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Chapter 23: Problem 85

Of the following, the two solids that will liberate \(\mathrm{Cl}_{2}(\mathrm{g})\) when heated with \(\mathrm{HCl}(\mathrm{aq})\) are \((\mathrm{a}) \mathrm{NaCl}(\mathrm{s})\) (b) \(\mathrm{ZnCl}_{2}(\mathrm{s}) ;(\mathrm{c}) \mathrm{MnO}_{2}(\mathrm{s}) ;(\mathrm{d}) \mathrm{CuO}(\mathrm{s}) ;(\mathrm{e}) \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(\mathrm{s})\) (f) \(\mathrm{NaOH}(\mathrm{s})\)

Short Answer

Expert verified
The two solids that will liberate \(Cl_{2}(g)\) when heated with \(HCl(aq)\) are \(MnO_{2}(s)\) and \(K_{2}Cr_{2}O_{7}(s)\).

Step by step solution

01

Use Reactivity Series

Firstly, we need to use the reactivity series or electrochemical series. In the electrochemical series, the displacement of Chlorine would occur by elements that are above it in the series. So, from the given options, \(MnO_{2}(s)\) and \(K_{2}Cr_{2}O_{7}(s)\) can displace Chlorine as Manganese and Chromium are above Chlorine in the reactivity series.
02

Formulate the Reactions

Let's illustrate this with balanced chemical equations. For \(MnO_{2}(s)\), the reaction with \(HCl(aq)\) can be written as: \(4HCl(aq) + MnO_{2}(s) \rightarrow MnCl_{2}(aq) + 2H_{2}O(l) + Cl_{2}(g)\). Similarly, for \(K_{2}Cr_{2}O_{7}(s)\), the reaction with \(HCl(aq)\) can be written as: \(14HCl(aq) + K_{2}Cr_{2}O_{7}(s) \rightarrow 2KCl(aq) + 2CrCl_{3}(s) + 7H_{2}O(l) + 3Cl_{2}(g)\). In both reactions, \(Cl_{2}(g)\) is liberated and therefore, the solids \(MnO_{2}(s)\) and \(K_{2}Cr_{2}O_{7}(s)\) meet the condition imposed by the question.

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Most popular questions from this chapter

You are given these three reducing agents: \(\mathrm{Zn}(\mathrm{s})\) \(\mathrm{Sn}^{2+}(\mathrm{aq}),\) and \(\mathrm{I}^{-}(\mathrm{aq}) .\) Use data from Appendix \(\mathrm{D}\) to determine which of them can, under standard-state conditions in acidic solution, reduce (a) \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})\) to \(\mathrm{Cr}^{3+}(\mathrm{aq})\) (b) \(\mathrm{Cr}^{3+}(\text { aq })\) to \(\mathrm{Cr}^{2+}(\mathrm{aq})\) (c) \(\mathrm{SO}_{4}^{2-}(\text { aq })\) to \(\mathrm{SO}_{2}(\mathrm{g})\)

The text mentions that scandium metal is obtained from its molten chloride by electrolysis, and that titanium is obtained from its chloride by reduction with magnesium. Why are these metals not obtained by the reduction of their oxides with carbon (coke), as are metals such as zinc and iron?

Although Au reacts with and dissolves in aqua regia (3 parts \(\mathrm{HCl}+1\) part \(\mathrm{HNO}_{3}\) ), Ag does not dissolve. What is (are) the likely reason(s) for this difference?

With only minor irregularities, the melting points of the first series of transition metals rise from that of Sc to that of Cr and then fall to that of Zn. Give a plausible explanation for this phenomenon based on atomic structure.

Describe the chemical composition of the material called (a) pig iron; (b) ferromanganese alloy; (c) chromite ore; (d) brass; (e) aqua regia; (f) blister copper; (g) stainless steel.
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