Assertion -Following reaction is a disproportionation reaction- Br2-2OH- - BrO- -Br- - 2H2O Reason- Br2 is oxidized to BrO- as well as reduced to Br-

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Standard XII

Chemistry

Addition of Sulphuric Acid and Water

Assertion :Fo...

Question

Assertion :Following reaction is a disproportionation reaction:
$B r_{2} + 2 O H^{-} \to B r O^{-} + B r^{-} + 2 H_{2} O$ Reason: $B r_{2}$ is oxidized to $B r O^{-}$ as well as reduced to $B r^{-}$ .

Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

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Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion

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Assertion is correct but Reason is incorrect

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Both Assertion and Reason are incorrect

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Solution

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
In this reaction, bromine is oxidized to form $B r O^{-}$ . At the same time, bromine is reduced to $B r^{-}$ ion.
Hence, the reaction is known as disproportionation reaction.
Thus, both assertion and reason are correct and reason is the correct explanation for assertion.

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Assertion :Following reaction is a disproportionation reaction:Br2+2OH−→BrO−+Br−+2H2O Reason: Br2 is oxidized to BrO− as well as reduced to Br−.

Assertion :Following reaction is a disproportionation reaction:
$B r_{2} + 2 O H^{-} \to B r O^{-} + B r^{-} + 2 H_{2} O$ Reason: $B r_{2}$ is oxidized to $B r O^{-}$ as well as reduced to $B r^{-}$ .