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Chapter 8: Problem 31

Balance this chemical equation by inspection: \(\mathrm{Al}_{2} \mathrm{Cl}_{6}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Al}(\mathrm{OH})_{3}+\mathrm{HCl}\)

Short Answer

Expert verified
The balanced chemical equation is: \[\mathrm{Al}_{2} \mathrm{Cl}_{6}+6\mathrm{H}_{2} \mathrm{O} \rightarrow 2\mathrm{Al}(\mathrm{OH})_{3}+6\mathrm{HCl}\]

Step by step solution

01

Identify the elements involved

The given chemical equation has four elements: aluminum (Al), chlorine (Cl), hydrogen (H), and oxygen (O).
02

Balance the aluminum (Al) atoms

There are 2 aluminum atoms in \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\) and 1 aluminum atom in \(\mathrm{Al}(\mathrm{OH})_{3}\). To balance the aluminum atoms, place a coefficient of 2 in front of \(\mathrm{Al}(\mathrm{OH})_{3}\): \[\mathrm{Al}_{2} \mathrm{Cl}_{6}+\mathrm{H}_{2} \mathrm{O} \rightarrow 2\mathrm{Al}(\mathrm{OH})_{3}+\mathrm{HCl}\]
03

Balance the chlorine (Cl) atoms

There are 6 chlorine atoms in \(\mathrm{Al}_{2} \mathrm{Cl}_{6}\) and 1 chlorine atom in \(\mathrm{HCl}\). To balance the chlorine atoms, place a coefficient of 6 in front of \(\mathrm{HCl}\): \[\mathrm{Al}_{2} \mathrm{Cl}_{6}+\mathrm{H}_{2} \mathrm{O} \rightarrow 2\mathrm{Al}(\mathrm{OH})_{3}+6\mathrm{HCl}\]
04

Balance the hydrogen (H) and oxygen (O) atoms

Now there are 6 hydrogen atoms in \(\mathrm{HCl}\) and 2 hydrogen atoms in \(\mathrm{H}_{2} \mathrm{O}\), as well as 1 oxygen atom in \(\mathrm{H}_{2} \mathrm{O}\). To balance hydrogen and oxygen atoms, place a coefficient of 6 in front of \(\mathrm{H}_{2} \mathrm{O}\): \[\mathrm{Al}_{2} \mathrm{Cl}_{6}+6\mathrm{H}_{2} \mathrm{O} \rightarrow 2\mathrm{Al}(\mathrm{OH})_{3}+6\mathrm{HCl}\] Now, the equation is balanced, with 2 aluminum (Al) atoms, 6 chlorine (Cl) atoms, 12 hydrogen (H) atoms, and 6 oxygen (O) atoms on both sides of the equation. The balanced chemical equation is: \[\mathrm{Al}_{2} \mathrm{Cl}_{6}+6\mathrm{H}_{2} \mathrm{O} \rightarrow 2\mathrm{Al}(\mathrm{OH})_{3}+6\mathrm{HCl}\]

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Most popular questions from this chapter

Which equations represent chemical reactions: (a) \(\mathrm{CO}_{2}(\mathrm{~s}) \rightarrow \mathrm{CO}_{2}(g)\) (b) \(3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{O}_{3}(g)\) (c) \(\mathrm{NaCl}(s)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{NaOH}(a q)+\mathrm{HCl}(a q)\) (d) \(\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{CH}_{4}(g) \rightarrow \mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g)\)

Fill in this table: $$ \begin{array}{lll} & & \text { Soluble or } \\ \text { Name } & \text { Formula } & \text { insoluble } \\ \hline \text { Sodium phosphate } & & \\ & \mathrm{Ba}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2} & \\ & \left(\mathrm{NH}_{4}\right)_{2} \mathrm{~S} & \\ \text { Iron(II) carbonate } & & \\ \text { Mercury(II) chloride } & & \\ & \mathrm{Co}(\mathrm{OH})_{2} & \\ & \mathrm{HgCl} & \\ \hline \end{array} $$

Classify each compound as acid, base, or salt: (a) \(\mathrm{KCl}\) (b) \(\mathrm{CH}_{3} \mathrm{COOH}\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}\) (d) \(\mathrm{H}_{3} \mathrm{BO}_{3}\) (e) \(\mathrm{LiC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

Write (a) a reaction with all species intact and using \((a q),(s)\), or \((l)\) for the reaction between aqueous solutions of sulfuric acid and calcium hydroxide. (b) What salt is formed as a result of neutralization?

Balance this chemical equation and assign it a reaction type: \(\mathrm{CO}(g)+\mathrm{NO}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{N}_{2}(g)\)
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