Chemistry · Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number and balancing of redox reactions
In the reaction, the acts as:
In the reaction, \( A g_{2} O+H_{2} O_{2} \rightarrow \) \( 2 A g+H_{2} O+O_{2}, \) the \( H_{2} O_{2} \) acts as:
- A. oxidising agent
- B. bleaching agent
- C. acid
- D. reducing agent
Step-by-step solution
In the reaction, Ag2O contains Ag+ which is reduced to Ag (oxidation state +1 to 0). H2O2 has oxygen at -1 oxidation state, which is oxidized to O2 (0 oxidation state). Since H2O2 loses electrons (is oxidized), it acts as a reducing agent, reducing Ag+ to Ag.
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