Reactions which involve disproportionation of the oxides of nitrogen :

2 N O_{2} + H_{2} O ⟶ H N O_{3} + H N O_{2}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

N_{2} O_{4} ⟶ N O^{+} + N O_{3}^{-}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

3 H N O_{2} ⟶ H N O_{3} + 2 N O + H_{2} O

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

3 N O ⟶ N_{2} O + N O_{2}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct options are
A $2 N O_{2} + H_{2} O ⟶ H N O_{3} + H N O_{2}$
B $N_{2} O_{4} ⟶ N O^{+} + N O_{3}^{-}$
C $3 H N O_{2} ⟶ H N O_{3} + 2 N O + H_{2} O$
D $3 N O ⟶ N_{2} O + N O_{2}$
Disproportionation is a specific type of redox reaction in which a species is simultaneously reduced and oxidised to form two different products.
In their chemical activity, the nitrogen oxides undergo extensive oxidation-reduction reactions.
Reaction:
(a) $2 N O_{2} + H_{2} O ⟶ H N O_{3} + H N O_{2}$
(b) $N_{2} O_{4} ⟶ N O^{+} + N O_{3}^{-}$
(c) $3 H N O_{2} ⟶ H N O_{3} + 2 N O + H_{2} O$
(d) $3 N O ⟶ N_{2} O + N O_{2}$

Suggest Corrections

Similar questions

H N O_{2} t o H N O_{3}

3 H N O_{2} \to H N O_{3} + 2 N O + H_{2} O

N H_{3} + O_{2} \to N O + H_{2} O

N O + O_{2} \to N O_{2}

N O_{2} + H_{2} O \to H N O_{3} + H N O_{2}

N H O_{2} \to H N O_{3} + N O + H_{2} O

3 H N O_{2} ⟶ 2 N O + H N O_{3} + H_{2} O

Balance this equation ( I )No2+H2O=HNo2+HNO3

H g {(N O_{3})}_{2} Δ - \to W + X + O_{2}

X + H_{2} O ⟶ H N O_{2} + H N O_{3}

W + H N O_{3} ⟶ Y + N O + H_{2} O

Y + N a_{2} S_{2} O_{3} (e x c e s s) ⟶ Z + N a N O_{3}

W

X

Y

Z

Join BYJU'S Learning Program