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Chapter 21: Problem 34

In \(1825,\) Hans Oersted produced aluminum chloride by passing chlorine over a heated mixture of carbon and aluminum oxide. In 1827 , Friedrich Wöhler obtained aluminum by heating aluminum chloride with potassium. Write plausible equations for these reactions.

Short Answer

Expert verified
The balanced equations for the reactions are: 2Al2O3 + 9C + 6Cl2 -> 4AlCl3 + 9CO2 and AlCl3 + 3K -> Al + 3KCl.

Step by step solution

01

Write Equation for First Reaction

In the first reaction, get chlorine gas to react with a heated mixture of carbon and aluminum oxide to produce aluminum chloride. The unbalanced equation would look like this: Al2O3 + C + Cl2 -> AlCl3 + CO2. To balance this equation, correct the reactants and products so the number of each type of atom on each side of the equation is the same: 2Al2O3 + 9C + 6Cl2 -> 4AlCl3 + 9CO2.
02

Write Equation for Second Reaction

In the second reaction, Friedrich Wöhler obtained aluminum by heating aluminum chloride with potassium. The unbalanced equation would be: AlCl3 + K -> Al + KCl. To balance this, correct the amounts of reactants and products so they match on both sides of the equation. The resulting balanced equation is: AlCl3 + 3K -> Al + 3KCl.
03

Double Check the Balanced Equations

After writing the balanced reactions, it is always essential to double-check to ensure that the number of each atom in the reactants equals the number in the products. Double-check the work in steps 1 and 2 to verify they are accurately balanced. This truth assures the mass conservation principle in chemistry.

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Most popular questions from this chapter

The dissolution of \(\mathrm{MgCO}_{3}(\mathrm{s})\) in \(\mathrm{NH}_{4}^{+}(\mathrm{aq})\) can be represented as \(\mathrm{MgCO}_{3}(\mathrm{s})+\mathrm{NH}_{4}^{+}(\mathrm{aq}) \rightleftharpoons\) $$ \mathrm{Mg}^{2+}(\mathrm{aq})+\mathrm{HCO}_{3}^{-}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) $$ Calculate the molar solubility of \(\mathrm{MgCO}_{3}\) in each of the following solutions: (a) \(1.00 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq}) ;\) (b) a buffer that is \(1.00 \mathrm{M} \mathrm{NH}_{3}\) and \(1.00 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl} ;\) (c) a buffer that is \(0.100 \mathrm{M} \mathrm{NH}_{3}\) and \(1.00 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}.\)

Handbooks and lists of chemicals do not contain entries under the formulas \(\mathrm{Al}\left(\mathrm{HCO}_{3}\right)_{3}\) and \(\mathrm{Al}_{2}\left(\mathrm{CO}_{3}\right)_{2} .\) Explain why these compounds do not exist.

Write Lewis structures for the following species, both of which involve coordinate covalent bonding: (a) tetrafluoroborate ion, \(\mathrm{BF}_{4}^{-}\), used in metal cleaning and in electroplating baths (b) boron trifluoride ethylamine, used in curing epoxy resins (ethylamine is \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2}\) )

Write plausible equations for the (a) reaction of \(\mathrm{Al}(\mathrm{s})\) with \(\mathrm{Br}_{2}(1)\) (b) production of \(\mathrm{Cr}\) from \(\mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})\) by the thermite reaction, with Al as the reducing agent; (c) separation of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) impurity from bauxite ore.

A description for preparing potassium aluminum alum calls for dissolving aluminum foil in KOH(aq). The solution obtained is treated with \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}),\) and the alum is crystallized from the resulting solution. Write plausible equations for these reactions.
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