The correct option is
A The explanation for the correct option:
Option(A):
- Ozone is a stronger oxidizing agent than Hydrogen peroxide.
- So when Hydrogen peroxide reacts with ozone, the former acts as a reducing agent and reduces ozone to oxygen as follows.
- Hence, cannot oxidize .
The explanation for the incorrect options:
Option(B):
- When reacting with Potassium iodide and Hydrochloric acid, Potassium iodide acts as a reducing agent whereas Hydrogen peroxide acts as an oxidizing agent.
- The balanced chemical equation for this reaction is written as
![stack 2 K I with left parenthesis Potassium space iodide right parenthesis below space plus stack space H subscript 2 O subscript 2 space open parentheses l close parentheses with left parenthesis Hydrogen space peroxide right parenthesis below plus stack space 2 H Cl open parentheses aq close parentheses with left parenthesis Hyfrocholric space acid right parenthesis below rightwards arrow stack I subscript 2 space end subscript with open parentheses Iodine close parentheses below plus stack space 2 K Cl space with left parenthesis Potassium space chloride right parenthesis below plus stack space 2 H subscript 2 O with open parentheses Water close parentheses 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- Here Hydrogen peroxide oxidizes iodine of Potassium iodide from -1 state to 0 states in free iodine.
Option(C)
- When Hydrogen peroxide, reacts with Lead sulfide( ) to give Lead sulfate ( )and water as products.
- The balanced chemical equation for the reaction between Lead sulfide and Hydrogen peroxide is shown below.
- Here Hydrogen peroxide oxidizes Lead sulfide in which sulfur is in a -2 oxidation state to Lead sulfate in which sulfur is in a +6 oxidation state.
Option(D):
- The reaction of Sodium sulfite ( ) with Hydrogen peroxide is given by:
- Here, Sulfur is oxidized from +4 state to +6 state by Hydrogen peroxide.
Hence, hydrogen peroxide cannot oxidize ozone, option (A) is correct.