Use the following information to answer questions 29-31.
Pennies are made primarily of zinc, which is coated with a thin layer of
copper through electroplating, using a setup like the one above. The solution
in the beaker is a strong acid (which produces H' ions), and the cell is wired
so that the copper electrode is the anode and zinc penny is the cathode. Use
the following reduction potentials to answer questions \(29-31 .\)
$$\begin{array}{|l|l|}\hline \text { Half-Reaction } & {\text { Standard
Reduction Potential }} \\ \hline \mathrm{Cu}^{2++2 e^{-} \rightarrow
\mathrm{Cu}(s)} & {+0.34 \mathrm{V}} \\ \hline 2 \mathrm{H}^{++2 e^{-}
\rightarrow \mathrm{H}_{2}(g)} & {0.00 \mathrm{V}} \\ \hline
\mathrm{Ni}^{2++2 e^{-} \rightarrow \mathrm{Ni}(s)} & {-0.25 \mathrm{V}} \\\
\hline \mathrm{Zn}^{2++2 e^{-} \rightarrow \mathrm{Zn}(s)} & {-0.76
\mathrm{V}} \\ \hline\end{array}$$
If, instead of copper, a nickel bar were to be used, could nickel be plated
onto the zinc penny effectively? Why or why not?
(A) Yes, nickel’s SRP is greater than that of zinc, which is all that is
required for nickel to be reduced at the cathode
(B) Yes, nickel is able to take electrons from the \(\mathrm{H}^{+}\) ions in
solution, allowing it to be reduced
(C) No, nickel's SRP is lower than that of \(\mathrm{H}^{+}\) ions, which means
the only product being produced at the cathode would be hydrogen gas
(D) No, nickel's SRP is negative, meaning it cannot be reduced in an
electrolytic cell