Which of the following displaces `Br_(2)` from an aqueous solution containing bromide ions ?

Options

A. `I_(2)`
B. `I_(3)^-`
C. `Cl_(2)`
D. `Cl^(-)`

Answer

To determine which of the following elements displaces \( \text{Br}_2 \) from an aqueous solution containing bromide ions, we need to consider the reactivity of halogens. The halogens are arranged in the periodic table in such a way that their reactivity decreases down the group.

### Step-by-Step Solution:

1. **Identify the Halogens**: The halogens include fluorine (F), chlorine (Cl), bromine (Br), and iodine (I).

2. **Understand Reactivity**: The reactivity of halogens decreases as you move down the group. Therefore, chlorine is more reactive than bromine, and bromine is more reactive than iodine.

3. **Consider the Reaction**: When a more reactive halogen is introduced into a solution containing a less reactive halogen's ions, it can displace the less reactive halogen.

4. **Apply the Concept**: Since we are looking for a substance that can displace \( \text{Br}_2 \) from bromide ions (\( \text{Br}^- \)), we need to find a halogen that is more reactive than bromine.

5. **Conclusion**: Chlorine (Cl) is more reactive than bromine (Br). Therefore, chlorine can displace bromine from an aqueous solution containing bromide ions. The reaction can be represented as:
\[ \text{Cl}_2 + 2 \text{Br}^- \rightarrow 2 \text{Cl}^- + \text{Br}_2 \]

### Final Answer:
Chlorine (Cl) displaces \( \text{Br}_2 \) from an aqueous solution containing bromide ions.

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