Which among the following are auto redox reactions?

P_{4} + O H^{-} \to H_{2} P O_{4}^{-} + P H_{3}

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S_{2} O_{3}^{2 -} \to S O_{4}^{2 -} + S

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H_{2} O_{2} \to H_{2} O + O_{2}

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A g C l + N H_{3} \to [A g (N H_{3})_{2}] C l

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Solution

The correct options are
A $P_{4} + O H^{-} \to H_{2} P O_{4}^{-} + P H_{3}$
B $S_{2} O_{3}^{2 -} \to S O_{4}^{2 -} + S$
D $H_{2} O_{2} \to H_{2} O + O_{2}$
Auto redox reaction is the reaction in which same substance itself undergoes both oxidation as well reduction.
1. $P$ is oxidised from 0 to +5 and reduced from 0 to -3 so this is an auto redox reaction.
2. $S$ is oxidised from +2 to +6 and reduced from +2 to 0 so this is an auto redox reaction.
3. $O$ is oxidised from -1 to 0 and reduced from -1 to -2 so this is an auto redox reaction.
4.Oxidation state of $A g$ does not change during reaction so this is not auto redox reaction.

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Similar questions

H_{2} P O_{4}^{-}

H_{2} P O_{4} + H_{2} O \to H_{3} O^{+} + H_{2} P O_{4}^{-}

H_{2} P O_{4}^{-} + H_{2} O \to H P O_{4}^{2 -} + H_{3} O^{+}

H_{2} P O_{4}^{-} + O H^{-} \to H_{3} P O_{4} + O^{2 -}

H_{2} P O_{4}^{-}

P_{4} + O H^{-} + H_{2} O \to H_{2} P O_{2}^{-} + P H_{3}

H_{2} P O_{4}^{-}

H_{3} P O_{4} + H_{2} O \to H_{3} O^{+} + H_{2} P O_{4}^{-}

H_{2} P O_{4}^{-} + H_{2} O \to H P O_{4}^{2 -} + H_{3} O^{+}

H_{2} P O_{4}^{-} + O H^{-} \to H_{3} P O_{4} + O^{2 -}

H_{2} P O_{4}^{-}

P_{4} + O H^{-} + H_{2} O \to H_{2} P O_{2} + P H_{3}

B + N a O H \to 2 N a_{3} B O_{3} + H_{2}

P_{4} + N a O H + H_{2} O \to N a H_{2} P O_{2} + P H_{3}

S + N a O H \to N a_{2} S_{2} O_{3} + N a_{2} S + H_{2} O

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