Question

Chlorine undergoes disproportionation in alkaline medium as shown below:
\(a \, \text{Cl}_2(g) + b \, \text{OH}^-(\text{aq}) \rightarrow c \, \text{ClO}^-(\text{aq}) + d \, \text{Cl}^-(\text{aq}) + e \, \text{H}_2\text{O}(\text{l})\)
The values of \( a \), \( b \), \( c \), and \( d \) in a balanced redox reaction are respectively:

• A. 1, 2, 1, and 1
• B. 2, 2, 1, and 3
• C. 2, 2, 1, and 3
• D. 2, 2, 1, and 3

Answer 1

The Correct Option is A

The disproportionation reaction of chlorine in alkaline medium can be balanced as follows. Chlorine (Cl₂) is both reduced and oxidized:

Cl₂ + 2OH⁻ → Cl⁻ + ClO⁻ + H₂O

Thus, the values of a, b, c, and d are 1, 2, 1, and 1 respectively.

So, the correct answer is: Option (1)