Chemistry · Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number and balancing of redox reactions
The reaction describes:
The reaction \( \boldsymbol{H}_{2} \boldsymbol{S}+\boldsymbol{H}_{2} \boldsymbol{O}_{2} \rightarrow \boldsymbol{S}+ \) \( 2 H_{2} O \) describes:
- A. acidic nature of \( H_{2} O_{2} \)
- B. alkaline nature of \( H_{2} O_{2} \)
- C. oxidizing nature of \( H_{2} O_{2} \)
- D. reducing nature of \( H_{2} O_{2} \)
Step-by-step solution
In the reaction H2S + H2O2 → S + 2H2O, sulfur in H2S is oxidized from oxidation state -2 to 0 (loss of electrons), while oxygen in H2O2 is reduced from -1 to -2 (gain of electrons). Therefore, H2O2 acts as an oxidizing agent, demonstrating its oxidizing nature.
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