Which of the following equations depict the oxidising nature of H2O2?
(i) 2MnO4- + 6H+ + 5H2O2 → 2Mn2+ + 8H2O + 5O2
(ii) 2Fe3+ + 2H+ + H2O2 → 2Fe2+ + 2H2O + O2
(iii) 2I- + 2H+ + H2O2 → I2+ 2H2O
(iv) KIO4 + H2O2→ KIO3 + H2O + O2
Which of the following equations depict the oxidising nature of H2O2?
(i) 2MnO4- + 6H+ + 5H2O2 → 2Mn2+ + 8H2O + 5O2
(ii) 2Fe3+ + 2H+ + H2O2 → 2Fe2+ + 2H2O + O2
(iii) 2I- + 2H+ + H2O2 → I2+ 2H2O
(iv) KIO4 + H2O2→ KIO3 + H2O + O2
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1 Answer
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This is a multiple choice answer as classified in NCERT Exemplar
Option (iii)
2I- + 2H+ + H2O2 → I2+ 2H2O
As the oxidation state of iodine changes from -1 to 0, this shows peroxide is oxidising in nature.
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H2S has minimum boiling point.
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Volume strength of H2O2 = Molarity * 11.2
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Compound Melting Point (K)
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