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

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 Link

ajeigbeibraheem ajeigbeibraheem · Answer 2 · 2021-12-06T13:45:32+01:00

The oxidizing agent in the reaction is [tex]\mathbf{NO_{3(aq)}^-}[/tex].

An oxidizing agent is a substance that causes reduction when it removes an electron from another reactant species in a chemical equation.

On the other hand, a reducing agent is a substance that causes oxidation when it accepts an electron from another reacting species in a chemical equation.

From the given chemical equation:

[tex]\mathbf{8H^+_{(aq)} + 6cl^{-}_{(aq)} + Sn _{(s)} + 4 NO_3^-_{(aq)} \to SnCl_6^{2-}_{(aq)} + 4NO_{2(g)} + 4H_2O_{(l)}}[/tex]

The oxidizing agent is = [tex]\mathbf{NO_{3(aq)}^-}[/tex]. This is because Sn is oxidized from 0 to +4.

Learn more about oxidation and reduction here:

https://brainly.com/question/13699873?referrer=searchResults