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Chapter 22: Problem 26

\(\mathrm{O}_{3}(\mathrm{g})\) is a powerful oxidizing agent. Write equations to represent oxidation of \((a) I^{-}\) to \(I_{2}\) in acidic solution; (b) sulfur in the presence of moisture to sulfuric acid; (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) to \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\) in basic solution. In each case \(\mathrm{O}_{3}(\mathrm{g})\) is reduced to \(\mathrm{O}_{2}(\mathrm{g})\).

Short Answer

Expert verified
The balanced equations are: (a) 2I^- + O3 + H2O = I2 + 2OH- + O2. (b) S + O3 + H2O2 = H2SO4 + 2H2O + O2. (c) \([\mathrm{Fe}(\mathrm{CN})_{6}]^{4-} + O3 + H2O = [\mathrm{Fe}(\mathrm{CN})_{6}]^{3-} + 2OH- + O2.

Step by step solution

01

Identify the Oxidation State Changes

Identify the changes in oxidation state of the species involved in the reaction. (a) \(I^{-}\) is oxidized to \(I_{2}\). (b) Sulfur is oxidized to sulfuric acid \(H_{2}SO_{4}\). (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}\) is oxidized to \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}\). In each case, \(\mathrm{O}_{3}(\mathrm{g})\) is reduced to \(\mathrm{O}_{2}(\mathrm{g})\).
02

Write Unbalanced Equations

(a) \(I^{-} + O_{3} \rightarrow I_{2} + O_{2}\) (b) \(S + O_{3} \rightarrow H_{2}SO_{4} + O_{2}\) (c) \(\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-} + O_{3} \rightarrow \left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-} + O_{2}\)
03

Balance The Equations using half-reaction method

(a) 2I^- + O3 + H2O = I2 + 2OH- + O2. (b) S + O3 + H2O = H2SO4 + O2. Balance the sulfur and then the oxygen atoms by adding hydrogen peroxide (H2O2) to the left side of the equation and water (H2O) to the right side. (c) \([\mathrm{Fe}(\mathrm{CN})_{6}]^{4-} + O3 = [\mathrm{Fe}(\mathrm{CN})_{6}]^{3-} + O2. Balance the iron and then the oxygen atoms by adding one water (H2O) molecule to the left side of the equation and two hydroxide (OH-) ions to the right side.

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Most popular questions from this chapter

Show by calculation whether the reaction $2 \mathrm{HOCl}(\mathrm{aq}) \longrightarrow \mathrm{HClO}_{2}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq})$ will go essentially to completion as written for standardstate conditions.

Suppose that the sulfur present in seawater as \(\mathrm{SO}_{4}^{2-}\) \(\left(2650 \mathrm{mg} \mathrm{L}^{-1}\right)\) could be recovered as elemental sulfur. If this sulfur were then converted to \(\mathrm{H}_{2} \mathrm{SO}_{4},\) how many cubic kilometers of seawater would have to be processed to yield the average U.S. annual consumption of about 45 million tons of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)

The boiling points of oxygen and argon are \(-183^{\circ} \mathrm{C}\) and \(-189^{\circ} \mathrm{C},\) respectively. Because the boiling points are so similar, argon obtained from the fractional distillation of liquid air is contaminated with oxygen. The following three-step procedure can be used to obtain pure argon from the oxygen-contaminated sample: (1) Excess hydrogen is added to the mixture and then the mixture is ignited. (2) The mixture from step (1) is then passed over hot copper(II) oxide. (3) The mixture from step (2) is passed over a dehydrated zeolite material (see Chapter 21 ). Explain the purpose of each step, writing chemical equations for any reactions that occur.

Write a plausible chemical equation to represent the reaction of \((\mathrm{a}) \mathrm{Cl}_{2}(\mathrm{g}) \quad\) with cold \(\quad \mathrm{NaOH}(\mathrm{aq})\) (b) \(\mathrm{NaI}(\mathrm{s})\) with hot \(\mathrm{H}_{2} \mathrm{SO}_{4}(\text { concd aq }) ;\) (c) \(\mathrm{Cl}_{2}(\mathrm{g})\) with \(\mathrm{KI}_{3}(\mathrm{aq}) ; \quad\) (d) \(\quad \mathrm{NaBr}(\mathrm{s}) \quad\) with hot \(\mathrm{H}_{3} \mathrm{PO}_{4}\) \((\text { concd aq })\) (e) \(\mathrm{NaHSO}_{3}(\mathrm{aq})\) with \(\mathrm{MnO}_{4}^{-1}(\mathrm{aq})\) in dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\).

The bond energies of \(\mathrm{Cl}_{2}\) and \(\mathrm{F}_{2}\) are 243 and \(159 \mathrm{kJ} \mathrm{mol}^{-1},\) respectively. Use these data to explain why \(\mathrm{XeF}_{2}\) is a much more stable compound than \(\mathrm{XeCl}_{2} .[\text { Hint: Recall that Xe exists as a monatomic gas. }]\).
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