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Chapter 21: Problem 27

Write chemical equations to represent the (a) reaction of \(\mathrm{Al}(\mathrm{s})\) with \(\mathrm{HCl}(\mathrm{aq})\) (b) reaction of \(\mathrm{Al}(\mathrm{s})\) with \(\mathrm{NaOH}(\mathrm{aq})\) (c) oxidation of \(\mathrm{Al}(\mathrm{s})\) to \(\mathrm{Al}^{3+}(\) aq) by an aqueous solution of sulfuric acid; the reduction product is \(\mathrm{SO}_{2}(\mathrm{g}).\)

Short Answer

Expert verified
(a) \( \mathrm{Al}(\mathrm{s}) + 3\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{AlCl}_{3}(\mathrm{aq}) + 3\mathrm{H}_{2}(\mathrm{g}) \) (b) \( \mathrm{Al}(\mathrm{s}) + 3\mathrm{NaOH}(\mathrm{aq}) \rightarrow 2\mathrm{NaAlO}_{2}(\mathrm{aq}) + 3\mathrm{H}_{2}(\mathrm{g}) \) (c) \(2\mathrm{Al}(\mathrm{s}) + 3\mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Al}_{2}(\mathrm{SO}_4)_{3}(\mathrm{aq}) + 3\mathrm{SO}_2(\mathrm{g}) + 3\mathrm{H}_2\mathrm{O}(\mathrm{l})\)

Step by step solution

01

Reaction of Al(s) with HCl(aq)

When aluminum reacts with Hydrochloric acid, aluminum chloride and hydrogen gas are produced. The unbalanced chemical reaction is: \(\mathrm{Al}(\mathrm{s}) + \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{AlCl}_{3}(\mathrm{aq}) + \mathrm{H}_{2}(\mathrm{g})\). To balance this reaction, it's necessary to add '3' as the coefficient of \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\) on each side of the reaction: \( \mathrm{Al}(\mathrm{s}) + 3\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{AlCl}_{3}(\mathrm{aq}) + 3\mathrm{H}_{2}(\mathrm{g}) \)
02

Reaction of Al(s) with NaOH(aq)

When aluminum reacts with Sodium hydroxide, sodium aluminate and hydrogen gas are produced. The unbalanced chemical reaction is: \(\mathrm{Al}(\mathrm{s}) + \mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{NaAlO}_{2}(\mathrm{aq}) + \mathrm{H}_{2}(\mathrm{g})\). To balance this reaction, it's necessary to add '3' as the coefficient of \(\mathrm{NaOH}\) and \(\mathrm{H}_{2}\), and '2' as the coefficient of \(\mathrm{NaAlO}_{2}\) on each side of the reaction: \( \mathrm{Al}(\mathrm{s}) + 3\mathrm{NaOH}(\mathrm{aq}) \rightarrow 2\mathrm{NaAlO}_{2}(\mathrm{aq}) + 3\mathrm{H}_{2}(\mathrm{g}) \)
03

Oxidation of Al(s) to Al3+(aq) by H2SO4(aq)

When aluminum is oxidized by sulfuric acid, Aluminum sulfate, sulfur dioxide and water are formed. The unbalanced chemical reaction is: \(\mathrm{Al}(\mathrm{s}) + \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Al}_{2}(\mathrm{SO}_4)_{3}(\mathrm{aq}) + \mathrm{SO}_2(\mathrm{g}) + \mathrm{H}_2\mathrm{O}(\mathrm{l})\). To balance this reaction, use '2' as coefficient of \(\mathrm{Al}\), '3' for \(\mathrm{H}_{2}\mathrm{SO}_{4}\) and \(\mathrm{H}_2\mathrm{O}\): \(2\mathrm{Al}(\mathrm{s}) + 3\mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Al}_{2}(\mathrm{SO}_4)_{3}(\mathrm{aq}) + 3\mathrm{SO}_2(\mathrm{g}) + 3\mathrm{H}_2\mathrm{O}(\mathrm{l})\)

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Most popular questions from this chapter

Lithium superoxide, \(\mathrm{LiO}_{2}(\mathrm{s}),\) has never been isolated. Use ideas from Chapter \(12,\) together with data from this chapter and Appendix \(D\), to estimate \(\Delta H_{f}\) for \(\mathrm{LiO}_{2}(\mathrm{s})\) and assess whether \(\mathrm{LiO}_{2}(\mathrm{s})\) is thermodynamically stable with respect to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}).\) (a) Use the Kapustinskii equation, along with appropriate data below, to estimate the lattice energy, \(U,\) for \(\left.\mathrm{LiO}_{2}(\mathrm{s}) . \text { (See exercise } 126 \text { in Chapter } 12 .\right)\) The ionic radii for \(L\) i \(^{+}\) and \(O_{2}^{-}\) are \(73 \mathrm{pm}\) and \(144 \mathrm{pm},\) respectively. (b) Use your result from part (a) in the BornFajans-Haber cycle to estimate \(\Delta H_{\mathrm{f}}^{2}\) for \(\mathrm{LiO}_{2}(\mathrm{s})\) [Hint: For the process \(\mathrm{O}_{2}(\mathrm{g})+\mathrm{e}^{-} \rightarrow \mathrm{O}_{2}^{-}(\mathrm{g}), \Delta H^{\circ}=.\) \(-43 \mathrm{kJ} \mathrm{mol}^{-1} .\) See Table 21.2 and Appendix \(\mathrm{D}\) for the other data that are required.] (c) Use your result from part (b) to calculate the enthalpy change for the decomposition of \(\mathrm{LiO}_{2}(\mathrm{s})\) to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}) .\) For \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s}), \Delta H_{\mathrm{f}}^{\circ}=-598.73\) \(\mathrm{kJmol}^{-1}.\) (d) Use your result from part (c) to decide whether \(\mathrm{LiO}_{2}(\mathrm{s})\) is thermodynamically stable with respect to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}) .\) Assume that entropy effects can be neglected.

The first electrolytic process to produce sodium metal used molten NaOH as the electrolyte. Write probable half-equations and an overall equation for this electrolysis.

Explain the important distinction between each pair of terms: (a) peroxide and superoxide; (b) quicklime and slaked lime; (c) soap and detergent; (d) silicate and silicone; (e) sol and gel.

Describe a simple test for determining whether a pure white solid is LiCl or KCl.

Listed are several pairs of substances. For some pairs, one or both members of the pair react individually with water to produce a gas. For others, neither member of the pair reacts with water. The pair for which each member reacts with water and yields the same gaseous product is (a) \(\mathrm{Al}(\mathrm{s})\) and \(\mathrm{Ba}(\mathrm{s}) ;\) (b) \(\mathrm{Ca}(\mathrm{s})\) and \(\mathrm{CaH}_{2}(\mathrm{s}) ; \quad(\mathrm{c}) \quad \mathrm{Na}(\mathrm{s})\) and \(\mathrm{Na}_{2} \mathrm{O}_{2}(\mathrm{s}) ; \quad\) (d) \(\mathrm{K}(\mathrm{s})\) and \(\mathrm{KO}_{2}(\mathrm{s}) ;(\mathrm{e}) \mathrm{NaHCO}_{3}(\mathrm{s})\) and \(\mathrm{HCl}(\mathrm{aq}).\)
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