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  • While sulphur dioxide and hydrogen peroxide can act as oxidising as well asreducing agents in their reactions,

8.8 While sulphur dioxide and hydrogen peroxide can act as oxidising as well as reducing agents in their reactions, ozone and nitric acid act only as oxidants. Why? 

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  • sulphur dioxide (SO_{2}) here oxidation state of sulphur is +4  and the range of oxidation number of S is from -2 to +6. It means it can accept an electron and lose as well, therefore, it can behave as oxidant and reductant both. 
  • In case of hydrogen peroxide (H_{2}O_{2}) oxidation state is -1 and the oxidation state of O can vary from 0 to -2. So it shows both oxidizing and reducing properties.
  • For HNO_{3} , Nitrogen has +5 oxidation state and it varies from +5 to -3. So it only accepts electrons. The oxidation state of N only decreases. Hence it acts as only oxidants.
  • And in case of O_{3} , the oxidation state of O is zero(0) and the range of oxidation number of O is 0 to -2. It only decreases in this case also so therefore it acts as only oxidants.

 

Posted by

Gautam harsolia

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