Answer:
(i) Oxidizing Agent: NO2 / Reducing Agent: NH3-
(ii) Oxidizing Agent: AgNO3 / Reducing Agent: Zn
Explanation:
(i) 8NH3( g) + 6NO2( g) => 7N2( g) + 12H2O( l)
Both reactants contain nitrogen with differing oxidation states, yielding a product with a unique oxidation state of nitrogen. Thus, nitrogen experiences both oxidation and reduction in this reaction.
Nitrogen changes its oxidation state from 4+ in NO2 to 0 in N2, indicating reduction as it gains electrons. NO2 acts as the oxidizing agent (electron acceptor).
Nitrogen alters from an oxidation state of 3- in NH3 to 0 in N2, showing oxidation as it loses electrons. NH3 serves as the reducing agent (electron donor).
(ii) Zn(s) +AgNO3(aq) => Zn(NO3)2(aq) + Ag(s)
Ag shows a change in oxidation state from 1+ to 0 in Ag(s).
Ag undergoes reduction since it gains electrons, and for this reason AgNO3 is recognized as the oxidizing agent (electron acceptor).
Zn transforms from an oxidation state of 0 in Zn(s) to 2+ in Zn(NO3)2. It is oxidized, rendering Zn as the reducing agent (electron donor).
Balanced equation:
Zn(s) +2AgNO3(aq) => Zn(NO3)2(aq) + 2Ag(s)
