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Chapter 20: Problem 42

From each of the following pairs of substances, use data in Appendix \(\mathrm{E}\) to choose the one that is the stronger oxidizing agent: (a) \(\mathrm{Cl}_{2}(g)\) or \(\mathrm{Br}_{2}(l)\) (b) \(\mathrm{Zn}^{2+}(a q)\) or \(\mathrm{Cd}^{2+}(a q)\) (c) \(\mathrm{BrO}_{3}^{-}(a q)\) or \(\mathrm{IO}_{3}^{-}(a q)\) (d) \(\mathrm{H}_{2} \mathrm{O}_{2}(a q)\) or \(\mathrm{O}_{3}(g)\)

Short Answer

Expert verified
(a) \(Cl_{2}(g)\) is the stronger oxidizing agent. (b) \(Cd^{2+}(aq)\) is the stronger oxidizing agent. (c) \(BrO_{3}^-(aq)\) is the stronger oxidizing agent. (d) \(O_{3}(g)\) is the stronger oxidizing agent.

Step by step solution

01

Look up the reduction potential values for each substance

Search for the substances in Appendix E. Appendix E should have a table showing the standard reduction potentials for various substances.
02

Compare the standard reduction potentials for each pair

Determine the stronger oxidizing agent by comparing each reduction potential value. The substance with the more positive (higher) reduction potential is the stronger oxidizing agent. (a) For \(Cl_{2}(g)\) and \(Br_{2}(l)\): \(Cl_{2}(g) + 2e^- \rightarrow 2Cl^-(aq)\), \(E^\circ = +1.36\, V\) \(Br_{2}(l) + 2e^- \rightarrow 2Br^-(aq)\), \(E^\circ = +1.07\, V\) \(Cl_{2}(g)\) has a more positive reduction potential, so it is the stronger oxidizing agent. (b) For \(Zn^{2+}(aq)\) and \(Cd^{2+}(aq)\): \(Zn^{2+}(aq) + 2e^- \rightarrow Zn(s)\), \(E^\circ = -0.76\, V\) \(Cd^{2+}(aq) + 2e^- \rightarrow Cd(s)\), \(E^\circ = -0.40\, V\) \(Cd^{2+}(aq)\) has a more positive reduction potential, so it is the stronger oxidizing agent. (c) For \(BrO_{3}^-(aq)\) and \(IO_{3}^-(aq)\): \(BrO_{3}^-(aq) + 6H^+(aq) + 6e^- \rightarrow Br^-(aq) + 3H_2O(l)\), \(E^\circ = +1.49\, V\) \(IO_{3}^-(aq) + 6H^+(aq) + 6e^- \rightarrow I^-(aq) + 3H_2O(l)\), \(E^\circ = +1.21\, V\) \(BrO_{3}^-(aq)\) has a more positive reduction potential, so it is the stronger oxidizing agent. (d) For \(H_{2}O_{2}(aq)\) and \(O_{3}(g)\): \(H_{2}O_{2}(aq) + 2H^+(aq) + 2e^- \rightarrow 2H_2O(l)\), \(E^\circ = +1.77\, V\) \(O_{3}(g) + 2H^+(aq) + 2e^- \rightarrow O_{2}(g) + H_2O(l)\), \(E^\circ = +2.07\, V\) \(O_{3}(g)\) has a more positive reduction potential, so it is the stronger oxidizing agent.

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Most popular questions from this chapter

(a) \(\mathrm{A} \mathrm{Cr}^{3+}(a q)\) solution is electrolyzed, using a current of \(7.60 \mathrm{~A}\). What mass of \(\mathrm{Cr}(s)\) is plated out after \(2.00\) days? (b) What amperage is required to plate out \(0.250 \mathrm{~mol} \mathrm{Cr}\) from a \(\mathrm{Cr}^{3+}\) solution in a period of \(8.00 \mathrm{~h}\) ?

A voltaic cell is constructed that uses the following reaction and operates at \(298 \mathrm{~K}\) : $$ \mathrm{Zn}(s)+\mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{Zn}^{2+}(a q)+\mathrm{Ni}(s) $$ (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when \(\left[\mathrm{Ni}^{2+}\right]=3.00 \mathrm{M}\) and \(\left[\mathrm{Zn}^{2+}\right]=0.100 \mathrm{M} ?\) (c) What is the emf of the cell when \(\left[\mathrm{Ni}^{2+}\right]=0.200 M\), and \(\left[\mathrm{Zn}^{2+}\right]=0.900 \mathrm{M} ?\)

Indicate whether the following balanced equations involve oxidation-reduction. If they do, identify the elements that undergo changes in oxidation number. (a) \(\mathrm{PBr}_{3}(l)+3 \mathrm{H}_{2} \mathrm{O}(l)--\rightarrow \mathrm{H}_{3} \mathrm{PO}_{3}(a q)+3 \mathrm{HBr}(a q)\) (b) \(\mathrm{NaI}(a q)+3 \mathrm{HOCl}(a q)-\cdots \rightarrow \mathrm{NaIO}_{3}(a q)+3 \mathrm{HCl}(a q)\) (c) \(3 \mathrm{SO}_{2}(g)+2 \mathrm{HNO}_{3}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)--\rightarrow\) $$ 3 \mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NO}(g) $$ (d) \(2 \mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaBr}(s)--\rightarrow\) \(\mathrm{Br}_{2}(l)+\mathrm{SO}_{2}(g)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (a) \(\mathrm{Mo}^{3+}(a q) \longrightarrow \mathrm{Mo}(s)\) (acidic or basic solution) (b) \(\mathrm{H}_{2} \mathrm{SO}_{3}(a q)--\rightarrow \mathrm{SO}_{4}^{2-}(a q)\) (acidic solution) (c) \(\mathrm{NO}_{3}^{-}(a q)-\cdots \rightarrow \mathrm{NO}(g)\) (acidic solution) (d) \(\mathrm{O}_{2}(\mathrm{~g})-\longrightarrow \mathrm{H}_{2} \mathrm{O}(l)\) (acidic solution) (e) \(\mathrm{Mn}^{2+}(a q)-\rightarrow \rightarrow \mathrm{MnO}_{2}(s)\) (basic solution) (f) \(\mathrm{Cr}(\mathrm{OH})_{3}(s)-\cdots \mathrm{CrO}_{4}^{2-}(a q)\) (basic solution) (g) \(\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)\) (basic solution)

Using data from Appendix \(\mathrm{E}\), calculate the equilibrium constant for the disproportionation of the copper(I) ion at room temperature: \(2 \mathrm{Cu}^{+}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+\mathrm{Cu}(s)\)
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