Match List I with List II. .tg border-collapse:collapse;border-spacing:0; .tg tdborder-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal; .tg thborder-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal; .tg .tg-c3owborder-color:inherit;text-align:center;vertical-align:top .tg .tg-7bttborder-color:inherit;font-weight:bold;text-align:center;vertical-align:top .tg .tg-0pkyborder-color:inherit;text-align:left;vertical-align:top LIST I Reaction LIST II Type of redox reaction A. N_2(~g)+O_2(~g) arrow 2 NO_(g) I. Decomposition B. 2 ~Pb(NO_3)_2(~s) arrow 2 PbO_(s)+4 NO_2(~g)+O_2(~g) II. Displacement C. 2 Na_(s)+2 H_2 O_(l) arrow 2 NaOH_(aq .)+H_2(~g) III. Disproportionation D. 2 NO_2(~g)+2^- OH( aq. ) arrow NO_2(aq .)^-+NO_3( aq. )^-+H_2 O_(l) IV. Combination Choose the correct answer from the options given below :

(A)-(IV), (B)-(I), (C)-(II), (D)-(III)

(A)-(I), (B)-(II), (C)-(III), (D)-(IV)

(A)-(II), (B)-(III), (C)-(IV), (D)-(I)

(A)-(III), (B)-(II), (C)-(I), (D)-(IV)

Redox Reactions PYQ — JEE Main 2024 · 6 Apr · Shift 2 · Q5 with Solution

Match List I with List II.

	LIST I Reaction		LIST II Type of redox reaction
A.	$\mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NO}_{(\mathrm{g})}$	I.	Decomposition
B.	$2 \mathrm{~Pb}\left(\mathrm{NO}_3\right)_{2(\mathrm{~s})} \rightarrow 2 \mathrm{PbO}_{(\mathrm{s})}+4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$	II.	Displacement
C.	$2 \mathrm{Na}_{(\mathrm{s})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow 2 \mathrm{NaOH}_{(\mathrm{aq} .)}+\mathrm{H}_{2(\mathrm{~g})}$	III.	Disproportionation
D.	$2 \mathrm{NO}_{2(\mathrm{~g})}+2^{-} \mathrm{OH}(\text { aq. }) \rightarrow \mathrm{NO}_{2(\mathrm{aq} .)}^{-}+\mathrm{NO}_{3(\text { aq. })}^{-}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$	IV.	Combination

Choose the correct answer from the options given below :

A
(A)-(IV), (B)-(I), (C)-(II), (D)-(III)
B
(A)-(I), (B)-(II), (C)-(III), (D)-(IV)
C
(A)-(II), (B)-(III), (C)-(IV), (D)-(I)
D
(A)-(III), (B)-(II), (C)-(I), (D)-(IV)

View written solutionFree

Correct answer: A

Identify the type of each reaction in List I

A. $\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}$

Two reactants combine to form a single product type.

This is a combination reaction.

So, $A \rightarrow IV$

B. $2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}$

A single compound breaks into simpler substances.

This is a decomposition reaction.

So, $B \rightarrow I$

C. $2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}$

Sodium displaces hydrogen from water.

This is a displacement reaction.

So, $C \rightarrow II$

D. $2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}$

Here nitrogen in $\mathrm{NO_2}$ has oxidation state $+4$ .

In products:

In $\mathrm{NO_2^-}$ , N is $+3$
In $\mathrm{NO_3^-}$ , N is $+5$

So the same species undergoes both oxidation and reduction.

This is disproportionation.

So, $D \rightarrow III$

Final matching

$A-IV, \quad B-I, \quad C-II, \quad D-III$

Compare with options

This corresponds to Option A.

Comparison with stored answer

Stored correct answer: A

My derived answer: A

They agree.

More from Redox Reactions

Match List I with List II.

	LIST I Reaction		LIST II Type of redox reaction
A.	$\mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NO}_{(\mathrm{g})}$	I.	Decomposition
B.	$2 \mathrm{~Pb}\left(\mathrm{NO}_3\right)_{2(\mathrm{~s})} \rightarrow 2 \mathrm{PbO}_{(\mathrm{s})}+4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$	II.	Displacement
C.	$2 \mathrm{Na}_{(\mathrm{s})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})} \rightarrow 2 \mathrm{NaOH}_{(\mathrm{aq} .)}+\mathrm{H}_{2(\mathrm{~g})}$	III.	Disproportionation
D.	$2 \mathrm{NO}_{2(\mathrm{~g})}+2^{-} \mathrm{OH}(\text { aq. }) \rightarrow \mathrm{NO}_{2(\mathrm{aq} .)}^{-}+\mathrm{NO}_{3(\text { aq. })}^{-}+\mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$	IV.	Combination

Choose the correct answer from the options given below :

A
(A)-(IV), (B)-(I), (C)-(II), (D)-(III)
B
(A)-(I), (B)-(II), (C)-(III), (D)-(IV)
C
(A)-(II), (B)-(III), (C)-(IV), (D)-(I)
D
(A)-(III), (B)-(II), (C)-(I), (D)-(IV)

View written solutionFree

Correct answer: A

Identify the type of each reaction in List I

A. $\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}$

Two reactants combine to form a single product type.

This is a combination reaction.

So, $A \rightarrow IV$

B. $2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}$

A single compound breaks into simpler substances.

This is a decomposition reaction.

So, $B \rightarrow I$

C. $2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}$

Sodium displaces hydrogen from water.

This is a displacement reaction.

So, $C \rightarrow II$

D. $2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}$

Here nitrogen in $\mathrm{NO_2}$ has oxidation state $+4$ .

In products:

In $\mathrm{NO_2^-}$ , N is $+3$
In $\mathrm{NO_3^-}$ , N is $+5$

So the same species undergoes both oxidation and reduction.

This is disproportionation.

So, $D \rightarrow III$

Final matching

$A-IV, \quad B-I, \quad C-II, \quad D-III$

Compare with options

This corresponds to Option A.

Comparison with stored answer

Stored correct answer: A

My derived answer: A

They agree.

Redox Reactions question

Redox Reactions question

A. $\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}$

B. $2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}$

C. $2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}$

D. $2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}$

More from Redox Reactions

Redox Reactions question

Redox Reactions question

A. $\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}$

B. $2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}$

C. $2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}$

D. $2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}$

More from Redox Reactions

A. N2(g)+O2(g)→2NO(g)\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}N2​(g)+O2​(g)→2NO(g)

B. 2Pb(NO3)2(s)→2PbO(s)+4NO2(g)+O2(g)2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}2Pb(NO3​)2​(s)→2PbO(s)+4NO2​(g)+O2​(g)

C. 2Na(s)+2H2O(l)→2NaOH(aq)+H2(g)2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}2Na(s)+2H2​O(l)→2NaOH(aq)+H2​(g)

D. 2NO2(g)+2OH−(aq)→NO2−(aq)+NO3−(aq)+H2O(l)2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}2NO2​(g)+2OH−(aq)→NO2−​(aq)+NO3−​(aq)+H2​O(l)

More from Redox Reactions

A. N2(g)+O2(g)→2NO(g)\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}N2​(g)+O2​(g)→2NO(g)

B. 2Pb(NO3)2(s)→2PbO(s)+4NO2(g)+O2(g)2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}2Pb(NO3​)2​(s)→2PbO(s)+4NO2​(g)+O2​(g)

C. 2Na(s)+2H2O(l)→2NaOH(aq)+H2(g)2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}2Na(s)+2H2​O(l)→2NaOH(aq)+H2​(g)

D. 2NO2(g)+2OH−(aq)→NO2−(aq)+NO3−(aq)+H2O(l)2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}2NO2​(g)+2OH−(aq)→NO2−​(aq)+NO3−​(aq)+H2​O(l)

More from Redox Reactions

A. $\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}$

B. $2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}$

C. $2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}$

D. $2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}$

A. $\mathrm{N_2(g) + O_2(g) \rightarrow 2NO(g)}$

B. $2\mathrm{Pb(NO_3)_2(s)} \rightarrow 2\mathrm{PbO(s)} + 4\mathrm{NO_2(g)} + \mathrm{O_2(g)}$

C. $2\mathrm{Na(s)} + 2\mathrm{H_2O(l)} \rightarrow 2\mathrm{NaOH(aq)} + \mathrm{H_2(g)}$

D. $2\mathrm{NO_2(g)} + 2\mathrm{OH^- (aq)} \rightarrow \mathrm{NO_2^- (aq)} + \mathrm{NO_3^- (aq)} + \mathrm{H_2O(l)}$