Chemistry · Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number and balancing of redox reactions
In the following redox reaction: +\boldsymbol{N} \boldsymbol{O}_{\boldsymbol{3}}
In the following redox reaction: \( \boldsymbol{Z} \boldsymbol{n}(\boldsymbol{s})+\boldsymbol{N} \boldsymbol{O}_{\boldsymbol{3}}^{-}(\boldsymbol{a} \boldsymbol{q})+\boldsymbol{H}^{+}(\boldsymbol{a} \boldsymbol{q}) \longrightarrow \) \( Z n^{2+}(a q)+N H_{4}^{+}(a q) \) \( Z n(s) \) and \( N O_{3}^{-}(a q) \) respectively are respectively:
- A. oxidant and reductant
- B. reductant and oxidant
- C. both oxidant
- D. both reductant
Step-by-step solution
Zn(s) has oxidation state 0 and changes to +2 in Zn2+, losing electrons, so it acts as a reductant. N in NO3- has oxidation state +5 and changes to -3 in NH4+, gaining electrons, so NO3- acts as an oxidant.
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