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Chapter 18: Problem 5

You want to “plate out” nickel metal from a nickel nitrate solution onto a piece of metal inserted into the solution. Should you use copper or zinc? Explain.

Short Answer

Expert verified
In conclusion, to plate out nickel metal from a nickel nitrate solution, zinc should be used instead of copper. This is because zinc is more reactive than nickel and is lower in the electrochemical series (Zn²⁺/Zn = -0.76 V) compared to nickel (Ni²⁺/Ni = -0.25 V). Therefore, zinc will displace nickel ions in the solution, allowing the plating process to occur. On the other hand, copper is less reactive than nickel and will not be able to displace the nickel ions, rendering it unsuitable for plating nickel.

Step by step solution

01

Understand the Electrochemical Series

The electrochemical series is a list of elements arranged in the order of their standard electrode potentials. Elements higher up in the series are more likely to accept electrons and undergo reduction, while elements lower in the series are more likely to lose electrons and undergo oxidation. In relatively simple words, elements higher in the series are more reactive, and elements lower in the series are less reactive.
02

Find the Positions of Nickel, Copper, and Zinc in the Electrochemical Series

We need to locate the positions of nickel, copper, and zinc in the electrochemical series. Their standard electrode potentials are as follows: Nickel (Ni²⁺/Ni) = -0.25 V Copper (Cu²⁺/Cu) = +0.34 V Zinc (Zn²⁺/Zn) = -0.76 V
03

Compare the Reactivity of Copper and Zinc Relative to Nickel

From the standard electrode potentials, we can see that: - Nickel is higher in the electrochemical series compared to copper (Ni²⁺/Ni = -0.25 V and Cu²⁺/Cu = +0.34 V). This means that copper will not displace nickel from the nickel nitrate solution, as it is less reactive than nickel. - Zinc is lower in the electrochemical series compared to nickel (Ni²⁺/Ni = -0.25 V and Zn²⁺/Zn = -0.76 V). This means that zinc will displace nickel from the nickel nitrate solution, as it is more reactive than nickel.
04

Determine the Suitable Metal for Plating Nickel

Based on the comparison of reactivity, using zinc (the more reactive metal) will allow us to plate out nickel metal from the nickel nitrate solution successfully, as it will displace the nickel ions in the solution. On the other hand, using copper (the less reactive metal) will not result in plating nickel, as it won't be able to displace the nickel ions. In conclusion, we should use zinc to plate out nickel metal from the nickel nitrate solution.

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Most popular questions from this chapter

An electrochemical cell consists of a nickel metal electrode immersed in a solution with \(\left[\mathrm{Ni}^{2+}\right]=1.0 M\) separated by a porous disk from an aluminum metal electrode immersed in a solution with \(\left[\mathrm{Al}^{3+}\right]=1.0 M .\) Sodium hydroxide is added to the aluminum compartment, causing \(\mathrm{Al}(\mathrm{OH})_{3}(s)\) to precipitate. After precipitation of Al(OH) \(_{3}\) has ceased, the concentration of \(\mathrm{OH}^{-}\) is \(1.0 \times 10^{-4} M\) and the measured cell potential is 1.82 \(\mathrm{V}\) . Calculate the \(K_{\mathrm{sp}}\) value for \(\mathrm{Al}(\mathrm{OH})_{3}\). $$\mathrm{Al}(\mathrm{OH})_{3}(s) \rightleftharpoons \mathrm{Al}^{3+}(a q)+3 \mathrm{OH}^{-}(a q) \quad K_{\mathrm{sp}}=?$$

In the electrolysis of an aqueous solution of $\mathrm{Na}_{2} \mathrm{SO}_{4},$ what reactions occur at the anode and the cathode (assuming standard conditions)? $$\begin{array}{ll} {\text{}} & \quad{ \mathscr{E}^{\circ} } \\ \hline {\mathrm{S}_{2} \mathrm{O}_{8}^{2-}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{SO}_{4}^{2-}} & {2.01 \mathrm{V}} \\ {\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}} & {1.23 \mathrm{V}} \\ {2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow \mathrm{H}_{2}+2 \mathrm{OH}^{-}} & {-0.83 \mathrm{V}} \\\ {\mathrm{Na}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Na}} & {-2.71 \mathrm{V}}\end{array}$$

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One of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce 1,4-dicyanobutane. The reduction reaction is $$2 \mathrm{CH}_{2}=\mathrm{CHCN}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}$$ The \(\mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}\) is then chemically reduced using hydrogen gas to $\mathrm{H}_{2} \mathrm{N}-\left(\mathrm{CH}_{2}\right)_{6}-\mathrm{NH}_{2},$ which is used to produce production of nylon. What current must be used to produce \(150 . \mathrm{kg} \mathrm{NC}-\left(\mathrm{CH}_{2}\right)_{4}-\mathrm{CN}\) per hour?
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