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Chapter 21: Problem 90

Write the simplest chemical equation to represent the reaction of (a) \(\mathrm{K}_{2} \mathrm{CO}_{3}\left(\text { aq) and } \mathrm{Ba}(\mathrm{OH})_{2}(\mathrm{aq})\right.\); (b) \(\operatorname{Mg}\left(\mathrm{HCO}_{3}\right)_{2}(\) aq) on heating; (c) tin(II) oxide when heated with carbon; (d) \(\mathrm{CaF}_{2}(\mathrm{s})\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{concd}\) aq); (e) \(\mathrm{NaHCO}_{3}(\mathrm{s})\) and \(\mathrm{HCl}(\mathrm{aq}) ;\) (f) \(\mathrm{PbO}_{2}(\mathrm{s})\) and HBr(aq); and (g) the reduction of \(\mathrm{SiF}_{4}\) to pure \(\mathrm{Si},\) by using Na as the reducing agent.

Short Answer

Expert verified
The reactions are: (a) \(K_2CO_3 + Ba(OH)_2 -> BaCO_3 + 2KOH\), (b) \(Mg(HCO_3)_2 -> MgCO_3 + CO_2 + H_2O\), (c) \(SnO + C -> Sn + CO\), (d) \(CaF_2 + H_2SO_4 -> CaSO_4 + 2HF\), (e) \(NaHCO_3+ HCl -> NaCl + CO_2 + H_2O\), (f) \(PbO_2+ 4HBr -> PbBr_2 + H_2O + Br_2\), (g) \(SiF_4 + 4Na -> 4NaF + Si\).

Step by step solution

01

Reaction of K2CO3(aq) and Ba(OH)2(aq)

K2CO3(aq) + Ba(OH)2(aq) -> BaCO3(s) + 2KOH(aq). This is a double-displacement reaction where the carbonate ion from potassium carbonate combines with barium ion to form barium carbonate, which precipitates out of the solution.
02

Reaction of Mg(HCO3)2(aq) on heating

\(\mathrm{Mg(HCO_3)_2(aq)}\) -> \(\mathrm{MgCO_3 (s) + CO_2(g) + H_2O(g)}\). On heating, magnesium bicarbonate decomposes to form magnesium carbonate, carbon dioxide and water.
03

Reaction of tin(II) oxide when heated with carbon

\(\mathrm{SnO(s) + C(s)}\) -> \(\mathrm{Sn(s) + CO(g)}\). In this redox reaction, carbon reduces tin(II) oxide to elemental tin and is itself oxidized to carbon monoxide.
04

Reaction of CaF2(s) and H2SO4(concd)(aq)

\(\mathrm{CaF_2(s) + H_2SO_4(concd)(aq)}\) -> \(\mathrm{CaSO_4(s) + 2HF (g)}\). This is a double-displacement reaction where the fluoride ion from calcium fluoride displaces the sulfate ion in sulfuric acid.
05

Reaction of NaHCO3(s) and HCl(aq)

\(\mathrm{NaHCO_3(s))+ HCl(aq)\) -> \(\mathrm{NaCl(aq) + CO_2(g) + H_2O(l)}\). Sodium bicarbonate reacts with hydrochloric acid to form sodium chloride, carbon dioxide, and water.
06

Reaction of PbO2 and HBr(aq)

\(\mathrm{PbO_2(s)}\)+ 4HBr(aq) -> \(\mathrm{PbBr_2(aq) + H_2O(l) + Br_2(l)}\). Lead(II) oxide reacts with hydrobromic acid to create lead(II) bromide, water, and bromine.
07

Reduction of SiF4 to Si using Na

\(\mathrm{SiF_4(g)}\)+ 4Na(s) -> \(\mathrm{4NaF(s)+Si(s)}\). Silicon tetrafluoride reacts with sodium to form sodium fluoride and silicon. Sodium serves as the reducing agent in this reaction.

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Most popular questions from this chapter

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 \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NH}_{2}\) ).

There has been some interest in the alkali metal fullerides, \(\mathrm{M}_{n} \mathrm{C}_{60}(\mathrm{s}),\) because at low temperatures, some of these compounds become superconducting. The alkali metal fullerides are ionic crystals comprising \(\mathrm{M}^{+}\) ions and \(\mathrm{C}_{60}^{n-}\) ions. The value of \(n\) can be deduced from the crystal structure. If \(M_{n} C_{60}\) consists of a cubic closest packed array of fulleride ions, with \(\mathrm{M}^{+}\) ions occupying all the octahedral and tetrahedral holes in the fulleride lattice, then what is the value of \(n\) and what is the empirical formula of the fulleride?

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