QBManager

CHXI08:REDOX REACTIONS

315453 $H_{2} O_{2} + H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}$ is an example of disproportionation because

1 O.N. of oxygen only decreases

2 O.N. of oxygen only increases

3 O.N. of oxygen decreases as well as increases

4 O.N. of oxygen neither decreases nor increases

CHXI08:REDOX REACTIONS

315454 In the reaction,
$3 {Br}_{2} + 6 {CO}_{3}^{2 -} + 3 H_{2} O \to 5 {Br}^{-} + {BrO}_{3}^{-} + 6 {HCO}_{3}^{-}$

1 Bromine is oxidised and carbonate is reduced

2 Bromine is oxidised as well as reduced

3 Bromine is reduced and water is oxidised

4

{Br}_{2}

is neither oxidised nor reduced

Explanation:

O.N. of $Br$ in
${Br}_{2} = 0$
${Br}^{-} = - 1$
${BrO}_{3}^{-} = + 5$
$Br$ is oxidised as well as reduced.

CHXI08:REDOX REACTIONS

315455 Which reaction does not represent auto redox or disproportionation?

1

{Cl}_{2} + {OH}^{-} ⟶ {Cl}^{-} + {ClO}_{3}^{-} + H_{2} O

2

2 H_{2} O_{2} ⟶ H_{2} O + O_{2}

3

2 {Cu}^{+} ⟶ {Cu}^{2 +} + Cu

4

{({NH}_{4})}_{2} {Cr}_{2} O_{7} ⟶ N_{2} + {Cr}_{2} O_{3} + 4 H_{2} O

Explanation:

In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) ${Cl}_{2}$ ; (2), $H_{2} O_{2}$ and (3), ${Cu}^{+}$ is oxidized as well as reduced. In (4), $N$ is oxidized and $Cr$ is reduced in one molecule of ${({NH}_{4})}_{2} {Cr}_{2} O_{7}$ and thus it is intramolecular redox.

CHXI08:REDOX REACTIONS

315456 Identify disproportionation reaction

1

{CH}_{4} + 2 O_{2} ⟶ {CO}_{2} + 2 H_{2} O

2

{CH}_{4} + 4 {Cl}_{2} ⟶ {CCl}_{4} + 4 HCl

3

2 F_{4} + 2 {OH}^{-} ⟶ 2 F^{-} + {OF}_{2} + H_{2} O

4

2 {NO}_{2} + 2 {OH}^{-} ⟶ {NO}_{2}^{-} + {NO}_{3}^{-} + H_{2} O

NCERT Exemplar

CHXI08:REDOX REACTIONS

315457 During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is

1

1 : 5

2

5 : 1

3

3 : 1

4

1 : 3

Explanation:

$3 I_{2} + \underset{―}{6} {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O$
So, ratio of iodate to iodide ion is $1 : 5$ .

CHXI08:REDOX REACTIONS

315453 $H_{2} O_{2} + H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}$ is an example of disproportionation because

1 O.N. of oxygen only decreases

2 O.N. of oxygen only increases

3 O.N. of oxygen decreases as well as increases

4 O.N. of oxygen neither decreases nor increases

CHXI08:REDOX REACTIONS

315454 In the reaction,
$3 {Br}_{2} + 6 {CO}_{3}^{2 -} + 3 H_{2} O \to 5 {Br}^{-} + {BrO}_{3}^{-} + 6 {HCO}_{3}^{-}$

1 Bromine is oxidised and carbonate is reduced

2 Bromine is oxidised as well as reduced

3 Bromine is reduced and water is oxidised

4

{Br}_{2}

is neither oxidised nor reduced

Explanation:

O.N. of $Br$ in
${Br}_{2} = 0$
${Br}^{-} = - 1$
${BrO}_{3}^{-} = + 5$
$Br$ is oxidised as well as reduced.

CHXI08:REDOX REACTIONS

315455 Which reaction does not represent auto redox or disproportionation?

1

{Cl}_{2} + {OH}^{-} ⟶ {Cl}^{-} + {ClO}_{3}^{-} + H_{2} O

2

2 H_{2} O_{2} ⟶ H_{2} O + O_{2}

3

2 {Cu}^{+} ⟶ {Cu}^{2 +} + Cu

4

{({NH}_{4})}_{2} {Cr}_{2} O_{7} ⟶ N_{2} + {Cr}_{2} O_{3} + 4 H_{2} O

Explanation:

In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) ${Cl}_{2}$ ; (2), $H_{2} O_{2}$ and (3), ${Cu}^{+}$ is oxidized as well as reduced. In (4), $N$ is oxidized and $Cr$ is reduced in one molecule of ${({NH}_{4})}_{2} {Cr}_{2} O_{7}$ and thus it is intramolecular redox.

CHXI08:REDOX REACTIONS

315456 Identify disproportionation reaction

1

{CH}_{4} + 2 O_{2} ⟶ {CO}_{2} + 2 H_{2} O

2

{CH}_{4} + 4 {Cl}_{2} ⟶ {CCl}_{4} + 4 HCl

3

2 F_{4} + 2 {OH}^{-} ⟶ 2 F^{-} + {OF}_{2} + H_{2} O

4

2 {NO}_{2} + 2 {OH}^{-} ⟶ {NO}_{2}^{-} + {NO}_{3}^{-} + H_{2} O

NCERT Exemplar

CHXI08:REDOX REACTIONS

315457 During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is

1

1 : 5

2

5 : 1

3

3 : 1

4

1 : 3

Explanation:

$3 I_{2} + \underset{―}{6} {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O$
So, ratio of iodate to iodide ion is $1 : 5$ .

CHXI08:REDOX REACTIONS

315453 $H_{2} O_{2} + H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}$ is an example of disproportionation because

1 O.N. of oxygen only decreases

2 O.N. of oxygen only increases

3 O.N. of oxygen decreases as well as increases

4 O.N. of oxygen neither decreases nor increases

CHXI08:REDOX REACTIONS

315454 In the reaction,
$3 {Br}_{2} + 6 {CO}_{3}^{2 -} + 3 H_{2} O \to 5 {Br}^{-} + {BrO}_{3}^{-} + 6 {HCO}_{3}^{-}$

1 Bromine is oxidised and carbonate is reduced

2 Bromine is oxidised as well as reduced

3 Bromine is reduced and water is oxidised

4

{Br}_{2}

is neither oxidised nor reduced

Explanation:

O.N. of $Br$ in
${Br}_{2} = 0$
${Br}^{-} = - 1$
${BrO}_{3}^{-} = + 5$
$Br$ is oxidised as well as reduced.

CHXI08:REDOX REACTIONS

315455 Which reaction does not represent auto redox or disproportionation?

1

{Cl}_{2} + {OH}^{-} ⟶ {Cl}^{-} + {ClO}_{3}^{-} + H_{2} O

2

2 H_{2} O_{2} ⟶ H_{2} O + O_{2}

3

2 {Cu}^{+} ⟶ {Cu}^{2 +} + Cu

4

{({NH}_{4})}_{2} {Cr}_{2} O_{7} ⟶ N_{2} + {Cr}_{2} O_{3} + 4 H_{2} O

Explanation:

In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) ${Cl}_{2}$ ; (2), $H_{2} O_{2}$ and (3), ${Cu}^{+}$ is oxidized as well as reduced. In (4), $N$ is oxidized and $Cr$ is reduced in one molecule of ${({NH}_{4})}_{2} {Cr}_{2} O_{7}$ and thus it is intramolecular redox.

CHXI08:REDOX REACTIONS

315456 Identify disproportionation reaction

1

{CH}_{4} + 2 O_{2} ⟶ {CO}_{2} + 2 H_{2} O

2

{CH}_{4} + 4 {Cl}_{2} ⟶ {CCl}_{4} + 4 HCl

3

2 F_{4} + 2 {OH}^{-} ⟶ 2 F^{-} + {OF}_{2} + H_{2} O

4

2 {NO}_{2} + 2 {OH}^{-} ⟶ {NO}_{2}^{-} + {NO}_{3}^{-} + H_{2} O

NCERT Exemplar

CHXI08:REDOX REACTIONS

315457 During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is

1

1 : 5

2

5 : 1

3

3 : 1

4

1 : 3

Explanation:

$3 I_{2} + \underset{―}{6} {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O$
So, ratio of iodate to iodide ion is $1 : 5$ .

CHXI08:REDOX REACTIONS

315453 $H_{2} O_{2} + H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}$ is an example of disproportionation because

1 O.N. of oxygen only decreases

2 O.N. of oxygen only increases

3 O.N. of oxygen decreases as well as increases

4 O.N. of oxygen neither decreases nor increases

CHXI08:REDOX REACTIONS

315454 In the reaction,
$3 {Br}_{2} + 6 {CO}_{3}^{2 -} + 3 H_{2} O \to 5 {Br}^{-} + {BrO}_{3}^{-} + 6 {HCO}_{3}^{-}$

1 Bromine is oxidised and carbonate is reduced

2 Bromine is oxidised as well as reduced

3 Bromine is reduced and water is oxidised

4

{Br}_{2}

is neither oxidised nor reduced

Explanation:

O.N. of $Br$ in
${Br}_{2} = 0$
${Br}^{-} = - 1$
${BrO}_{3}^{-} = + 5$
$Br$ is oxidised as well as reduced.

CHXI08:REDOX REACTIONS

315455 Which reaction does not represent auto redox or disproportionation?

1

{Cl}_{2} + {OH}^{-} ⟶ {Cl}^{-} + {ClO}_{3}^{-} + H_{2} O

2

2 H_{2} O_{2} ⟶ H_{2} O + O_{2}

3

2 {Cu}^{+} ⟶ {Cu}^{2 +} + Cu

4

{({NH}_{4})}_{2} {Cr}_{2} O_{7} ⟶ N_{2} + {Cr}_{2} O_{3} + 4 H_{2} O

Explanation:

In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) ${Cl}_{2}$ ; (2), $H_{2} O_{2}$ and (3), ${Cu}^{+}$ is oxidized as well as reduced. In (4), $N$ is oxidized and $Cr$ is reduced in one molecule of ${({NH}_{4})}_{2} {Cr}_{2} O_{7}$ and thus it is intramolecular redox.

CHXI08:REDOX REACTIONS

315456 Identify disproportionation reaction

1

{CH}_{4} + 2 O_{2} ⟶ {CO}_{2} + 2 H_{2} O

2

{CH}_{4} + 4 {Cl}_{2} ⟶ {CCl}_{4} + 4 HCl

3

2 F_{4} + 2 {OH}^{-} ⟶ 2 F^{-} + {OF}_{2} + H_{2} O

4

2 {NO}_{2} + 2 {OH}^{-} ⟶ {NO}_{2}^{-} + {NO}_{3}^{-} + H_{2} O

NCERT Exemplar

CHXI08:REDOX REACTIONS

315457 During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is

1

1 : 5

2

5 : 1

3

3 : 1

4

1 : 3

Explanation:

$3 I_{2} + \underset{―}{6} {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O$
So, ratio of iodate to iodide ion is $1 : 5$ .

CHXI08:REDOX REACTIONS

315453 $H_{2} O_{2} + H_{2} O_{2} ⟶ 2 H_{2} O + O_{2}$ is an example of disproportionation because

1 O.N. of oxygen only decreases

2 O.N. of oxygen only increases

3 O.N. of oxygen decreases as well as increases

4 O.N. of oxygen neither decreases nor increases

CHXI08:REDOX REACTIONS

315454 In the reaction,
$3 {Br}_{2} + 6 {CO}_{3}^{2 -} + 3 H_{2} O \to 5 {Br}^{-} + {BrO}_{3}^{-} + 6 {HCO}_{3}^{-}$

1 Bromine is oxidised and carbonate is reduced

2 Bromine is oxidised as well as reduced

3 Bromine is reduced and water is oxidised

4

{Br}_{2}

is neither oxidised nor reduced

Explanation:

O.N. of $Br$ in
${Br}_{2} = 0$
${Br}^{-} = - 1$
${BrO}_{3}^{-} = + 5$
$Br$ is oxidised as well as reduced.

CHXI08:REDOX REACTIONS

315455 Which reaction does not represent auto redox or disproportionation?

1

{Cl}_{2} + {OH}^{-} ⟶ {Cl}^{-} + {ClO}_{3}^{-} + H_{2} O

2

2 H_{2} O_{2} ⟶ H_{2} O + O_{2}

3

2 {Cu}^{+} ⟶ {Cu}^{2 +} + Cu

4

{({NH}_{4})}_{2} {Cr}_{2} O_{7} ⟶ N_{2} + {Cr}_{2} O_{3} + 4 H_{2} O

Explanation:

In auto redox or disproportionation, same element is oxidized as well as reduced. In (1) ${Cl}_{2}$ ; (2), $H_{2} O_{2}$ and (3), ${Cu}^{+}$ is oxidized as well as reduced. In (4), $N$ is oxidized and $Cr$ is reduced in one molecule of ${({NH}_{4})}_{2} {Cr}_{2} O_{7}$ and thus it is intramolecular redox.

CHXI08:REDOX REACTIONS

315456 Identify disproportionation reaction

1

{CH}_{4} + 2 O_{2} ⟶ {CO}_{2} + 2 H_{2} O

2

{CH}_{4} + 4 {Cl}_{2} ⟶ {CCl}_{4} + 4 HCl

3

2 F_{4} + 2 {OH}^{-} ⟶ 2 F^{-} + {OF}_{2} + H_{2} O

4

2 {NO}_{2} + 2 {OH}^{-} ⟶ {NO}_{2}^{-} + {NO}_{3}^{-} + H_{2} O

NCERT Exemplar

CHXI08:REDOX REACTIONS

315457 During the disproportionation of iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is

1

1 : 5

2

5 : 1

3

3 : 1

4

1 : 3

Explanation:

$3 I_{2} + \underset{―}{6} {OH}^{-} \to {IO}_{3}^{-} + 5 I^{-} + 3 H_{2} O$
So, ratio of iodate to iodide ion is $1 : 5$ .

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