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Using this activity chart, which reaction will happen when a piece of copper is placed in a lead nitrate solution?

\begin{tabular}{|l|l|}
\hline \multicolumn{2}{|l|}{Activity Series} \\
\hline [tex]$Pb$[/tex] & \\
\hline [tex]$Cu$[/tex] & \multirow{1}{*|}{} \\
\hline
\end{tabular}

A. \(2 Cu + 3 Pb \left( NO_3 \right)_2 \rightarrow 3 Cu \left( NO_3 \right)_2 + 2 Pb\)

B. No reaction occurs.

C. \(2 Cu + 3 Pb \left( NO_3 \right)_2 \rightarrow 2 Cu \left( NO_3 \right)_2 + 3 Pb\)

D. \(3 Cu + 3 Pb \left( NO_3 \right)_2 \rightarrow 3 Cu \left( NO_3 \right)_2 + 3 Pb\)

E. The answer cannot be determined from the information given.



Answer :

GinnyAnswer
To determine whether a reaction will occur when copper (Cu) is placed in lead nitrate (\(Pb(NO_3)_2\)) solution, we need to refer to the activity series of metals.

The activity series of metals ranks metals according to their reactivity, with the most reactive metals at the top and the least reactive at the bottom. A more reactive metal can displace a less reactive metal from its compound, but not vice versa.

Given our activity series:
[tex]\[ \begin{tabular}{|l|} \hline Activity series \\ \hline Pb \\ \hline Cu \\ \hline \end{tabular} \][/tex]

From this series, we see that lead (Pb) is more reactive than copper (Cu).

According to the rules of the activity series:
- A metal can displace another metal from a compound if it is higher in the activity series.
- A less reactive metal cannot displace a more reactive metal from its compound.

Here, copper has a lower reactivity compared to lead. Since copper is less reactive than lead, copper cannot displace lead from its compound \(Pb(NO_3)_2\).

Thus, there will be no reaction when copper is placed in a lead nitrate solution.

Therefore, the correct answer is:

B. No reaction occurs.

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