The oxidation states of the most electronegative element in the products of the reaction of bao 2 with dilute h 2so 4 .
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The products of the reaction are hydrogen peroxide (H2O2) and insoluble barium sulphate (BaSO4).
BaO2 + H2SO4 = BaSO4 + H2O2
The most electronegative element here is oxygen.
The oxidation state of oxygen in H2O2 is -1, and it is -2 in BaSO4.
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The products of the reaction are hydrogen peroxide (H2O2) and insoluble barium sulphate (BaSO4).
BaO2 + H2SO4 = BaSO4 + H2O2
The most electronegative element here is oxygen.
The oxidation state of oxygen in H2O2 is -1, and it is -2 in BaSO4.
The most common oxidation state of oxygen in compound formation is -2. But in peroxides (H2O2, BaO2, Na2O2 etc) its oxidation state is -1.
It may be noted here that the given reaction is not a redox reaction as it does not result in change in the oxidation number of any element. It is a double decomposition reaction.
BaO2 + H2SO4 = BaSO4 + H2O2
The most electronegative element here is oxygen.
The oxidation state of oxygen in H2O2 is -1, and it is -2 in BaSO4.
The most common oxidation state of oxygen in compound formation is -2. But in peroxides (H2O2, BaO2, Na2O2 etc) its oxidation state is -1.
It may be noted here that the given reaction is not a redox reaction as it does not result in change in the oxidation number of any element. It is a double decomposition reaction.
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