Consider the Galvanic cell ` Zn^- |ZnSO_4 ||CuSO_4 +Cu^(o+)` the reaction at cathode is .

Options

A. `Cu^(2+) +2e rarr Cu`
B. `Zn^(2+) +2e^(-) rarr Zn`
C. ` Cu^(2+) +2e^(-) + 2e^(-) rarr Cu + Zn^(2+) `
D. ` Zn^(2+) + Cu rarr +Cu^(2+)`

Explanation

To determine the reaction at the cathode in the given galvanic cell setup, we will follow these steps:

### Step-by-Step Solution:

1. **Identify the Components of the Galvanic Cell**:
- The galvanic cell consists of a zinc electrode (Zn) and a copper electrode (Cu) with their respective sulfate solutions (ZnSO4 and CuSO4).
- The anode is where oxidation occurs (Zn), and the cathode is where reduction occurs (Cu).

2. **Determine the Oxidation and Reduction Reactions**:
- At the anode (Zn electrode), zinc will oxidize:
\[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^{-} \]
- At the cathode (Cu electrode), copper ions from the CuSO4 solution will be reduced:
\[ \text{Cu}^{2+} + 2e^{-} \rightarrow \text{Cu} \]

3. **Write the Overall Reaction**:
- The overall cell reaction can be written by combining the oxidation and reduction half-reactions:
\[ \text{Zn} + \text{Cu}^{2+} \rightarrow \text{Zn}^{2+} + \text{Cu} \]

4. **Identify the Reaction at the Cathode**:
- The specific reaction occurring at the cathode is:
\[ \text{Cu}^{2+} + 2e^{-} \rightarrow \text{Cu} \]

5. **Final Answer**:
- Therefore, the reaction at the cathode is:
\[ \text{Cu}^{2+} + 2e^{-} \rightarrow \text{Cu} \]