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Chapter 5: Problem 44

Write a balanced equation for the redox reactions. (a) The reaction of aluminum metal with hydroiodic acid. (b) The reduction of vanadyl ion ( \(\mathrm{VO}^{2+}\) ) to vanadic ion \(\left(\mathrm{V}^{3+}\right)\) in acidic solution with zinc metal as the reducing agent. (c) The oxidation of methanol by chlorate ion in acidic solution, producing carbon dioxide gas, water, and chlorine dioxide gas as products.

Short Answer

Expert verified
(a) Balanced equation: 2Al + 6HI = 2AlI3 + 3H2. (b) Balanced equation: VO2+ + Zn + 2H+ = V3+ + Zn2+ + H2O. (c) Balanced equation: 3CH3OH + 5ClO3- + 12H+ = 3CO2 + 14H2O + 5ClO2.

Step by step solution

01

Part (a) Reaction of Aluminum Metal with Hydroiodic Acid

The unbalanced chemical reaction can be written as follows: \[Al + HI \rightarrow AlI_3 +H_2.\] Now, balance the equation: \[2Al + 6HI \rightarrow 2AlI_3 + 3H_2.\]
02

Part (b) Reduction of Vanadyl Ion to Vanadic Ion

The unbalanced half-reactions are: \[VO^{2+} \rightarrow V^{3+}\] and \[Zn \rightarrow Zn^{2+}.\] After balancing, we find: \[VO^{2+} + Zn + 2H^{+} \rightarrow V^{3+} + Zn^{2+} + H_2O.\]
03

Part (c) The Oxidation of Methanol by Chlorate Ion

Unbalanced reactions are: \[ CH_3OH \rightarrow CO_2 + H_2O\], and \[ClO_3^- \rightarrow ClO_2 + O_2.\] After balancing we have: \[ 3CH_3OH + 5ClO_3^- + 12H^{+} \rightarrow 3CO_2 + 14H_2O + 5ClO_2.\]

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Most popular questions from this chapter

What are the oxidizing and reducing agents in the following redox reactions? (a) \(5 \mathrm{SO}_{3}^{2-}+2 \mathrm{MnO}_{4}^{-}+6 \mathrm{H}^{+} \longrightarrow\) \(5 \mathrm{SO}_{4}^{2-}+2 \mathrm{Mn}^{2+}+3 \mathrm{H}_{2} \mathrm{O}\) (b) \(2 \mathrm{NO}_{2}(\mathrm{g})+7 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) (c) \(2\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}+\mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{H}^{+} \longrightarrow\) \(2\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}+2 \mathrm{H}_{2} \mathrm{O}\)

Following are some laboratory methods occasionally used for the preparation of small quantities of chemicals. Write a balanced equation for each. (a) preparation of \(\mathrm{H}_{2} \mathrm{S}(\mathrm{g}): \mathrm{HCl}(\mathrm{aq})\) is heated with \(\mathrm{FeS}(\mathrm{s})\) (b) preparation of \(\mathrm{Cl}_{2}(\mathrm{g}): \mathrm{HCl}(\mathrm{aq})\) is heated with \(\mathrm{MnO}_{2}(\mathrm{s}) ; \mathrm{MnCl}_{2}(\mathrm{aq})\) and \(\mathrm{H}_{2} \mathrm{O}(1)\) are other products (c) preparation of \(\mathrm{N}_{2}: \mathrm{Br}_{2}\) and \(\mathrm{NH}_{3}\) react in aqueous solution; \(\mathrm{NH}_{4} \mathrm{Br}\) is another product (d) preparation of chlorous acid: an aqueous suspension of solid barium chlorite is treated with dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\)

Iron (Fe) is obtained from rock that is extracted from open pit mines and then crushed. The process used to obtain the pure metal from the crushed rock produces solid waste, called tailings, which are stored in disposal areas near the mines. The tailings pose a serious environmental risk because they contain sulfides, such as pyrite ( \(\mathrm{FeS}_{2}\) ), which oxidize in air to produce metal ions and \(\mathrm{H}^{+}\) ions that can enter into surface water or ground water. The oxidation of \(\mathrm{FeS}_{2}\) to \(\mathrm{Fe}^{3+}\) is described by the unbalanced chemical equation below. \(\mathrm{FeS}_{2}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \longrightarrow\) \(\quad \mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \quad(\text { not balanced })\) Thus, the oxidation of pyrite produces \(\mathrm{Fe}^{3+}\) and \(\mathrm{H}^{+}\) ions that can leach into surface or ground water. The leaching of \(\mathrm{H}^{+}\) ions causes the water to become very acidic. To prevent acidification of nearby ground or surface water, limestone \(\left(\mathrm{CaCO}_{3}\right)\) is added to the tailings to neutralize the \(\mathrm{H}^{+}\) ions: \(\mathrm{CaCO}_{3}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \underset{\mathrm{Ca}^{2+}}{\longrightarrow}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{CO}_{2}(\mathrm{g})\) (a) Balance the equation above for the reaction of \(\mathrm{FeS}_{2}\) and \(\mathrm{O}_{2}\). [ Hint: Start with the half-equations \(\mathrm{FeS}_{2}(\mathrm{s}) \rightarrow\) \(\left.\mathrm{Fe}^{3+}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq}) \text { and } \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(1) .\right]\) (b) What is the minimum amount of \(\mathrm{CaCO}_{3}(\mathrm{s})\) required, per kilogram of tailings, to prevent contamination if the tailings contain \(3 \%\) S by mass? Assume that all the sulfur in the tailings is in the form \(\mathrm{FeS}_{2}\).

Classify each of the following statements as true or false. (a) Barium chloride, \(\mathrm{BaCl}_{2^{\prime}}\) is a weak electrolyte in aqueous solution. (b) In the reaction \(\mathrm{H}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(1) \rightarrow \mathrm{H}_{2}(\mathrm{g})+\) \(\mathrm{OH}^{-}(\mathrm{aq}),\) water acts as both an acid and an oxidizing agent. (c) A precipitate forms when aqueous sodium carbonate, \(\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq}),\) is treated with excess aqueous hydrochloric acid, HCl(aq). (d) Hydrofluoric acid, \(\overline{\mathrm{HF}}\), is a strong acid in water. (e) Compared with a 0.010 M solution of \(\mathrm{NaNO}_{3}\), a \(0.010 \mathrm{M}\) solution of \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) is a better conductor of electricity.

A neutralization reaction between an acid and a base is a common method of preparing useful salts. Give net ionic equations showing how the following salts could be prepared in this way: (a) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4};\) (b) \(\mathrm{NH}_{4} \mathrm{NO}_{3} ;\) and \((\mathrm{c})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\).
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