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Chapter 23: Problem 59

Attempts to make \(\mathrm{CuI}_{2}\) by the reaction of \(\mathrm{Cu}^{2+}(\mathrm{aq})\) and \(\mathrm{I}^{-}(\text {aq })\) produce \(\mathrm{CuI}(\mathrm{s})\) and \(\mathrm{I}_{3}^{-}(\mathrm{aq})\) instead. Without performing detailed calculations, show why this reaction should occur. $$2 \mathrm{Cu}^{2+}(\mathrm{aq})+5 \mathrm{I}^{-}(\mathrm{aq}) \longrightarrow 2 \mathrm{CuI}(\mathrm{s})+\mathrm{I}_{3}^{-}(\mathrm{aq})$$

Short Answer

Expert verified
The reaction \[2 \mathrm{Cu}^{2+}(\mathrm{aq})+5 \mathrm{I}^{-}(\mathrm{aq})\longrightarrow 2 \mathrm{CuI}(\mathrm{s})+\mathrm{I}_{3}^{-}(\mathrm{aq})\] produces \(\mathrm{CuI}(\mathrm{s})\) and \(\mathrm{I}_{3}^{-}(\mathrm{aq})\) instead of \(\mathrm{CuI}_{2}\) because these are the more thermodynamically stable compounds. Iodides are less stable than other halides which explains why \( \mathrm{I}_{3}^{-}(\mathrm{aq}) \) is formed.

Step by step solution

01

Analyze the given reaction

Looking at the reaction, \[2 \mathrm{Cu}^{2+}(\mathrm{aq})+5 \mathrm{I}^{-}(\mathrm{aq})\longrightarrow 2 \mathrm{CuI}(\mathrm{s})+\mathrm{I}_{3}^{-}(\mathrm{aq})\], we see that when \(\mathrm{Cu}^{2+}(\mathrm{aq})\) and \(\mathrm{I}^{-}(\text {aq })\) are combined, they produce \(\mathrm{CuI}(\mathrm{s})\) and \(\mathrm{I}_{3}^{-}(\mathrm{aq})\), not \(\mathrm{CuI}_{2}\).
02

Identify thermodynamically stable products

In a chemical reaction, the products that are formed are generally the ones that have lower energy and are more stable. In this case, \(\mathrm{CuI}(\mathrm{s})\) and \(\mathrm{I}_{3}^{-}(\mathrm{aq})\) are more stable than \(\mathrm{CuI}_{2}\). Therefore, \(\mathrm{CuI}(\mathrm{s})\) and \(\mathrm{I}_{3}^{-}(\mathrm{aq})\) are produced instead of \(\mathrm{CuI}_{2}\).
03

Justification based on Periodic trends

In the periodic table, as we go down the group, the halides become less stable. That means iodides (I-) are less stable when compared to the upper halides which justifies why \(\mathrm{I}_{3}^{-}\) is produced.

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Most popular questions from this chapter

Both \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})\) and \(\mathrm{MnO}_{4}^{-}(\mathrm{aq})\) can be used to titrate \(\mathrm{Fe}^{2+}(\mathrm{aq})\) to \(\mathrm{Fe}^{3+}(\mathrm{aq}) .\) Suppose you have available as titrants two solutions: \(0.1000 \mathrm{M} \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq})\) and \(0.1000 \mathrm{M} \mathrm{MnO}_{4}^{-}(\mathrm{aq})\). (a) For which solution would the greater volume of titrant be required for the titration of a particular sample of \(\mathrm{Fe}^{2+}(\text { aq }) ?\) Explain. (b) How many \(\mathrm{mL}\) of \(0.1000 \mathrm{M} \mathrm{MnO}_{4}^{-}(\) aq) would be required for a titration if the same titration requires \(24.50 \mathrm{mL}\) of \(0.1000 \mathrm{M} \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(\mathrm{aq}) ?\)

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