Question

Observe the following reactions (not balanced) \text{Cl}_2 + \text{NaOH} \rightarrow \text{NaCl} + X + \text{H}_2\text{O}
\text{Cl}_2 + \text{NaOH} \rightarrow \text{NaCl} + Y + \text{H}_2\text{O}

• A. \( -1, \, +1 \)
• B. \( +5, \, +1 \)
• C. \( +1, \, -1 \)
• D. \( +1, \, +5 \) \

Hint:

In reactions involving chlorine, keep track of oxidation and reduction by comparing the changes in oxidation states of chlorine in different compounds.

Answer 1

The Correct Option is B

The reactions are as follows: \[ \text{Cl}_2 + \text{NaOH (aq)} \rightarrow \text{NaCl} + X + \text{H}_2\text{O} \quad \text{(reaction 1)} \] \[ \text{Cl}_2 + \text{NaOH (aq)} \rightarrow \text{NaCl} + Y + \text{H}_2\text{O} \quad \text{(reaction 2)} \] In reaction 1, chlorine undergoes a reduction to form chloride ion (\( \text{NaCl} \)), and X has an oxidation state of +1. In reaction 2, chlorine undergoes oxidation to form a species Y, where chlorine has an oxidation state of +5. Thus, the oxidation states of chlorine in X and Y are \( +1 \) and \( +5 \) respectively.