Question

Given the partial equation: H2O2 + ClO2 → O2 + ClO2−, balance the reaction in basic solution using the half-reaction method and fill in the coefficients. The missing blanks represent H2O, H+, or OH-, as required to balance the reaction. Enter the coefficients as integers, using the lowest whole numbers. If the coefficient for something is "1", make sure to type that in and not leave it blank. Enter only the coefficients. H2O2 + ClO2 + _____ → O2 + ClO2− + _____

Answer 1

Answer : The balanced chemical equation in basic medium will be,

`H_2O_2+2ClO_2+2OH^-\rightarrow O_2+2ClO_2^-+2H_2O`

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,

`H_2O_2+ClO_2\rightarrow O_2+ClO_2^-`

The oxidation-reduction half reaction will be :

Oxidation :
`H_2O_2\rightarrow O_2`

Reduction :
`ClO_2\rightarrow ClO_2^-`

Now balance the hydrogen atom.

Oxidation :
`H_2O_2\rightarrow O_2+2H^+`

Reduction :
`ClO_2\rightarrow ClO_2^-`

To neutralizing the hydrogen ion by adding hydroxide ion on both side.

Oxidation :
`H_2O_2+2OH^-\rightarrow O_2+2H^+2OH^-`

Reduction :
`ClO_2\rightarrow ClO_2^-`

Hydrogen ion hydroxide ion combine to form water.

Oxidation :
`H_2O_2+2OH^-\rightarrow O_2+2H_2O`

Reduction :
`ClO_2\rightarrow ClO_2^-`

Now balance the charge.

Oxidation :
`H_2O_2+2OH^-\rightarrow O_2+2H_2O+2e^-`

Reduction :
`ClO_2+e^-\rightarrow ClO_2^-`

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 :
`H_2O_2+2OH^-\rightarrow O_2+2H_2O+2e^-`

Reduction :
`2ClO_2+2e^-\rightarrow 2ClO_2^-`

The balanced chemical equation in basic medium will be,

`H_2O_2+2ClO_2+2OH^-\rightarrow O_2+2ClO_2^-+2H_2O`