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CHXI08:REDOX REACTIONS

315450 Which of the acid possesses oxidizing, reducing and complex forming properties?

1

{HNO}_{3}

2

H_{2} {SO}_{4}

3 HCl

4

{HNO}_{2}

Explanation:

An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent.
Here, in ${HNO}_{2}$ , ' N ' is in +3 state (Intermediate oxidation state).

CHXI08:REDOX REACTIONS

315451 Which of the following reaction is an example of redox reaction?

1

{CH}_{2} = {CH}_{2} (g) + H_{2} (g) \to H_{3} C - {CH}_{3} (g)

2

NaOH (

aq

) + HCl (

aq

) \to NaCl (

aq

)

+ H_{2} O (1)

3

{XeF}_{6} (g) + 3 H_{2} O (1) \to {XeO}_{3} + 6 HF

4 All of these

Explanation:

$\underset{C \to - 2}{C H_{2} = C H_{2}} + \underset{H \to 0}{H_{2}} \to \underset{C \to - 3,H \to + 1 (oxidation state)}{C H_{3} - C H_{3}}$
So, it is disproportionation.

CHXI08:REDOX REACTIONS

315462 Of the following processes, the one that represents disproportionation is

1

Cu + 4 {HNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 {NO}_{2} + 2 H_{2} O

2

3 I_{2} + 6 {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O

3

{Cl}_{2} + I_{2} \to 2 ICl

4

Zn + 2 HCl \to {ZnCl}_{2} + H_{2}

CHXI08:REDOX REACTIONS

315452 Which of the following elements does not show disproportionation tendency?

1

Cl

2

Br

3

F

4 I

Explanation:

Being the most electronegative element, $F$ can only be reduced and hence it always shows an oxidation number of $- 1$ . Further, due to the absence of $d$ - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.

NCERT Exemplar

CHXI08:REDOX REACTIONS

315450 Which of the acid possesses oxidizing, reducing and complex forming properties?

1

{HNO}_{3}

2

H_{2} {SO}_{4}

3 HCl

4

{HNO}_{2}

Explanation:

An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent.
Here, in ${HNO}_{2}$ , ' N ' is in +3 state (Intermediate oxidation state).

CHXI08:REDOX REACTIONS

315451 Which of the following reaction is an example of redox reaction?

1

{CH}_{2} = {CH}_{2} (g) + H_{2} (g) \to H_{3} C - {CH}_{3} (g)

2

NaOH (

aq

) + HCl (

aq

) \to NaCl (

aq

)

+ H_{2} O (1)

3

{XeF}_{6} (g) + 3 H_{2} O (1) \to {XeO}_{3} + 6 HF

4 All of these

Explanation:

$\underset{C \to - 2}{C H_{2} = C H_{2}} + \underset{H \to 0}{H_{2}} \to \underset{C \to - 3,H \to + 1 (oxidation state)}{C H_{3} - C H_{3}}$
So, it is disproportionation.

CHXI08:REDOX REACTIONS

315462 Of the following processes, the one that represents disproportionation is

1

Cu + 4 {HNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 {NO}_{2} + 2 H_{2} O

2

3 I_{2} + 6 {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O

3

{Cl}_{2} + I_{2} \to 2 ICl

4

Zn + 2 HCl \to {ZnCl}_{2} + H_{2}

CHXI08:REDOX REACTIONS

315452 Which of the following elements does not show disproportionation tendency?

1

Cl

2

Br

3

F

4 I

Explanation:

Being the most electronegative element, $F$ can only be reduced and hence it always shows an oxidation number of $- 1$ . Further, due to the absence of $d$ - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.

NCERT Exemplar

CHXI08:REDOX REACTIONS

315450 Which of the acid possesses oxidizing, reducing and complex forming properties?

1

{HNO}_{3}

2

H_{2} {SO}_{4}

3 HCl

4

{HNO}_{2}

Explanation:

An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent.
Here, in ${HNO}_{2}$ , ' N ' is in +3 state (Intermediate oxidation state).

CHXI08:REDOX REACTIONS

315451 Which of the following reaction is an example of redox reaction?

1

{CH}_{2} = {CH}_{2} (g) + H_{2} (g) \to H_{3} C - {CH}_{3} (g)

2

NaOH (

aq

) + HCl (

aq

) \to NaCl (

aq

)

+ H_{2} O (1)

3

{XeF}_{6} (g) + 3 H_{2} O (1) \to {XeO}_{3} + 6 HF

4 All of these

Explanation:

$\underset{C \to - 2}{C H_{2} = C H_{2}} + \underset{H \to 0}{H_{2}} \to \underset{C \to - 3,H \to + 1 (oxidation state)}{C H_{3} - C H_{3}}$
So, it is disproportionation.

CHXI08:REDOX REACTIONS

315462 Of the following processes, the one that represents disproportionation is

1

Cu + 4 {HNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 {NO}_{2} + 2 H_{2} O

2

3 I_{2} + 6 {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O

3

{Cl}_{2} + I_{2} \to 2 ICl

4

Zn + 2 HCl \to {ZnCl}_{2} + H_{2}

CHXI08:REDOX REACTIONS

315452 Which of the following elements does not show disproportionation tendency?

1

Cl

2

Br

3

F

4 I

Explanation:

Being the most electronegative element, $F$ can only be reduced and hence it always shows an oxidation number of $- 1$ . Further, due to the absence of $d$ - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.

NCERT Exemplar

CHXI08:REDOX REACTIONS

315450 Which of the acid possesses oxidizing, reducing and complex forming properties?

1

{HNO}_{3}

2

H_{2} {SO}_{4}

3 HCl

4

{HNO}_{2}

Explanation:

An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent.
Here, in ${HNO}_{2}$ , ' N ' is in +3 state (Intermediate oxidation state).

CHXI08:REDOX REACTIONS

315451 Which of the following reaction is an example of redox reaction?

1

{CH}_{2} = {CH}_{2} (g) + H_{2} (g) \to H_{3} C - {CH}_{3} (g)

2

NaOH (

aq

) + HCl (

aq

) \to NaCl (

aq

)

+ H_{2} O (1)

3

{XeF}_{6} (g) + 3 H_{2} O (1) \to {XeO}_{3} + 6 HF

4 All of these

Explanation:

$\underset{C \to - 2}{C H_{2} = C H_{2}} + \underset{H \to 0}{H_{2}} \to \underset{C \to - 3,H \to + 1 (oxidation state)}{C H_{3} - C H_{3}}$
So, it is disproportionation.

CHXI08:REDOX REACTIONS

315462 Of the following processes, the one that represents disproportionation is

1

Cu + 4 {HNO}_{3} \to Cu {({NO}_{3})}_{2} + 2 {NO}_{2} + 2 H_{2} O

2

3 I_{2} + 6 {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O

3

{Cl}_{2} + I_{2} \to 2 ICl

4

Zn + 2 HCl \to {ZnCl}_{2} + H_{2}

CHXI08:REDOX REACTIONS

315452 Which of the following elements does not show disproportionation tendency?

1

Cl

2

Br

3

F

4 I

Explanation:

Being the most electronegative element, $F$ can only be reduced and hence it always shows an oxidation number of $- 1$ . Further, due to the absence of $d$ - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.

NCERT Exemplar

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