Oxidation and reduction always occur sim...

Oxidation and reduction always occur simultaneously. These reactions which involve simultaneous oxidation and reduction are called redox reactions. Therefore, every redox reaction is made up of two half reactions. One half reaction represents oxidation and other half reaction represents the reduction. Oxidation and reduction of an atom, molecule or ion can also be defined in terms of electrons. The substance that gains electrons, is reduced to a lower oxidation state and acts as an oxidising agent. Similarly, the substance which loses electrons is oxidised to a higher oxidation state, and is called a reducing agent.
In which of the following reactions hydrogen peroxide is acting as a reducing agent?

`2FeCl_(2)+2HCl+H_(2)O_(2)to2FeCl_(3)+2H_(2)O`

`Cl_(2)+H_(2)O_(2)to2HCl+O_(2)`

`2HI+H_(2)O_(2)to2H_(2)O+I_(2)`

`H_(2)SO_(3)+H_(2)O_(2)toH_(2)SO_(4)+H_(2)O`

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The correct Answer is:

`H_(2)O_(2)` is oxidised to `O_(2)`, hence acts as a reducing agent.

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Oxidation and reduction always occur simultaneously. These reactions which involve simultaneous oxidation and reduction are called redox reactions. Therefore, every redox reaction is made up of two half reactions. One half reaction represents oxidation and other half reaction represents the reduction. Oxidation and reduction of an atom, molecule or ion can also be defined in terms of electrons. The substance that gains electrons, is reduced to a lower oxidation state and acts as an oxidising agent. Similarly, the substance which loses electrons is oxidised to a higher oxidation state, and is called a reducing agent. The reaction : H_(2)S+H_(2)O_(2)toS+2H_(2)O indicates

oxidising action of `H_(2)O_(2)`

reducing nature of `H_(2)O_(2)`

acidic nature of `H_(2)O_(2)`

alkaline nature of `H_(2)O_(2)`.

oxidation by 3 electrons

reduction by 5 electrons

oxidation by 5 electrons

reduction by 3 electrons

`CrO_(4)^(2-) rarr Cr_2O_(7)^(2-)`

`Cr rarr CrCl_3`

`Na rarr Na^(+)`

`2S_2O_(3)^(2-) rarr S_4O_(6)^(2-)`