/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 46 An aqueous solution of \(\mathrm... [FREE SOLUTION] | 91影视

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Chapter 22: Problem 46

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q)\), (b) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+}\), (c) aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) to mercury metal. Write balanced equations for these reactions.

Short Answer

Expert verified
The balanced equations for the given reactions are: (a) \(8H^{+} + 5SO_{2} + 2KMnO_{4} \to 5MnSO_{4} + 8H_{2}O\) (b) \(6SO_{2} + 14H^{+} + 2K_{2}Cr_{2}O_{7} \to 4Cr^{3+} + 6SO_{4}^{2-} + 7H_{2}O\) (c) \(2Hg_{2}(NO_{3})_{2} + 4H^{+} + 2SO_{2} \to 4Hg + 2SO_{4}^{2-} + 6H^{+}\)

Step by step solution

01

Identify the products for each reaction

(a) KMnO4 + SO2 -> MnSO4 (b) K2Cr2O7 + SO2 -> Cr3+ + SO4^2- (c) Hg2(NO3)2 + SO2 -> Hg + SO4^2-
02

Balance the oxygens and hydrogens

(a) KMnO4 + H2O + SO2 -> MnSO4 (b) K2Cr2O7 + 7H2O + 3SO2 -> 2Cr3+ + 3SO4^2- + 14H+ (c) Hg2(NO3)2 + 2H2O + SO2 -> 2Hg + SO4^2- + 4H+
03

Balance the charges

(a) 8H+ + KMnO4 + 5e- + SO2 -> Mn2+ + 4H2O (b) 6e- + 14H+ + K2Cr2O7 + 3SO2 -> 2Cr3+ + 3SO4^2- + 7H2O (c) 2e- + 4H+ + Hg2(NO3)2 + SO2 -> 2Hg + SO4^2- + 6H+
04

Combine the half-reaction equations

(a) 8H+ + 5SO2 + 2KMnO4 -> 5MnSO4 + 8H2O (b) 6SO2 + 14H+ + 2K2Cr2O7 -> 4Cr3+ + 6SO4^2- + 7H2O (c) 2Hg2(NO3)2 + 4H+ + 2SO2 -> 4Hg + 2SO4^2- + 6H+

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Most popular questions from this chapter

Carbon forms an unusual unstable oxide of formula \(\mathrm{C}_{3} \mathrm{O}_{2}\), called carbon suboxide. Carbon suboxide is made by using \(\mathrm{P}_{2} \mathrm{O}_{5}\) to dehydrate the dicarboxylic acid called malonic acid, which has the formula \(\mathrm{HOOC}-\mathrm{CH}_{2}-\mathrm{COOH}\). (a) Write a balanced reaction for the production of carbon suboxide from malonic acid. (b) How many grams of carbon suboxide could be made from \(20.00 \mathrm{~g}\) of malonic acid? (c) Suggest a Lewis structure for \(\mathrm{C}_{3} \mathrm{O}_{2}\) - (Hint: The Lewis structure of malonic acid suggests which atoms are connected to which.) (d) By using the information in Table 8.5, predict the \(\mathrm{C}-\mathrm{C}\) and \(\mathrm{C}-\mathrm{O}\) bond lengths in \(\mathrm{C}_{3} \mathrm{O}_{2}\). (e) Sketch the Lewis structure of a product that could result by the addition of \(2 \mathrm{~mol}\) of \(\mathrm{H}_{2}\) to \(1 \mathrm{~mol}\) of \(\mathrm{C}_{3} \mathrm{O}_{2}\) -

Name the following compounds and assign oxidation states to the halogens in them: (a) \(\mathrm{Fe}\left(\mathrm{ClO}_{3}\right)_{3}\), (b) \(\mathrm{HClO}_{2}\), (c) \(\mathrm{XeF}_{60}\) (d) \(\mathrm{BrF}_{5}\), (e) \(\mathrm{XeOF}_{4}\), (f) \(\mathrm{HIO}_{3}\),

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium nitrite, (b) ammonia, (c) nitrous oxide, (d) sodium cyanide, (e) nitric acid, (f) nitrogen dioxide, (g) nitrogen, (h) boron nitride.

(a) The \(\mathrm{P}_{4}, \mathrm{P}_{4} \mathrm{O}_{6}\) and \(\mathrm{P}_{4} \mathrm{O}_{10}\) molecules have a common structural feature of four \(\mathrm{P}\) atoms arranged in a tetrahedron (Figures \(22.27\) and 22.28). Does this mean that the bonding between the \(\mathrm{P}\) atoms is the same in all these cases? Explain. (b) Sodium trimetaphosphate \(\left(\mathrm{Na}_{3} \mathrm{P}_{3} \mathrm{O}_{9}\right)\) and sodium tetrametaphosphate \(\left(\mathrm{Na}_{4} \mathrm{P}_{4} \mathrm{O}_{12}\right)\) are used as water-softening agents. They contain cyclic \(\mathrm{P}_{3} \mathrm{O}_{9}{ }^{3-}\) and \(\mathrm{P}_{4} \mathrm{O}_{12}{ }^{4-}\) ions, respectively. Propose reasonable structures for these ions.

Indicate whether each of the following statements is true or false (a) \(\mathrm{H}_{2}(g)\) and \(\mathrm{D}_{2}(g)\) are allotropic forms of hydrogen. (b) \(\mathrm{ClF}_{3}\) is an interhalogen compound. (c) \(\mathrm{MgO}(\) s) is an acidic anhydride. (d) \(\mathrm{SO}_{2}(g)\) is an acidic anhydride. (c) \(2 \mathrm{H}_{3} \mathrm{PO}_{4}(l) \rightarrow \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}(l)+\mathrm{H}_{2} \mathrm{O}(g)\) is an example of a condensation reaction. (f) Tritium is an isotope of the element hydrogen. (g) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g)\) is an example of a disproportionation reaction.
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