Match the reactions of metals with dilute $H N O_{3} (i n L i s t I)$ with the nitrogen compounds obtained by oxidation/reduction $(i n L i s t I I)$ .

Open in App

Solution

A. Nitric acid being strong oxidizing agent, oxidises 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 very dilute $H N O_{3}, H_{2}$ gas is evolved. Mg and Mn are highly reactive metals, they are able to displace hydrogen from the nitric acid.
$M g + H N O_{3} ⟶ M g {(N O_{3})}_{2} + H_{2}$
B. 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 react 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. $3 P b + {8 H N O_{3}}_{(d i l .)} ⟶ 3 P b {(N O_{3})}_{2} + 4 H_{2} O + 2 N O$

Suggest Corrections

Similar questions

H N O_{3}

H N O_{3}

(i n L i s t I)

(i n L i s t I I)

Join BYJU'S Learning Program