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Chapter 21: Problem 18

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

Short Answer

Expert verified
The exercise involves writing equations for several types of chemical reactions: (a) thermal decomposition, (b) electrolysis, (c) displacement, (d) neutralization and (e) dehydration.

Step by step solution

01

(a) Heating \(\operatorname{Mg}\left(\mathrm{HCO}_{3}\right)_{2}(\mathrm{s})\)

When \(\operatorname{Mg}\left(\mathrm{HCO}_{3}\right)_{2}(\mathrm{s})\) is heated, it decomposes into magnesium oxide (MgO), water (H2O), and carbon dioxide (CO2). It is a type of thermal decomposition reaction. The equation is:\[\operatorname{Mg}\left(\mathrm{HCO}_{3}\right)_{2}(\mathrm{s})\rightarrow \operatorname{MgO}\left(\mathrm{s}\right)+\mathrm{H}_{2}\mathrm{O}(\mathrm{g})+2 \mathrm{CO}_{2}(\mathrm{g})\]
02

(b) Electrolysis of \(\mathrm{BaCl}_{2}(l)\)

Electrolysis involves breaking down a compound into its elements using an electric current. \(\mathrm{BaCl}_{2}\) will break down into barium (Ba) and chlorine (Cl2) gas. The equation is:\[\mathrm{BaCl}_{2}(l) \rightarrow \mathrm{Ba}(s)+\mathrm{Cl}_{2}(g)\]
03

(c) Adding $\operatorname{Sr}\left(\mathrm{s}\right)$ to cold dilute $\operatorname{HBr}\left(\mathrm{aq}\right)$

When strontium (Sr) is added to cold dilute hydrobromic acid (HBr), a displacement reaction occurs, creating strontium bromide (SrBr2) and hydrogen gas (H2). The equation is:\[\mathrm{Sr}\left(\mathrm{s}\right)+2 \mathrm{HBr}\left(\mathrm{aq}\right) \rightarrow \mathrm{SrBr}_{2}\left(\mathrm{aq}\right)+\mathrm{H}_{2}\left(\mathrm{g}\right)\]
04

(d) Adding \(\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq})\) to \(\mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{aq})\)

A neutralization reaction takes place when calcium hydroxide (Ca(OH)2) is added to sulphuric acid (H2SO4), forming calcium sulphate (CaSO4) and water (H2O). The equation is:\[\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{CaSO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})\]
05

(e) Heating \(\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\)

When \(\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s})\), or gypsum, is heated, it loses water and forms a plaster of Paris. This is a type of dehydration reaction. The equation is:\[\mathrm{CaSO}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{CaSO}_{4} \cdot \frac{1}{2} \mathrm{H}_{2} \mathrm{O}(\mathrm{s})+ \frac{3}{2} \mathrm{H}_{2} \mathrm{O}(\mathrm{g})\]

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Most popular questions from this chapter

A chemical dictionary gives the following descriptions of the production of some compounds. Write plausible chemical equations based on these descriptions. (a) lead(II) carbonate: adding a solution of sodium bicarbonate to a solution of lead nitrate. (b) lithium carbonate: reaction of lithium oxide with ammonium carbonate solution. (c) hydrogen peroxide: by the action of dilute sulfuric acid on barium peroxide. (d) lead(IV) oxide: action of an alkaline solution of calcium hypochlorite on lead(II) oxide.

The best oxidizing agent of the following oxides is (a) \(\mathrm{Li}_{2} \mathrm{O} ;(\mathrm{b}) \mathrm{MgO} ;(\mathrm{c}) \mathrm{Al}_{2} \mathrm{O}_{3} ;(\mathrm{d}) \mathrm{CO}_{2} ;(\mathrm{e}) \mathrm{SnO}_{2} ;(\mathrm{f}) \mathrm{PbO}_{2}.\)

An analysis of a Solvay-process plant shows that for every \(1.00 \mathrm{kg}\) of \(\mathrm{NaCl}\) consumed, \(1.03 \mathrm{kg}\) of \(\mathrm{NaHCO}_{3}\) are obtained. The quantity of \(\mathrm{NH}_{3}\) consumed in the overall process is \(1.5 \mathrm{kg}.\) (a) What is the percent efficiency of this process for converting NaCl to \(\mathrm{NaHCO}_{3} ?\) (b) Why is so little \(\mathrm{NH}_{3}\) required?

Although the triiodide ion, \(\mathrm{I}_{3}^{-}\), is known to exist in aqueous solutions, the ion is stable in only certain ionic solids. For example, \(\mathrm{CsI}_{3}\) is stable with respect to decomposition to CsI and \(\mathrm{I}_{2},\) but \(\mathrm{LiI}_{3}\) is not stable with respect to LiI and I \(_{2}\). Draw a Lewis structure for the \(I_{3}^{-}\) ion and suggest a reason why \(\mathrm{CsI}_{3}\) is stable with respect to decomposition to the iodide but \(\mathrm{LiI}_{3}\) is not.

Arrange the following compounds in the expected order of increasing solubility in water, and give the basis for your arrangement: \(\mathrm{Li}_{2} \mathrm{CO}_{3}, \mathrm{Na}_{2} \mathrm{CO}_{3}\) \(\mathrm{MgCO}_{3}.\)
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