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Oxidation is de-electronation whereas reduction is electronation. Oxidants are the substances which oxidise others and reduced themselves. On the other hand reductants are the substances which reduce others and oxidised themselves. The oxidation number of an element in a compound decides its nature to act as oxidant or reductant. Oxidation-reduction occur simultaneously and the overal chemical change is called redox reaction. Redox reactions are of three types : (i) Intermolecular erdox reactions, (ii) Auto-redox or disproportionation reaction, and (iii) Intramolecular redox reactions. In which of the following `H_(2)O_(2)` acts as reductant ? (I) `H_(2)O_(2) + O_(3) rarr H_(2)O+2O_(2)` (II) `PbO_(2) + H_(2)O_(2) rarr PbO+H_(2)O + O_(2)` (III) `HCHO + H_(2)O_(2) rarr HCOOH + H_(2)O` (IV) `Cl_(2) + H_(2)O_(2) rarr 2HCl + O_(2)`A. I, II, IVB. I,II,IIIC. I,IVD. II,III |
Answer» Correct Answer - A Oxidation number of `O` in `H_(2)O_(2)(-1)` increases to zero. |
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