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Chapter 21: Problem 51

Starting with aluminum, describe with balanced equations how you would prepare (a) \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\) (b) \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (c) \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) (d) \(\mathrm{NH}_{4} \mathrm{Al}\left(\mathrm{SO}_{4}\right)_{2} \cdot 12 \mathrm{H}_{2} \mathrm{O}\)

Short Answer

Expert verified
Preparation of (a) Al2Cl6 : 2 Al + 3 Cl2 -> 2 AlCl3, (b) Al2O3 : 4 Al + 3 O2 -> 2 Al2O3, (c) Al2(SO4)3 : 2 Al + 3 H2SO4 -> Al2(SO4)3 + 3 H2, (d) NH4Al(SO4)2.12H2O : Al2(SO4)3 + 2(NH4)2SO4 + 24 H2O -> 2 NH4Al(SO4)2.12H2O

Step by step solution

01

Preparation of Al2Cl6

Aluminum will react with Chlorine gas to form Aluminum Chloride (AlCl3). The balanced equation for this reaction is: \n2 Al (s) + 3 Cl2 (g) -> 2 AlCl3 (s)
02

Preparation of Al2O3

Aluminum will react with Oxygen to form Aluminum oxide (Al2O3). The balanced chemical reaction is: \n4 Al (s) + 3 O2 (g) -> 2 Al2O3 (s)
03

Preparation of Al2(SO4)3

Aluminum will react with Sulfuric acid to form Aluminium sulfate (Al2(SO4)3). The balanced equation for the reaction: \n2 Al (s) + 3 H2SO4 (aq) -> Al2(SO4)3 (aq) + 3 H2 (g)
04

Preparation of NH4Al(SO4)2.12H2O

Aluminium sulphate prepared in the previous step can further react with Ammonium sulfate to form Ammonium aluminium sulfate dodecahydrate. The balanced reaction is: \nAl2(SO4)3(aq) + 2(NH4)2SO4(aq) + 24 H2O(l) -> 2 NH4Al(SO4)2.12H2O(s)

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Most popular questions from this chapter

Name the following minerals: (a) \(\mathrm{MgCO}_{3}\), (b) \(\mathrm{Na}_{3} \mathrm{AlF}_{6}\), (c) \(\mathrm{Al}_{2} \mathrm{O}_{3},\) (d) \(\mathrm{Ag}_{2} \mathrm{~S},\) (e) \(\mathrm{HgS},\) (f) \(\mathrm{ZnS},\) (g) \(\mathrm{SrSO}_{4}\) (h) \(\mathrm{PbCO}_{3}\) (i) \(\mathrm{MnO}_{2}\), (j) \(\mathrm{TiO}_{2}\).

It has been shown that \(\mathrm{Na}_{2}\) species form in the vapor phase. Describe the formation of the "disodium molecule" in terms of a molecular orbital energylevel diagram. Would you expect the alkaline earth metals to exhibit a similar property?

Although iron is only about two-thirds as abundant as aluminum in Earth's crust, mass for mass it costs only about one-quarter as much to produce. Why?

Starting with magnesium and concentrated nitric acid, describe how you would prepare magnesium oxide. [Hint: First convert \(\mathrm{Mg}\) to \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\). Next, \(\mathrm{MgO}\) can be obtained by heating \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\).]

Describe a medicinal or health-related application for each of the following compounds: \(\mathrm{NaF}, \mathrm{Li}_{2} \mathrm{CO}_{3}\) \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{CaCO}_{3}, \mathrm{BaSO}_{4}, \mathrm{Al}(\mathrm{OH})_{2} \mathrm{NaCO}_{3} .\) (Youwould need to do a Web search for some of these compounds.)
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