acidic solution.

Supply an appropriate name for each of the following: (a) \(\mathrm{HPO}_{4}^{2-} ;\) (b) \(\mathrm{Ca}_{2} \mathrm{P}_{2} \mathrm{O}_{7} ;\) (c) \(\mathrm{H}_{6} \mathrm{P}_{4} \mathrm{O}_{13}\).

What is the oxidation state of sulfur in the following compounds? (a) \(\mathrm{SF}_{4} ;\) (b) \(\mathrm{S}_{2} \mathrm{F}_{10} ;\) (c) \(\mathrm{H}_{2} \mathrm{S} ;\) (d) \(\mathrm{CaSO}_{3}\).

The abundance of \(\mathrm{F}^{-}\) in seawater is \(1 \mathrm{g} \mathrm{F}^{-}\) per ton of seawater. Suppose that a commercially feasible method could be found to extract fluorine from seawater. (a) What mass of \(\mathrm{F}_{2}\) could be obtained from \(1 \mathrm{km}^{3}\) of seawater \(\left(d=1.03 \mathrm{g} \mathrm{cm}^{-3}\right) ?\) (b) Would the process resemble that for extracting bromine from seawater? Explain.
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