In the following reaction, which species acts as an oxidising agent?
$F e^{2 +} + 2 H^{+} + N O_{3}^{-} \to F e^{3 +} + N O_{2} + H_{2} O$

F e^{2 +}

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F e^{3 +}

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N O_{3}^{-}

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N O_{2}

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Solution

The correct option is C $N O_{3}^{-}$
The species that gets reduced itself is the oxidising agent.
The oxidation number of nitrogen changes from +5 to +4 which clearly indicates that it is being reduced.
Also, $F e^{2 +}$ is oxidised to $F e^{3 +}$ by the nitrate ion, hence, $(N O_{3}^{-})$ acts as an oxidising agent.

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Similar questions

N O_{3}^{-} + F e^{2 +} + H^{+} \to N O + F e^{3 +} + H_{2} O

Which of the following species are ions?

${C l}^{-}$ , ${F e}^{3 +}$ , ${N O}_{3}^{-}$ , ${F e C l}_{2}$ , ${O H}^{-}$ , ${S O}_{4}^{2 -}$ , $H_{2} O$ , $C_{12} H_{22} O_{11}$

E^{o}

{[F e {(C N)}_{6}]}^{4 -} ⟶ {[F e {(C N)}_{6}]}^{3 +} + e^{-}, E^{o} = - 0.35 V

{F e}^{2 +} \to {F e}^{3 +} + e^{- 1}

{F e}^{2 +} \to {F e}^{3 +} + e^{- 1}; E^{o} = - 0.77 V

F e O_{4}^{2 -}, {F e}^{3 +}, {F e}^{2 +}

F e

F e

F e^{2 +}

F e^{3 +}

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