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Chapter 20: Problem 44

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) \(\mathrm{Cl}^{-}(a q)\) or \(\mathrm{ClO}_{3}^{-}(a q)\) (d) \(\mathrm{H}_{2} \mathrm{O}_{2}(a q)\) or \(\mathrm{O}_{3}(g)\)

Short Answer

Expert verified
The stronger oxidizing agents for each pair are as follows: (a) Cl鈧�(g), (b) Cd虏鈦�(aq), (c) ClO鈧冣伝(aq), and (d) O鈧�(g).

Step by step solution

01

Look up Standard Reduction Potential values

From the given Appendix E, find the standard reduction potential values for each substance in the pairs provided. 3. Repeat this process for all pairs Once you've found the stronger oxidizing agent in each pair, repeat the process for all four pairs of substances.
02

Solution

03

(a) Cl鈧�(g) or Br鈧�(l)

Look up the values in Appendix E Standard reduction potential for Cl鈧�(g): \(+1.36 \ \mathrm{V}\) Standard reduction potential for Br鈧�(l): \(+1.07 \ \mathrm{V}\) Since Cl鈧�(g) has a higher reduction potential, it is the stronger oxidizing agent.
04

(b) Zn虏鈦�(aq) or Cd虏鈦�(aq)

Look up the values in Appendix E Standard reduction potential for Zn虏鈦�(aq): \(-0.76 \ \mathrm{V}\) Standard reduction potential for Cd虏鈦�(aq): \(-0.40 \ \mathrm{V}\) Since Cd虏鈦�(aq) has a higher reduction potential, it is the stronger oxidizing agent.
05

(c) Cl鈦�(aq) or ClO鈧冣伝(aq)

Look up the values in Appendix E Standard reduction potential for Cl鈦�(aq): \(-1.36 \ \mathrm{V}\) Standard reduction potential for ClO鈧冣伝(aq): \(+1.47 \ \mathrm{V}\) Since ClO鈧冣伝(aq) has a higher reduction potential, it is the stronger oxidizing agent.
06

(d) H鈧侽鈧�(aq) or O鈧�(g)

Look up the values in Appendix E Standard reduction potential for H鈧侽鈧�(aq): \(+0.68 \ \mathrm{V}\) Standard reduction potential for O鈧�(g): \(+2.07 \ \mathrm{V}\) Since O鈧�(g) has a higher reduction potential, it is the stronger oxidizing agent.

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Most popular questions from this chapter

The \(K_{s p}\) value for \(\mathrm{PbS}(s)\) is \(8.0 \times 10^{-28} .\) By using this value together with an electrode potential from Appendix \(\mathrm{E}\), determine the value of the standard reduction potential for the reaction $$\mathrm{PbS}(s)+2 \mathrm{e}^{-} \longrightarrow \mathrm{Pb}(s)+\mathrm{S}^{2-}(a q)$$

(a) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it serves as the anode of a voltaic cell. (b) The platinum electrode in a standard hydrogen electrode is specially prepared to have a large surface area. Why is this important? (c) Sketch a standard hydrogen electrode.

This oxidation-reduction reaction in acidic solution is spontaneous: $$ \begin{array}{r} 5 \mathrm{Fe}^{2+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}^{+}(a q) \longrightarrow \\ 5 \mathrm{Fe}^{3+}(a q)+\mathrm{Mn}^{2+}(a q)+4 \mathrm{H}_{2} \mathrm{O}(l) \end{array} $$ A solution containing \(\mathrm{KMnO}_{4}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is poured into one beaker, and a solution of \(\mathrm{FeSO}_{4}\) is poured into another. A salt bridge is used to join the beakers. A platinum foil is placed in each solution, and a wire that passes through a voltmeter connects the two solutions. (a) Sketch the cell, indicating the anode and the cathode, the direction of electron movement through the external circuit, and the direction of ion migrations through the solutions. (b) Sketch the process that occurs at the atomic level at the surface of the anode. (c) Calculate the emf of the cell under standard conditions. (d) Calculate the emf of the cell at \(298 \mathrm{~K}\) when the concentrations are the fol- $$ \text { lowing: } \mathrm{pH}=0.0,\left[\mathrm{Fe}^{2+}\right]=0.10 \mathrm{M},\left[\mathrm{MnO}_{4}^{-}\right]=1.50 \mathrm{M} $$ \(\left[\mathrm{Fe}^{3+}\right]=2.5 \times 10^{-4} \mathrm{M},\left[\mathrm{Mn}^{2+}\right]=0.001 \mathrm{M}\)

For each of the following reactions, write a balanced equation, calculate the standard emf, calculate \(\Delta G^{\circ}\) at \(298 \mathrm{~K},\) and calculate the equilibrium constant \(K\) at \(298 \mathrm{~K}\). (a) Aqueous iodide ion is oxidized to \(\mathrm{I}_{2}(s)\) by \(\mathrm{Hg}_{2}^{2+}(a q) .\) (b) In acidic solution, copper(I) ion is oxidized to copper(II) ion by nitrate ion. (c) In basic solution, \(\mathrm{Cr}(\mathrm{OH})_{3}(s)\) is oxidized to \(\mathrm{CrO}_{4}^{2-}(a q)\) by \(\mathrm{ClO}^{-}(a q)\).

A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following halfreaction: $$\mathrm{AgCl}(s)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)+\mathrm{Cl}^{-}(a q)$$ The two half-cells have \(\left[\mathrm{Cl}^{-}\right]=0.0150 \mathrm{M}\) and \(\left[\mathrm{Cl}^{-}\right]=\) \(2.55 \mathrm{M},\) respectively. (a) Which electrode is the cathode of the cell? (b) What is the standard emf of the cell? (c) What is the cell emf for the concentrations given? (d) For each electrode, predict whether \(\left[\mathrm{Cl}^{-}\right]\) will increase, decrease, or stay the same as the cell operates.
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