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?

Asked by Pragya Singh | 1 year ago |  63

##### Solution :-

In sulphur dioxide$$(SO_{ 2 })$$ the oxidation no. of S is +4 and the range of oxidation no. of sulphur is from +6 to -2.

Hence, $$SO_{ 2 }$$​ can act as a reducing and oxidising agent.

$$H_{ 2 }O_{ 2 }$$

In hydrogen peroxide $$H_{ 2 }O_{ 2 }$$ the oxidation no. of O is -1 and the range of the oxidation no. of oxygen is from 0 to -2. Oxygen can sometimes attain the oxidation no. +1 and +2.

Therefore, $$H_{ 2 }O_{ 2 }$$ can act as a reducing and oxidising agent.

In ozone $$(O_{ 3 })$$ the oxidation no. of O is 0 and the range of the oxidation no. of oxygen is from 0 to –2. Hence, the oxidation no. of oxygen only decreases in this case.

Therefore,$$O_{ 3 }$$​ acts only as an oxidant.

In nitric acid $$HNO_{ 3 }$$the oxidation no. of nitrogen is +5 and the range of the oxidation no. that nitrogen can have is from +5 to -3. Hence, the oxidation no. of nitrogen can only decrease in this case.

Therefore, $$HNO_{ 3 }$$​ acts only as an oxidant.

Answered by Abhisek | 1 year ago

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