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Chapter 20: Problem 45

By using the data in Appendix \(\mathrm{E}\), determine whether each of the following substances is likely to serve as an oxidant or a reductant: (a) \(\mathrm{Cl}_{2}(g),\) (b) \(\mathrm{MnO}_{4}^{-}(a q,\) acidic solution) (c) \(\mathrm{Ba}(s),\) (d) \(\mathrm{Zn}(s)\)

Short Answer

Expert verified
Using Appendix E, we find that \(\mathrm{Cl}_{2}(g)\) and \(\mathrm{MnO}_{4}^{-}(a q,\) acidic solution) are oxidants due to their positive standard reduction potential values at +1.36 V and +1.51 V, respectively. Conversely, \(\mathrm{Ba}(s)\) and \(\mathrm{Zn}(s)\) are reductants, as they have negative standard reduction potential values at -2.92 V and -0.76 V, respectively.

Step by step solution

01

Locate Standard Reduction Potentials

Refer to Appendix E to find the standard reduction potential values for each given substance.
02

Determine Oxidant or Reductant for \(\mathrm{Cl}_{2}(g)\)

The standard reduction potential for \(\mathrm{Cl}_{2}(g)\) is: \(\mathrm{Cl}_2(g) + 2e^- \rightarrow 2 \mathrm{Cl}^-(aq)\) E° = +1.36 V Since the value is positive, \(\mathrm{Cl}_{2}(g)\) will act as an oxidant.
03

Determine Oxidant or Reductant for \(\mathrm{MnO}_{4}^{-}(a q,\) acidic solution)

The standard reduction potential for \(\mathrm{MnO}_{4}^{-}(a q,\) acidic solution) is: \(\mathrm{MnO}_4^-(aq) + 8\mathrm{H}^+(aq) + 5e^- \rightarrow \mathrm{Mn}^{2+}(aq) + 4\mathrm{H}_2\mathrm{O}(l)\) E° = +1.51 V Since the value is positive, \(\mathrm{MnO}_{4}^{-}(a q,\) acidic solution) will act as an oxidant.
04

Determine Oxidant or Reductant for \(\mathrm{Ba}(s)\)

The standard reduction potential for \(\mathrm{Ba}(s)\) is: \(\mathrm{Ba}^{2+}(aq) + 2e^- \rightarrow \mathrm{Ba}(s)\) E° = -2.92 V Since the value is negative, \(\mathrm{Ba}(s)\) will act as a reductant.
05

Determine Oxidant or Reductant for \(\mathrm{Zn}(s)\)

The standard reduction potential for \(\mathrm{Zn}(s)\) is: \(\mathrm{Zn}^{2+}(aq) + 2e^- \rightarrow \mathrm{Zn}(s)\) E° = -0.76 V Since the value is negative, \(\mathrm{Zn}(s)\) will act as a reductant. In conclusion, \(\mathrm{Cl}_{2}(g)\) and \(\mathrm{MnO}_{4}^{-}(a q,\) acidic solution) are oxidants, while \(\mathrm{Ba}(s)\) and \(\mathrm{Zn}(s)\) are reductants.

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Most popular questions from this chapter

Is each of the following substances likely to serve as an oxidant or a reductant: (a) \(\mathrm{Ce}^{3+}(a q),\) (b) \(\mathrm{Ca}(s),\) (c) \(\mathrm{ClO}_{3}^{-}(a q)_{\text {, }}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5}(g)\) ?

In a galvanic cell the cathode is an \(\mathrm{Ag}^{+}(1.00 \mathrm{M}) / \mathrm{Ag}(s)\) halfcell. The anode is a standard hydrogen electrode immersed in a buffer solution containing \(0.10 \mathrm{M}\) benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) and \(0.050 \mathrm{M}\) sodium benzoate \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-} \mathrm{Na}^{+}\right) .\) The measured cell voltage is \(1.030 \mathrm{~V}\). What is the \(\mathrm{p} K_{a}\) of benzoic acid?

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 \(\mathrm{O}_{3}(g)\)

Gold exists in two common positive oxidation states, +1 and +3. The standard reduction potentials for these oxidation states are $$ \begin{aligned} \mathrm{Au}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \mathrm{Au}(s) & E_{\mathrm{red}}^{o}=+1.69 \mathrm{~V} \\ \mathrm{Au}^{3+}(a q)+3 \mathrm{e}^{-} \longrightarrow \mathrm{Au}(s) & E_{\mathrm{red}}^{\circ}=+1.50 \mathrm{~V} \end{aligned} $$ (a) Can you use these data to explain why gold does not tarnish in the air? (b) Suggest several substances that should be strong enough oxidizing agents to oxidize gold metal. (c) Miners obtain gold by soaking gold-containing ores in an aqueous solution of sodium cyanide. A very soluble complex ion of gold forms in the aqueous solution because of the redox reaction $$ \begin{aligned} 4 \mathrm{Au}(s)+8 \mathrm{NaCN}(a q)+& 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g) \longrightarrow \\ & 4 \mathrm{Na}\left[\mathrm{Au}(\mathrm{CN})_{2}\right](a q)+4 \mathrm{NaOH}(a q) \end{aligned} $$ What is being oxidized and what is being reduced in this reaction? (d) Gold miners then react the basic aqueous product solution from part (c) with Zn dust to get gold metal. Write a balanced redox reaction for this process. What is being oxidized, and what is being reduced?

(a) Assuming standard conditions, arrange the following in order of increasing strength as oxidizing agents in acidic solution: \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}, \mathrm{H}_{2} \mathrm{O}_{2}, \mathrm{Cu}^{2+}, \mathrm{Cl}_{2}, \mathrm{O}_{2} .\) (b) Arrange the fol- lowing in order of increasing strength as reducing agents in acidic solution: \(\mathrm{Zn}, \mathrm{I}^{-}, \mathrm{Sn}^{2+}, \mathrm{H}_{2} \mathrm{O}_{2}, \mathrm{Al}\).
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