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(1) \(SO{2}\) (P) Oxidizing agent ...

(1) \(SO_{2}\) (P) Oxidizing agent
(2) \(SO_{3}\) (Q) Reducing agent
(3) \(H_{2}O_{2}\) (R) Undergoes disproportionation
(4) NaF (S) Neither an oxidizing nor a reducing agent

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H_2O_2 cannot act as reducing agent.

SO_(2) is more powerful reducing agent in:

STATEMENT-1 H_(2)O_(2) to H_(2)O + (1)/(2)O_(2) . This is an example of disproportionation reaction. STATEMENT-2 H_(2)O_(2) can act as a oxidising as well as reducing agent .