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Chapter 22: Problem 45

Give a specific example of a chemical equation that illustrates the (a) reaction of a metal sulfide with \(\mathrm{HCl}(\mathrm{aq})\) (b) action of a nonoxidizing acid on a metal sulfite; (c) oxidation of \(\mathrm{SO}_{2}(\mathrm{aq})\) to \(\mathrm{SO}_{4}^{2-}(\mathrm{aq})\) by \(\mathrm{MnO}_{2}(\mathrm{s})\) in acidic solution; (d) disproportionation of \(S_{2} \mathrm{O}_{3}^{2-}\) in acidic solution.

Short Answer

Expert verified
The given reactions are: \n(a) \(FeS(s) + 2HCl(aq) \rightarrow FeCl_{2}(aq) + H_{2}S(g)\) \n(b) \(Na_{2}SO_{3}(s) + 2HCl(aq) \rightarrow 2NaCl(aq) + H_{2}O(l) + SO_{2}(g)\) \n(c) \(5SO_{2}(aq) + 2MnO_{2}(s) + 2H_{2}O(l) \rightarrow 2Mn^{2+}(aq) + 5SO_{4}^{2-}(aq) + 4H^{+}(aq)\) \n(d) \(S_{2}O_{3}^{2-}(aq) + 2H^{+}(aq) \rightarrow SO_{2}(aq) + H_{2}O(l) + S(s)\)

Step by step solution

01

Reaction of metal sulfide with HCl

We can use iron sulfide as an example here. When iron sulfide reacts with hydrochloric acid, it produces iron chloride and hydrogen sulfide as a gas. This can be represented as follows: \n\(FeS(s) + 2HCl(aq) \rightarrow FeCl_{2}(aq) + H_{2}S(g)\)
02

Action of nonoxidizing acid on metal sulfite

In this case, let's consider a nonoxidizing acid like hydrochloric acid coming into action with a metal sulfite - for example, sodium sulfite. Sodium sulfite reacts with hydrochloric acid to form sodium chloride, water, and release sulfur dioxide gas as follows: \n\(Na_{2}SO_{3}(s) + 2HCl(aq) \rightarrow 2NaCl(aq) + H_{2}O(l) + SO_{2}(g)\)
03

Oxidation of SO_{2} to SO_{4}^{2-} by MnO_{2} in acidic solution

The reaction can be shown as follows: \n\(5SO_{2}(aq) + 2MnO_{2}(s) + 2H_{2}O(l) \rightarrow 2Mn^{2+}(aq) + 5SO_{4}^{2-}(aq) + 4H^{+}(aq)\)
04

Disproportionation of S_{2}O_{3}^{2-} in acidic solution

Disproportionation is a reaction during which a higher and a lower oxidation state are formed. This can be shown as follows: \n\(S_{2}O_{3}^{2-}(aq) + 2H^{+}(aq) \rightarrow SO_{2}(aq) + H_{2}O(l) + S(s)\)

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Metal Sulfide Reaction with HCl
When a metal sulfide reacts with hydrochloric acid (HCl), a fascinating transformation takes place. For instance, consider the reaction with iron sulfide (FeS). When FeS is added to HCl, iron chloride (FeCl鈧�) and hydrogen sulfide (H鈧係) gas are produced:
\[ FeS(s) + 2HCl(aq) \rightarrow FeCl_{2}(aq) + H_{2}S(g) \]
This reaction illustrates typical characteristics found when metal sulfides meet HCl. The release of H鈧係 gas is notable for its unpleasant smell, akin to rotten eggs. Such reactions are prevalent in many chemical processes and are essential for understanding basic reaction mechanics.
Nonoxidizing Acid and Metal Sulfite
A nonoxidizing acid like hydrochloric acid can react uniquely with metal sulfites. Take sodium sulfite (Na鈧係O鈧�) as an example. When it reacts with HCl, we get sodium chloride (NaCl), water (H鈧侽), and sulfur dioxide (SO鈧�) gas:
\[ Na_{2}SO_{3}(s) + 2HCl(aq) \rightarrow 2NaCl(aq) + H_{2}O(l) + SO_{2}(g) \]
This reaction is a straightforward way to produce SO鈧�, a gas often used in industries such as paper manufacturing. This type of reaction emphasizes the versatility and utility of nonoxidizing acids in producing secondary products efficiently.
Oxidation of SO2
The oxidation of sulfur dioxide (SO鈧�) to sulfate ions (SO鈧劼测伝) involves an intriguing interaction. When SO鈧� meets manganese dioxide (MnO鈧�) in an acidic environment, it transforms as follows:
\[ 5SO_{2}(aq) + 2MnO_{2}(s) + 2H_{2}O(l) \rightarrow 2Mn^{2+}(aq) + 5SO_{4}^{2-}(aq) + 4H^{+}(aq) \]
This process is vital in understanding how sulfur transformations occur in nature and technology. The role of MnO鈧� as an oxidizing agent showcases how different substances can facilitate complex chemical conversions, such as turning a harmful gas into a useful ion.
Disproportionation Reaction
Disproportionation is a unique type of reaction where a single substance undergoes both oxidation and reduction. Consider thiosulfate ions (S鈧侽鈧兟测伝) in an acidic solution. They transform in the following way:
\[ S_{2}O_{3}^{2-}(aq) + 2H^{+}(aq) \rightarrow SO_{2}(aq) + H_{2}O(l) + S(s) \]
This reaction demonstrates how a compound can split into multiple oxidation states, producing sulfur dioxide, water, and elemental sulfur. Disproportionation reactions are essential in many natural and industrial chemical processes, highlighting the diverse behavior of chemical species.

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Most popular questions from this chapter

The oxides of the selenium(IV) and tellurium(IV) are \(\mathrm{SeO}_{2}\) and \(\mathrm{TeO}_{2} .\) One of these oxides is amphoteric and one is acidic. Which is which?

Each of the following compounds decomposes to produce \(\mathrm{O}_{2}(\mathrm{g})\) when heated: \((\mathrm{a}) \mathrm{HgO}(\mathrm{s}) ;\) (b) \(\mathrm{KClO}_{4}(\mathrm{s})\) Write plausible equations for these reactions.

Write a plausible chemical equation to represent the reaction of \((\mathrm{a}) \mathrm{Cl}_{2}(\mathrm{g}) \quad\) with cold \(\quad \mathrm{NaOH}(\mathrm{aq})\) (b) \(\mathrm{NaI}(\mathrm{s})\) with hot \(\mathrm{H}_{2} \mathrm{SO}_{4}(\text { concd aq }) ;\) (c) \(\mathrm{Cl}_{2}(\mathrm{g})\) with \(\mathrm{KI}_{3}(\mathrm{aq}) ; \quad\) (d) \(\quad \mathrm{NaBr}(\mathrm{s}) \quad\) with hot \(\mathrm{H}_{3} \mathrm{PO}_{4}\) \((\text { concd aq })\) (e) \(\mathrm{NaHSO}_{3}(\mathrm{aq})\) with \(\mathrm{MnO}_{4}^{-1}(\mathrm{aq})\) in dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\).

Show by calculation whether the reaction \(2 \mathrm{HOCl}(\mathrm{aq}) \longrightarrow \mathrm{HClO}_{2}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})\) will go essentially to completion as written for standardstate conditions.

One reaction for the production of adipic acid, \(\mathrm{HOOC}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{COOH},\) used in the manufacture of nylon, involves the oxidation of cyclohexanone, \(\mathrm{C}_{6} \mathrm{H}_{10} \mathrm{O},\) in a nitric acid solution. Assume that dinitrogen monoxide is also formed, and write a balanced equation for this reaction.
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