The reaction `Cu^(2+)(aq)+2Cl^(-)(aq) rarr Cu(s)+Cl_(2)(g)` has `E^(c-)._(cell)=-1.03V`. This reaction

Options

A. Can be made to produce electricity in voltaic cell
B. Can be made to occur in an electrolytic cell
C. Can occur in acidic medium only
D. Can occur in basic medium only.

Explanation

To analyze the given reaction and determine the conditions under which it can occur, we will follow these steps:

### Step 1: Identify the Reaction
The reaction provided is:
\[ \text{Cu}^{2+}(aq) + 2\text{Cl}^-(aq) \rightarrow \text{Cu}(s) + \text{Cl}_2(g) \]

### Step 2: Understand the Cell Potential
The cell potential (\(E^{\circ}_{cell}\)) is given as -1.03 V. A negative cell potential indicates that the reaction is non-spontaneous under standard conditions.

### Step 3: Determine the Type of Cell
Since the reaction is non-spontaneous (as indicated by the negative cell potential), it cannot occur spontaneously in a voltaic (galvanic) cell. Instead, it can be driven by an external source of energy, which is characteristic of an electrolytic cell.

### Step 4: Analyze the Medium
The question also asks whether the reaction can occur in acidic or basic medium. The presence of \(Cu^{2+}\) and \(Cl^-\) ions does not specify a requirement for acidic or basic conditions for the reaction to proceed. Thus, it can occur in either medium, but the electrolytic cell setup will be required to drive the reaction.

### Conclusion
1. The reaction cannot produce electricity in a voltaic cell because it is non-spontaneous.
2. The reaction can occur in an electrolytic cell since it requires an external energy source.
3. The reaction can occur in both acidic and basic media.

### Final Answer
The reaction can be made to occur in an electrolytic cell (Option B).

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