Question

Identify the oxidizing agent in the reaction: 8h+(aq) + 6cl−(aq) + sn(s) + 4no3−(aq) → sncl62−(aq) + 4no2(g) + 4h2o(l)

Answer 1

Balanced chemical reaction:
8H⁺(aq) + 6Cl⁻(aq) + Sn(s) + 4NO₃⁻(aq) → SnCl₆²⁻(aq) + 4NO₂(g) + 4H₂O(l).
Nitrate anion (NO₃⁻) is oxidazing agent, because nitrogen (oxidation number +5) in nitrate gains electrons and became nitrogen dioxide (NO₂), where now nitrogen has oxidation number +4, so nitrogen is reduced.

Answer 2

Answer: The oxidizing agent in the given reaction will be $NO_3^-$ ion.

Explanation:

Oxidizing agent are defined as the species which oxidize the other species and itself gets reduced. It undergoes a reduction reaction. The reduction reaction is defined as the reaction in which a specie gains electrons. The oxidation state of the specie gets reduced.

In the given chemical equation:

$8H^+(aq.)+6Cl^-(aq.)+Sn(s)+4NO^{3-}(aq.)\rightarrow SnCl_6^{2-}(aq.)+4NO_2(g)+ 4H_2O(l)$

Reactant side:

Oxidation state of hydrogen = +1

Oxidation state of oxygen = -2

Oxidation state of Tin = 0

Oxidation state of chlorine = -1

Oxidation state of nitrogen = +5

Product side:

Oxidation state of hydrogen = +1

Oxidation state of oxygen = -2

Oxidation state of Tin = +6

Oxidation state of chlorine = -1

Oxidation state of nitrogen = +4

As, the oxidation state of nitrogen is getting reduced. Hence, it is getting reduced and is considered as an oxidizing agent.