Match the reactions of metals with dilute $H N O_{3}$ (in column-I) with the nitrogen compounds (obtained by oxidation/reduction (in column-II).

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Solution

(A) Nitric acid being strong oxidizing agent, oxidizes the $H_{2}$ produced to water and itself gets reduced to any nitrogen oxide $(N_{2} O, N O, N O_{2})$ .

But when magnesium and manganese react with the very dilute $H N O_{3}, H_{2}$ gas is evolved. $M g$ and $M n$ are highly reactive metals, they are able to displace hydrogen from the nitric acid.

$M g + 2 H N O_{3} ⟶ M g {(N O_{3})}_{2} + H_{2}$

(B) The reaction of nitric acid with zinc involves a complicated set of redox reactions.

$4 Z n + 10 H N O_{3} ⟶ 4 Z n {(N O_{3})}_{2} + N_{2} O + 5 H_{2} O$

(C) Tin reacts with nitric acid to produce tin(II) nitrate, ammonium nitrate, and water.

$4 S n + 10 H N O_{3} ⟶ 4 S n {(N O_{3})}_{2} + N H_{4} N O_{3} + 3 H_{2} O$

(D) $3 P b + {8 H N O_{3}}_{(d i l .)} ⟶ 3 P b {(N O_{3})}_{2} + 4 H_{2} O + 2 N O$

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$\begin{matrix} C o l u m n - I & C o l u m n - I I I & M g + d i l . H N O_{3} & P & N O I I & Z n + d i l . H N O_{3} & Q & H_{2} I I I & C u + d i l . H N O_{3} & R & N_{2} O I V & P b + c o n c . H N O_{3} & S & N O_{2} \end{matrix}$

Q. Match the reactions given in column I with their respective oxidant/reductant given in column II.

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Match the reactions of metals with dilute HNO3 (in column-I) with the nitrogen compounds (obtained by oxidation/reduction (in column-II).

Match the reactions of metals with dilute $H N O_{3}$ (in column-I) with the nitrogen compounds (obtained by oxidation/reduction (in column-II).