Questions: In this lab we will be building a voltaic cell using Cu / Cu^2+ and Zn / Zn^2+. Write the two half reactions (one as a reduction and one as an oxidation based on forming a spontaneous reaction) and write the combined reaction. (Similar to equations 1-3 in the background reading, but for our system specifically). Use your balanced reactions to answer the questions.

Solution Steps

First, we need to identify the half-reactions for the copper and zinc electrodes.

For copper: \[ \text{Reduction:} \quad \mathrm{Cu}^{2+} + 2e^- \rightarrow \mathrm{Cu} \]

For zinc: \[ \text{Oxidation:} \quad \mathrm{Zn} \rightarrow \mathrm{Zn}^{2+} + 2e^- \]

Next, we combine the two half-reactions to form the overall balanced redox reaction. The electrons lost in the oxidation half-reaction must equal the electrons gained in the reduction half-reaction.

\[ \mathrm{Cu}^{2+} + 2e^- \rightarrow \mathrm{Cu} \quad \text{(Reduction)} \] \[ \mathrm{Zn} \rightarrow \mathrm{Zn}^{2+} + 2e^- \quad \text{(Oxidation)} \]

Adding these two half-reactions together, we get the overall reaction:

\[ \mathrm{Cu}^{2+} + \mathrm{Zn} \rightarrow \mathrm{Cu} + \mathrm{Zn}^{2+} \]

Final Answer