Question

9.7 2) Consider a cell that is composed of zinc metal in contact with a solution of zinc sulfate, \( \mathrm{ZnSO}_{4} \), and copper metal in a solution of copper (II) sulfate, \( \mathrm{CuSO}_{4} \). The zinc is shown in the diagram on the left and copper is on the right. Answer the following questions, the reduction half reactions are provided. \begin{tabular}{|c|c|} \hline Reduction Reaction & Reduction Potential \\ \hline \( \mathrm{Zn}^{2+}{ }_{(\mathrm{aq})}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}_{(\mathrm{s})} \) & \( -0.76 \mathrm{~V} \) \\ \hline \( \mathrm{Cu}^{2+}{ }_{(\mathrm{aq})}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}_{(\mathrm{s})} \) & \( 0.34 \mathrm{~V} \) \\ \hline \end{tabular} A) Which is the reduction reaction? B) Which is the oxidation reaction? C) Write the overall reaction D) Calculate the voltage for this cell. E) Label the following on the diagram Zinc electrode - Copper electrode - Zinc solution - Copper solution - Anode - Cathode - Salt Bridge \( \left(\mathrm{NaNO}_{3}\right) \) - Voltage - Draw an arrow to show the direction that the electrons travel - Write the ions present in the salt bridge - Use arrows to indicate the direction that the ions in the salt bridge will travel F) A student suggests that you could use spectroscopy to measure the amount of the solution that has reacted. Which solution would you need to use to test this theory? What visual changes would you expect to see as the reaction progresses?

          9.7
2) Consider a cell that is composed of zinc metal in contact with a solution of zinc sulfate, \( \mathrm{ZnSO}_{4} \), and copper metal in a solution of copper (II) sulfate, \( \mathrm{CuSO}_{4} \). The zinc is shown in the diagram on the left and copper is on the right. Answer the following questions, the reduction half reactions are provided.
\begin{tabular}{|c|c|}
\hline Reduction Reaction & Reduction Potential \\
\hline \( \mathrm{Zn}^{2+}{ }_{(\mathrm{aq})}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}_{(\mathrm{s})} \) & \( -0.76 \mathrm{~V} \) \\
\hline \( \mathrm{Cu}^{2+}{ }_{(\mathrm{aq})}+2 \mathrm{e}^{-} \rightarrow \mathrm{Cu}_{(\mathrm{s})} \) & \( 0.34 \mathrm{~V} \) \\
\hline
\end{tabular}
A) Which is the reduction reaction?
B) Which is the oxidation reaction?
C) Write the overall reaction
D) Calculate the voltage for this cell.
E) Label the following on the diagram
Zinc electrode
- Copper electrode
- Zinc solution
- Copper solution
- Anode
- Cathode
- Salt Bridge \( \left(\mathrm{NaNO}_{3}\right) \)
- Voltage
- Draw an arrow to show the direction that the electrons travel
- Write the ions present in the salt bridge
- Use arrows to indicate the direction that the ions in the salt bridge will travel
F) A student suggests that you could use spectroscopy to measure the amount of the solution that has reacted. Which solution would you need to use to test this theory?
What visual changes would you expect to see as the reaction progresses?

9.7
2) Consider a cell that is composed of zinc metal in contact with a solution of zinc sulfate, ZnSO4, and copper metal in a solution of copper (II) sulfate, CuSO4. The zinc is shown in the diagram on the left and copper is on the right. Answer the following questions, the reduction half reactions are provided.

Reduction Reaction Reduction Potential

Zn^2+(aq)+2 e^-→Zn(s) -0.76 V

Cu^2+(aq)+2 e^-→Cu(s) 0.34 V

A) Which is the reduction reaction?
B) Which is the oxidation reaction?
C) Write the overall reaction
D) Calculate the voltage for this cell.
E) Label the following on the diagram
Zinc electrode
- Copper electrode
- Zinc solution
- Copper solution
- Anode
- Cathode
- Salt Bridge (NaNO3)
- Voltage
- Draw an arrow to show the direction that the electrons travel
- Write the ions present in the salt bridge
- Use arrows to indicate the direction that the ions in the salt bridge will travel
F) A student suggests that you could use spectroscopy to measure the amount of the solution that has reacted. Which solution would you need to use to test this theory?
What visual changes would you expect to see as the reaction progresses?

Added by Elliot E.

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