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

Answer: (A)

1, 2, 1, and 1

Answer 2

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)