Respuesta :
Answer : The balanced chemical equation in basic medium will be,
[tex]H_2O_2+2ClO_2+2OH^-\rightarrow O_2+2ClO_2^-+2H_2O[/tex]
Explanation :
Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.
Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.
Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.
The given chemical reaction is,
[tex]H_2O_2+ClO_2\rightarrow O_2+ClO_2^-[/tex]
The oxidation-reduction half reaction will be :
Oxidation : [tex]H_2O_2\rightarrow O_2[/tex]
Reduction : [tex]ClO_2\rightarrow ClO_2^-[/tex]
Now balance the hydrogen atom.
Oxidation : [tex]H_2O_2\rightarrow O_2+2H^+[/tex]
Reduction : [tex]ClO_2\rightarrow ClO_2^-[/tex]
To neutralizing the hydrogen ion by adding hydroxide ion on both side.
Oxidation : [tex]H_2O_2+2OH^-\rightarrow O_2+2H^+2OH^-[/tex]
Reduction : [tex]ClO_2\rightarrow ClO_2^-[/tex]
Hydrogen ion hydroxide ion combine to form water.
Oxidation : [tex]H_2O_2+2OH^-\rightarrow O_2+2H_2O[/tex]
Reduction : [tex]ClO_2\rightarrow ClO_2^-[/tex]
Now balance the charge.
Oxidation : [tex]H_2O_2+2OH^-\rightarrow O_2+2H_2O+2e^-[/tex]
Reduction : [tex]ClO_2+e^-\rightarrow ClO_2^-[/tex]
The charges are not balance on both side of the reaction. We are multiplying reduction reaction by 2 and then added both equation, we get the balanced redox reaction.
Oxidation : [tex]H_2O_2+2OH^-\rightarrow O_2+2H_2O+2e^-[/tex]
Reduction : [tex]2ClO_2+2e^-\rightarrow 2ClO_2^-[/tex]
The balanced chemical equation in basic medium will be,
[tex]H_2O_2+2ClO_2+2OH^-\rightarrow O_2+2ClO_2^-+2H_2O[/tex]
