Suggest a scheme of classification of the following redox reaction:

$A)$ $N_{2} (g) + O_{2} (g) ⟶ 2 N O (g)$

$B)$ $2 P b (N O_{3})_{2} (s) ⟶ 2 P b O (s) + 4 N O_{2} (g) + O_{2} (g)$

$C)$ $N a H (s) + H_{2} O (l) ⟶ N a O H (a q) + H_{2} (g)$

$D) 2 N O_{2} (g) + 2 O H^{-} (a q) ⟶ N O_{2}^{-} (a q) + N O_{3}^{-} (a q) + H_{2} O (l)$

Open in App

Solution

$A)$ In the given reaction, the compound nitric oxide is formed by the combination of the elemental substances, nitrogen and oxygen. Therefore, this is an example of combination redox reaction

$B)$ The given reaction involves the breaking down of lead nitrate into three components. Therefore, this is categorized under Decomposition redox reaction

$C)$ Hydrogen of water has been displaced by hydride ion into dihydrogen gas. Therefore, this may be called as Displacement redox reaction.

$D)$ This reaction involves disproportion of $N O_{2}$ (+4 state) into $N O_{2}^{-}$ $(+ 3$ state) and $N O_{3}^{-}$ $(+ 5$ state). Therefore, this reaction is an example of disproportion redox reaction.

Suggest Corrections

Similar questions

Why it is more appropriate to write reactions

O_{3} (g) + H_{2} O_{2} (l) \to H_{2} O (l) + 2 O_{2} (g)

as :

O_{3} (g) + H_{2} O_{2} (l) \to H_{2} O (l) + O_{2} (g) + O_{2} (g)

Also suggest a technique to investigate the path of the above redox reaction.

Consider the reactions:

(a) 6 CO₂(g) + 6H₂O(l) → C₆ H₁₂ O₆(aq) + 6O₂(g)

(b) O₃(g) + H₂O₂(l) → H₂O(l) + 2O₂(g)

Why it is more appropriate to write these reactions as:

(a) 6CO₂(g) + 12H₂O(l) → C₆ H₁₂ O₆(aq) + 6H₂O(l) + 6O₂(g)

(b) O₃(g) + H₂O₂ (l) → H₂O(l) + O₂(g) + O₂(g)

Also suggest a technique to investigate the path of the above (a) and (b) redox

reactions.

Consider the reactions:
$6 C O_{2} (g) + 6 H_{2} O (l) \to C_{6} H_{12} O 6 (a q) + 6 O_{2} (g)$
Why it is more appropriate to write these reactions as:
$6 C O_{2} (g) + 12 H_{2} O (l) \to C_{6} H_{12} O_{6} (a q) + 6 H_{2} O (l) + 6 O_{2} (g)$
Also suggest a technique to investigate the path of the above (a) and (b) redox reactions.

$O_{3} (g) + H_{2} O_{2} (l) \to H_{2} O (l) + 2 O_{2} (g)$
Why it is more appropriate to write these reactions as:
$O_{3} (g) + H_{2} O_{2} (l) \to H_{2} O (l) + O_{2} (g) + O_{2} (g)$
Also suggest a technique to investigate the path of the above (a) and (b) redox reactions.

Q. Balance the following equation stepwise.
a. H₂S₂O₇(l) + H₂O(l) → H₂SO₄(l)
b. SO₂(g) + H₂S(aq) → S(s) + H₂O(l)
c. Ag(s) + HCl(aq) → AgCl ↓+ H₂ ↑
d. NaOH(aq) + H₂SO₄(aq) → Na₂SO₄(aq) + H₂O(l)

Q. For which of the following reactions,

Δ H \neq Δ U

Join BYJU'S Learning Program

Explore more

Electrochemical Series

Standard XII Chemistry

Join BYJU'S Learning Program

Suggest a scheme of classification of the following redox reaction: A) N2(g)+O2(g)⟶2NO(g) B) 2Pb(NO3)2(s)⟶2PbO(s)+4NO2(g)+O2(g) C) NaH(s)+H2O(l)⟶NaOH(aq)+H2(g) D) 2NO2(g)+2OH−(aq)⟶NO−2(aq)+NO−3(aq)+H2O(l)