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)
In this reaction, both two reactants contain nitrogen with a different oxidation number and produce only one product which contains nitrogen with a unique oxidation state. So, nitrogen is oxidized and reduced in the same reaction.
Nitrogen Undergoes a change in oxidation state from 4+ in NO2 to 0 in N2. It is reduced because it gains electrons (decrease its oxidation state). NO2 is the oxidizing agent (electron acceptor).
Nitrogen Changes from an oxidation state of 3- in NH3 to 0 in N2. It is oxidized because it loses electrons (increase its oxidation state). NH3 is the reducing agent (electron donor)
(ii) Zn(s) +AgNO3(aq) => Zn(NO3)2(aq) + Ag(s)
Ag changes oxidation state from 1+ to 0 in Ag(s).
Ag is reduced because it gains electrons and for this reason and AgNO3 is the oxidizing agent (electron acceptor)
Zn Changes from an oxidation state of 0 in Zn(s) to 2+ in Zn(NO3)2. It is oxidized and for this reason Zn is the reducing agent (electron donor).
Balanced equation:
Zn(s) +2AgNO3(aq) => Zn(NO3)2(aq) + 2Ag(s)
In reaction (i) NO2 is the oxidizing agent while NH3 is the reducing agent. In reaction (ii) AgNO3 is the oxidizing agent while Zn is the reducing agent.
First of all, the reaction equations must be balanced as follows;
(i) 8NH3( g) + 6NO2( g) => 7N2( g) + 12H2O(l)
Also;
(ii) Zn(s) + 2AgNO3(aq) => Zn(NO3)2(aq) + 2Ag(s)
Secondly, we need to find which specie was reduced and which specie was oxidized in the reaction. In the first reaction (i) nitrogen (IV) was reduced while NH3 was oxidized. In the second reaction (ii) AgNO3 was reduced while Zn was oxidized.
Since the oxidizing agent is reduced in a reaction and the reducing agent is oxidized in a reaction, it follows that;
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