Determine the oxidizing and reducing agent in the reaction below. ClO2- -> ClO2 + Cl-

Question

 Chemistry

Answer 1

ClO₂^- -> ClO₂ + Cl^- cannot occur.  This is not a reaction that can take place.  Perhaps you meant

2ClO^- ==>Cl^- + ClO₂^-

Cl on the left side of the equation in ClO^- has an oxidation number of +1 (O is -2)

Cl on the right side of the equation in ClO2^- has an oxidation number of +3 (O is -2)

Cl has gone from +1 to +3 meaning it has been oxidized making it the REDUCING AGENT.

Cl on the right side of the equation in Cl- has an oxidation number of -1

Cl has gone from +1 to -1 meaning it has been reduced making it the OXIDIZING AGENT.

Yes, Cl is both the oxidizing and reducing agent.  This is referred to as DISPROPORTIONATION.

 

 

 

If this is supposed to be run in acid, then you would have the following balanced equation: 5ClO2^- + 4H^+ ==> 4ClO2 + Cl^- + 2H2O Disproportionation is still in effect.