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Chapter 21: Problem 92

Write chemical equations to represent the most probable outcome in each of the following. If no reaction is likely to occur, so state. (a) \(\mathrm{B}(\mathrm{OH})_{3} \stackrel{\Delta}{\longrightarrow}\) (b) \(\mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow}\) (c) \(\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s}) \stackrel{\Delta}{\longrightarrow}\)

Short Answer

Expert verified
(a) \(\mathrm{B(OH)_3}\) \(\stackrel{\Delta}{\longrightarrow}\) \(\mathrm{B_2O_3}\) + \(3 \mathrm{H_2O}\) (b) \(\mathrm{Al_2O_3}\) \(\stackrel{\Delta}{\longrightarrow}\) no reaction (c) \(\mathrm{CaSO_4 \cdot 2 H_2O}\) \(\stackrel{\Delta}{\longrightarrow} \mathrm{CaSO_4 \cdot 0.5 H_2O}\) + \(1.5 \mathrm{H_2O}\)

Step by step solution

01

Analyze boron hydroxide

Heat causes boron hydroxide (\(\mathrm{B(OH)_3}\)) to decompose into boron trioxide and water. The chemical equation is: \(\mathrm{B(OH)_3}\) \( \stackrel{\Delta}{\longrightarrow}\) \(\mathrm{B_2O_3}\) + \(3 \mathrm{H_2O}\)
02

Analyze aluminum oxide

Aluminium oxide (\(\mathrm{Al_2O_3}\)) is a very stable compound and does not decompose upon heating. Thus, no reaction occurs, which we can write as: \(\mathrm{Al_2O_3}\) \(\stackrel{\Delta}{\longrightarrow}\) no reaction
03

Analyze Calcium sulfate dihydrate

Calcium sulfate dihydrate (\(\mathrm{CaSO_4 \cdot 2 H_2O}\)) loses two water molecules upon heating to form Calcium sulfate hemihydrate, the equation being: \(\mathrm{CaSO_4 \cdot 2 H_2O}\) \(\stackrel{\Delta}{\longrightarrow} \mathrm{CaSO_4 \cdot 0.5 H_2O}\) + \(1.5 \mathrm{H_2O}\)

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Most popular questions from this chapter

A particular water sample contains 56.9 ppm \(\mathrm{SO}_{4}^{2-}\) and \(176 \mathrm{ppm} \mathrm{HCO}_{3}^{-},\) with \(\mathrm{Ca}^{2+}\) as the only cation. (a) How many parts per million of \(\mathrm{Ca}^{2+}\) does the water contain? (b) How many grams of \(\mathrm{CaO}\) are consumed in removing \(\mathrm{HCO}_{3}^{-}\), from \(602 \mathrm{kg}\) of the water? (c) Show that the \(\mathrm{Ca}^{2+}\) remaining in the water after the treatment described in part (b) can be removed by adding \(\mathrm{Na}_{2} \mathrm{CO}_{3}.\) (d) How many grams of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) are required for the precipitation referred to in part (c)?

In the Dow process (Fig. \(21-13\) ), the starting material is \(\mathrm{Mg}^{2+}\) in seawater and the final product is Mg metal. This process seems to violate the principle of conservation of charge. Does it? Explain.

Write chemical equations for the reactions you would expect to occur when (a) \(\operatorname{Mg}\left(\mathrm{HCO}_{3}\right)_{2}(\mathrm{s})\) is heated to a high temperature (b) \(\mathrm{BaCl}_{2}(1)\) is electrolyzed (c) \(\operatorname{Sr}(\text { s) is added to cold dilute } \operatorname{HBr}( \text { aq) }\) (d) \(\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq})\) is added to \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\) (e) \(\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\) is heated

A chemical that should exist as a crystalline solid is seen to be a mixture of a solid and liquid in a container on a storeroom shelf. Give a plausible reason for that observation. Should the chemical be discarded or is it still useful for some purposes?

Use information from the chapter to write chemical equations to represent each of the following: (a) reaction of rubidium metal with water (b) thermal decomposition of aqueous \(\mathrm{KHCO}_{3}\) (c) combustion of lithium metal in oxygen gas (d) action of concentrated aqueous \(\mathrm{H}_{2} \mathrm{SO}_{4}\) on \(\mathrm{KCl}(\mathrm{s})\) (e) reaction of lithium hydride with water
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