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Consider the reactions
(A) H202 + 2HI → I2 + 2H20
(B) HOCl + H2O2 → H30+ + Clâ?? + 02
Which of the following statements is correct about H202 with reference to these reactions? Hydrogen peroxide is   _______      

(a) an oxidizing agent in both (A) and (B)
(b) an oxidizing agent in (A) and reducing agent in (B)
(c) a reducing agent in (A) and oxidizing agent in (B)
(d) a reducing agent in both (A) and (B)#new_quesion#The oxide that gives H202 on treatment with dilute H2S04 is
(a) Pb02
(b) Ba02 -8H20
(c) Mn02
(d) Ti02

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I have 18 Years Experience in teaching ( Chemistry NEET,IIT Mains, IIT Foundation)

1) Answer is b i,e is an oxidising agent in(A) and reducing agent in (B).Sinse in A Iodide is oxidised as Iodine(Oxidation number is increases i,e is -1 to 0),in B Chlorine is reduced to Chloride Ion(Oxidation number is decreases i,e +1 to -1) 2) answer is b i,e is BaO2 8H2o. Because BaO2 contains peroxide...
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1) Answer is b i,e is an oxidising agent in(A) and reducing agent in (B).Sinse in A Iodide is oxidised as Iodine(Oxidation number is increases i,e is -1 to 0),in B Chlorine is reduced to Chloride Ion(Oxidation number is decreases i,e +1 to -1)

2) answer is b i,e is BaO2 8H2o. Because BaO2 contains peroxide linkage.

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In question one First reaction H2O2 will act as oxidizing agent because HI is undergoing oxidation so h2o2 will act as oxidizing agent But in second case in this reaction H2o2 will be showing disproportionation reaction because it is undergoing oxidation as well reduction at a same time Option a is...
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In question one 

First reaction H2O2 will act as oxidizing agent because HI is undergoing oxidation so h2o2 will act as oxidizing agent 

But in second case in this reaction

H2o2 will be showing disproportionation reaction because it is undergoing oxidation as well reduction at a same time 

Option a is correct

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Comments

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