9.2: Voltaic Cells - Pre-lab
- Page ID
- 544337
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Name: ____________________ Date: ____________________
- Write the balanced equation and calculate the theoretical standard cell potential, \(E_\text{cell}^\circ\), for the following cell:
\(\ce{Zn(s) | Zn^{2+}(aq) || Cu^{2+}(aq) | Cu(s)}\)
- Use the table of standard reduction potentials in your text, or another approved reference, to complete the following table. An example is provided.
|
Electrodes |
Reduction Half-reactions |
Standard Reduction Potential, \(E^\circ\) [V] |
Voltaic Cell Potential, \(E^\circ\) [V] |
|---|---|---|---|
|
\(\enclose{circle}{\textbf{Zn}}\) Cu |
\(\ce{Zn^{2+} + 2e^- -> Zn(s)}\) \(\ce{Cu^{2+} + 2e^- -> Cu(s)}\) |
−0.76 +0.34 |
+1.10 |
|
Cu Ag |
|
|
|
|
Cu Mg |
|
|
|
|
Zn Sn |
|
|
|
|
Cu Sn |
|
|
|
- For the \(\ce{Zn}\)/\(\ce{Cu}\) cell, if the concentration of \(\ce{Zn^{2+}}\) is 0.01 M and the concentration of \(\ce{Cu^{2+}}\) is 1.0 M, will the measured \(E_\text{cell}\) be greater than, less than, or equal to the \(E_\text{cell}^\circ\)? Explain your reasoning based on the Nernst equation.
- Logic Check: You measure a cell potential of \(+0.46 \text{ V}\) for an Unknown Metal \(X\) connected to Copper (\(+0.34 \text{ V}\)).
- If Copper is the cathode (Red), what is the reduction potential of \(X\)?
- If Copper is the anode (Ox), what is the reduction potential of \(X\)?
- Look at a standard potential table. Which scenario matches a real metal (Ag, Mg, Zn, Sn)?
- If Copper is the cathode (Red), what is the reduction potential of \(X\)?