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Question

H2O2 cannot oxidise:


A

O3

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B

Kl/HCl

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C

PbS

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D

Na2SO3

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Solution

The correct option is A

O3


The explanation for the correct option:

Option(A): O3

  • Ozone (O3) is a stronger oxidizing agent than Hydrogen peroxide(H2O2).
  • So when Hydrogen peroxide reacts with ozone, the former acts as a reducing agent and reduces ozone to oxygen as follows.

O3(g)(Oxygen)+H2O2(l)(Hydrogenperoxide)H2O(l)(Water)+2O2(g)(Oxygen)

  • Hence, (H2O2) cannot oxidize O3.

The explanation for the incorrect options:

Option(B): Kl/HCl

  • When reacting with Potassium iodide and Hydrochloric acid, KI + HCl 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 below

  • Here Hydrogen peroxide oxidizes iodine of Potassium iodide from -1 state to 0 states in free iodine.

Option(C) PbS

  • When Hydrogen peroxide, H2O2 reacts with Lead sulfide( PbS) to give Lead sulfate (PbSO4 )and water as products.
  • The balanced chemical equation for the reaction between Lead sulfide and Hydrogen peroxide is shown below.

PbS(s)(Leadsulfide)+4H2O2(l)(hydrogenperoxide)PbSO4(s)(leadsulphate)+4H2O(l)(Water)

  • 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): Na2SO3

  • The reaction of Sodium sulfite (Na2SO3 ) with Hydrogen peroxide is given by:

Na2SO3(s)+(Sodiumsulfite)H2O2(l)(Hydrogenperoxide)H2O(l)(Water)+Na2SO4(s)(Sodiumsulfite)

  • Here, Sulfur is oxidized from +4 state to +6 state by Hydrogen peroxide.

Hence, hydrogen peroxide(H2O2) cannot oxidize ozone(O3), option (A) is correct.


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