Match List-I with the List-IIList-I
Reaction List-II
Type of redox reaction (A) N2(g) + O2(g) → 2NO(g) (I) Decomposition (B) 2Pb (NO3)2(s)
→ 2PbO(s) + 4NO2(g) + O2(g) (II) Displacement (C) 2Na(s) + 2H2O(l)
→ 2NaOH(aq) + H2(g) (III) Disproportionation (D) 2NO2(g) + 2OH-(aq)
→ NO2-(aq) + NO3-(aq) + H2O(l) (IV) Combination
Choose the correct answer from the options given below:
| List-I Reaction | List-II Type of redox reaction |
|---|---|
| (A) N2(g) + O2(g) → 2NO(g) | (I) Decomposition |
| (B) 2Pb (NO3)2(s) → 2PbO(s) + 4NO2(g) + O2(g) | (II) Displacement |
| (C) 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g) | (III) Disproportionation |
| (D) 2NO2(g) + 2OH-(aq) → NO2-(aq) + NO3-(aq) + H2O(l) | (IV) Combination |
- (A)-(I), (B)-(II), (C)-(III), (D)-(IV)
- (A)-(III), (B)-(II), (C)-(I), (D)-(IV)
- (A)-(II), (B)-(III), (C)-(IV), (D)-(I)
- (A)-(IV), (B)-(I), (C)-(II), (D)-(III)
The Correct Option is D
Approach Solution - 1
To solve the given problem, we need to match each reaction in List-I with the corresponding type of redox reaction mentioned in List-II.
Step-by-step Explanation:
- (A) N2(g) + O2(g) → 2NO(g)
This is a Combination Reaction. In this reaction, nitrogen (N2) and oxygen (O2) combine to form nitrogen monoxide (NO). This type of reaction involves the combination of two or more substances to form a single product. - (B) 2Pb(NO3)2(s) → 2PbO(s) + 4NO2(g) + O2(g)
This is a Decomposition Reaction. In this reaction, lead nitrate decomposes to form lead oxide, nitrogen dioxide, and oxygen gas. A decomposition reaction involves breaking down a compound into two or more components. - (C) 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
This is a Displacement Reaction. In displacement reactions, one element displaces another in a compound. Here, sodium displaces hydrogen from water to form sodium hydroxide and hydrogen gas. - (D) 2NO2(g) + 2OH-(aq) → NO2-(aq) + NO3-(aq) + H2O(l)
This is a Disproportionation Reaction. Disproportionation reactions involve the same element being simultaneously oxidized and reduced. In the given reaction, nitrogen dioxide is both oxidized to nitrate (NO3-) and reduced to nitrite (NO2-).
Matching the reactions with the type:
| List-I Reaction | List-II Type of Redox Reaction |
|---|---|
| (A) N2(g) + O2(g) → 2NO(g) | (IV) Combination |
| (B) 2Pb(NO3)2(s) → 2PbO(s) + 4NO2(g) + O2(g) | (I) Decomposition |
| (C) 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g) | (II) Displacement |
| (D) 2NO2(g) + 2OH-(aq) → NO2-(aq) + NO3-(aq) + H2O(l) | (III) Disproportionation |
Therefore, the correct answer is (A)-(IV), (B)-(I), (C)-(II), (D)-(III).
Approach Solution -2
\(\textbf{(A) $N_2(g) + O_2(g) \rightarrow 2NO(g)$:}\) This reaction is a combination reaction because two reactants combine to form a single product. Thus, $A \rightarrow (IV)$.
\(\textbf{(B) $2Pb(NO_3)_2(s) \rightarrow 2PbO(s) + 4NO_2(g) + O_2(g)$:} \\\) This is a decomposition reaction because a single compound breaks down into multiple products. Thus, $B \rightarrow (I)$.
\(\textbf{(C) $2Na(s) + 2H_2O \rightarrow 2NaOH(aq) + H_2(g)$:} \\\) This is a displacement reaction as sodium displaces hydrogen from water. Thus, $C \rightarrow (II)$.
\(\textbf{(D) $2NO_2(g) + 2OH^-(aq) \rightarrow NO^-_2(aq) + NO^-_3(aq) + H_2O(l)$:} \\\) This reaction involves disproportionation because the same species ($NO_2$) is oxidized and reduced simultaneously. Thus, $D \rightarrow (III)$.
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