QBManager

6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous $NaCl$ respectively: [RBQ]

1

H_{2}

gas at cathode,

O_{2}

gas at anode

2

H_{2}

gas at cathode,

{Cl}_{2}

gas at anode

3

H_{2}

gas at anode,

{Cl}_{2}

gas at cathode

4

H_{2}

gas at anode,

O_{2}

gas at cathode

CBSE 2008

6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1

{CuCl}_{2}

2

{KMnO}_{4}

3

{ZnCl}_{2}

4

{CH}_{3} COONa

Explanation:

It is due to positive electrode potential of $Cu$ .

NCERT-XII-34

6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
$\begin{matrix} E^{\circ} {Cr}_{2} O_{7}^{- 2} / {Cr}^{3 +} = 1.33 V, E^{\circ} {Cl}_{2} / {Cl}^{-} = 1.36 V, \\ E^{\circ} {MnO}_{4}^{-} / {Mn}^{2 +} = 1.51 V, E^{\circ} {Cr}^{3 +} / Cr = - 0.74 V \end{matrix}$ [RBQ]

1

{Cr}^{3 +} < {Cl}^{-} < {Mn}^{2 +} < Cr

2

{Mn}^{2 +} < {Cl}^{-} < {Cr}^{3 +} < Cr

3

{Cr}^{3 +} < {Cl}^{-} < {Cr}_{2} O_{7}^{2 -} < {MnO}_{4}^{-}

4

{Mn}^{2 +} < {Cr}^{3 +} < {Cl}^{-} < Cr

CBSE 2005

6 RBTS PAPER

163245 For the given cell $M g | {M g}^{2 +} | | {Cu}^{2 +} | Cu$ [RBQ]

1

Cu

is the oxidising agent

2 Cu is cathode

3 The cell reaction is

Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu

4 Both 2 and 3 option are correct

Explanation:

$Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu$

CBSE 2011

6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for $40 \min$ . The amount of zinc deposited at the cathode is : [RBQ]

1

40.65 g

2

0.4065 g

3

4.065 g

4

65.04 g

Explanation:

Current, $I = 5 A$
time, $t = 40 \min = 40 \times 60 = 2400 s$
Amount of electricity passed
$Q = It$
$Q = 5 \times 2400$
$Q = 12000 C$
$Z n^{2} + 2 e^{-} \to Z n$
$2 \times 96500 C$ charge deposite $= 65.39 g$ of zinc
$1 C$ charge deposite $= \frac{65.39}{2 \times 96500}$ gof zinc
therefore, $12000 C$ charge will deposite
$= \frac{65.39 \times 12000}{2 \times 96500} = 4.065 g of zinc$

NCERT-XII-52

6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous $NaCl$ respectively: [RBQ]

1

H_{2}

gas at cathode,

O_{2}

gas at anode

2

H_{2}

gas at cathode,

{Cl}_{2}

gas at anode

3

H_{2}

gas at anode,

{Cl}_{2}

gas at cathode

4

H_{2}

gas at anode,

O_{2}

gas at cathode

CBSE 2008

6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1

{CuCl}_{2}

2

{KMnO}_{4}

3

{ZnCl}_{2}

4

{CH}_{3} COONa

Explanation:

It is due to positive electrode potential of $Cu$ .

NCERT-XII-34

6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
$\begin{matrix} E^{\circ} {Cr}_{2} O_{7}^{- 2} / {Cr}^{3 +} = 1.33 V, E^{\circ} {Cl}_{2} / {Cl}^{-} = 1.36 V, \\ E^{\circ} {MnO}_{4}^{-} / {Mn}^{2 +} = 1.51 V, E^{\circ} {Cr}^{3 +} / Cr = - 0.74 V \end{matrix}$ [RBQ]

1

{Cr}^{3 +} < {Cl}^{-} < {Mn}^{2 +} < Cr

2

{Mn}^{2 +} < {Cl}^{-} < {Cr}^{3 +} < Cr

3

{Cr}^{3 +} < {Cl}^{-} < {Cr}_{2} O_{7}^{2 -} < {MnO}_{4}^{-}

4

{Mn}^{2 +} < {Cr}^{3 +} < {Cl}^{-} < Cr

CBSE 2005

6 RBTS PAPER

163245 For the given cell $M g | {M g}^{2 +} | | {Cu}^{2 +} | Cu$ [RBQ]

1

Cu

is the oxidising agent

2 Cu is cathode

3 The cell reaction is

Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu

4 Both 2 and 3 option are correct

Explanation:

$Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu$

CBSE 2011

6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for $40 \min$ . The amount of zinc deposited at the cathode is : [RBQ]

1

40.65 g

2

0.4065 g

3

4.065 g

4

65.04 g

Explanation:

Current, $I = 5 A$
time, $t = 40 \min = 40 \times 60 = 2400 s$
Amount of electricity passed
$Q = It$
$Q = 5 \times 2400$
$Q = 12000 C$
$Z n^{2} + 2 e^{-} \to Z n$
$2 \times 96500 C$ charge deposite $= 65.39 g$ of zinc
$1 C$ charge deposite $= \frac{65.39}{2 \times 96500}$ gof zinc
therefore, $12000 C$ charge will deposite
$= \frac{65.39 \times 12000}{2 \times 96500} = 4.065 g of zinc$

NCERT-XII-52

6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous $NaCl$ respectively: [RBQ]

1

H_{2}

gas at cathode,

O_{2}

gas at anode

2

H_{2}

gas at cathode,

{Cl}_{2}

gas at anode

3

H_{2}

gas at anode,

{Cl}_{2}

gas at cathode

4

H_{2}

gas at anode,

O_{2}

gas at cathode

CBSE 2008

6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1

{CuCl}_{2}

2

{KMnO}_{4}

3

{ZnCl}_{2}

4

{CH}_{3} COONa

Explanation:

It is due to positive electrode potential of $Cu$ .

NCERT-XII-34

6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
$\begin{matrix} E^{\circ} {Cr}_{2} O_{7}^{- 2} / {Cr}^{3 +} = 1.33 V, E^{\circ} {Cl}_{2} / {Cl}^{-} = 1.36 V, \\ E^{\circ} {MnO}_{4}^{-} / {Mn}^{2 +} = 1.51 V, E^{\circ} {Cr}^{3 +} / Cr = - 0.74 V \end{matrix}$ [RBQ]

1

{Cr}^{3 +} < {Cl}^{-} < {Mn}^{2 +} < Cr

2

{Mn}^{2 +} < {Cl}^{-} < {Cr}^{3 +} < Cr

3

{Cr}^{3 +} < {Cl}^{-} < {Cr}_{2} O_{7}^{2 -} < {MnO}_{4}^{-}

4

{Mn}^{2 +} < {Cr}^{3 +} < {Cl}^{-} < Cr

CBSE 2005

6 RBTS PAPER

163245 For the given cell $M g | {M g}^{2 +} | | {Cu}^{2 +} | Cu$ [RBQ]

1

Cu

is the oxidising agent

2 Cu is cathode

3 The cell reaction is

Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu

4 Both 2 and 3 option are correct

Explanation:

$Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu$

CBSE 2011

6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for $40 \min$ . The amount of zinc deposited at the cathode is : [RBQ]

1

40.65 g

2

0.4065 g

3

4.065 g

4

65.04 g

Explanation:

Current, $I = 5 A$
time, $t = 40 \min = 40 \times 60 = 2400 s$
Amount of electricity passed
$Q = It$
$Q = 5 \times 2400$
$Q = 12000 C$
$Z n^{2} + 2 e^{-} \to Z n$
$2 \times 96500 C$ charge deposite $= 65.39 g$ of zinc
$1 C$ charge deposite $= \frac{65.39}{2 \times 96500}$ gof zinc
therefore, $12000 C$ charge will deposite
$= \frac{65.39 \times 12000}{2 \times 96500} = 4.065 g of zinc$

NCERT-XII-52

6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous $NaCl$ respectively: [RBQ]

1

H_{2}

gas at cathode,

O_{2}

gas at anode

2

H_{2}

gas at cathode,

{Cl}_{2}

gas at anode

3

H_{2}

gas at anode,

{Cl}_{2}

gas at cathode

4

H_{2}

gas at anode,

O_{2}

gas at cathode

CBSE 2008

6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1

{CuCl}_{2}

2

{KMnO}_{4}

3

{ZnCl}_{2}

4

{CH}_{3} COONa

Explanation:

It is due to positive electrode potential of $Cu$ .

NCERT-XII-34

6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
$\begin{matrix} E^{\circ} {Cr}_{2} O_{7}^{- 2} / {Cr}^{3 +} = 1.33 V, E^{\circ} {Cl}_{2} / {Cl}^{-} = 1.36 V, \\ E^{\circ} {MnO}_{4}^{-} / {Mn}^{2 +} = 1.51 V, E^{\circ} {Cr}^{3 +} / Cr = - 0.74 V \end{matrix}$ [RBQ]

1

{Cr}^{3 +} < {Cl}^{-} < {Mn}^{2 +} < Cr

2

{Mn}^{2 +} < {Cl}^{-} < {Cr}^{3 +} < Cr

3

{Cr}^{3 +} < {Cl}^{-} < {Cr}_{2} O_{7}^{2 -} < {MnO}_{4}^{-}

4

{Mn}^{2 +} < {Cr}^{3 +} < {Cl}^{-} < Cr

CBSE 2005

6 RBTS PAPER

163245 For the given cell $M g | {M g}^{2 +} | | {Cu}^{2 +} | Cu$ [RBQ]

1

Cu

is the oxidising agent

2 Cu is cathode

3 The cell reaction is

Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu

4 Both 2 and 3 option are correct

Explanation:

$Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu$

CBSE 2011

6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for $40 \min$ . The amount of zinc deposited at the cathode is : [RBQ]

1

40.65 g

2

0.4065 g

3

4.065 g

4

65.04 g

Explanation:

Current, $I = 5 A$
time, $t = 40 \min = 40 \times 60 = 2400 s$
Amount of electricity passed
$Q = It$
$Q = 5 \times 2400$
$Q = 12000 C$
$Z n^{2} + 2 e^{-} \to Z n$
$2 \times 96500 C$ charge deposite $= 65.39 g$ of zinc
$1 C$ charge deposite $= \frac{65.39}{2 \times 96500}$ gof zinc
therefore, $12000 C$ charge will deposite
$= \frac{65.39 \times 12000}{2 \times 96500} = 4.065 g of zinc$

NCERT-XII-52

6 RBTS PAPER

163243 Find the product of electrolysis at anode and at cathode evolve due to electrolysis of aquous $NaCl$ respectively: [RBQ]

1

H_{2}

gas at cathode,

O_{2}

gas at anode

2

H_{2}

gas at cathode,

{Cl}_{2}

gas at anode

3

H_{2}

gas at anode,

{Cl}_{2}

gas at cathode

4

H_{2}

gas at anode,

O_{2}

gas at cathode

CBSE 2008

6 RBTS PAPER

163260 Which of the following aqueous solution produces metal after electrolysis : [RBQ]

1

{CuCl}_{2}

2

{KMnO}_{4}

3

{ZnCl}_{2}

4

{CH}_{3} COONa

Explanation:

It is due to positive electrode potential of $Cu$ .

NCERT-XII-34

6 RBTS PAPER

163244 Using the data given below find out in which option the order of reducing power is correct :
$\begin{matrix} E^{\circ} {Cr}_{2} O_{7}^{- 2} / {Cr}^{3 +} = 1.33 V, E^{\circ} {Cl}_{2} / {Cl}^{-} = 1.36 V, \\ E^{\circ} {MnO}_{4}^{-} / {Mn}^{2 +} = 1.51 V, E^{\circ} {Cr}^{3 +} / Cr = - 0.74 V \end{matrix}$ [RBQ]

1

{Cr}^{3 +} < {Cl}^{-} < {Mn}^{2 +} < Cr

2

{Mn}^{2 +} < {Cl}^{-} < {Cr}^{3 +} < Cr

3

{Cr}^{3 +} < {Cl}^{-} < {Cr}_{2} O_{7}^{2 -} < {MnO}_{4}^{-}

4

{Mn}^{2 +} < {Cr}^{3 +} < {Cl}^{-} < Cr

CBSE 2005

6 RBTS PAPER

163245 For the given cell $M g | {M g}^{2 +} | | {Cu}^{2 +} | Cu$ [RBQ]

1

Cu

is the oxidising agent

2 Cu is cathode

3 The cell reaction is

Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu

4 Both 2 and 3 option are correct

Explanation:

$Mg + {Cu}^{2 +} \to {Mg}^{2 +} + Cu$

CBSE 2011

6 RBTS PAPER

163246 A 5A current is passed through a solution of zinc sulphate for $40 \min$ . The amount of zinc deposited at the cathode is : [RBQ]

1

40.65 g

2

0.4065 g

3

4.065 g

4

65.04 g

Explanation:

Current, $I = 5 A$
time, $t = 40 \min = 40 \times 60 = 2400 s$
Amount of electricity passed
$Q = It$
$Q = 5 \times 2400$
$Q = 12000 C$
$Z n^{2} + 2 e^{-} \to Z n$
$2 \times 96500 C$ charge deposite $= 65.39 g$ of zinc
$1 C$ charge deposite $= \frac{65.39}{2 \times 96500}$ gof zinc
therefore, $12000 C$ charge will deposite
$= \frac{65.39 \times 12000}{2 \times 96500} = 4.065 g of zinc$

NCERT-XII-52