Chemical Effects of Current Test

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Chemical Effects of Current Test - 5

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Weekly Quiz Competition

Question 1
1 / -0

In a galvanic cell, electrons flow through the external circuit

A
from a negative electrode to a positive electrode

B
in both the directions

C
from a positive electrode to a negative electrode

D
from a cathode to an anode

Solution

In a galvanic cell, electrons flow through the external circuit from a negative electrode to a positive electrode.
Question 2
1 / -0

Arrange the following anions in the increasing ease of discharge.

A
SO₄^-2< Cl^–< I^– < OH^–

B
SO₄^-2< Cl^– < OH^– < I^–

C
Cl^– < I^– < SO₄^-2 < OH^–

D
Cl^– < I^– < OH^– < SO₄^-2

Solution

The anions get oxidised at the anode, and OH^- has the highest discharge potential.
So₄^-2 ion has low discharge potential and will be discharged only when a concentrated solution of a sulphate is taken.The ease of discharge of cations and anions during electrolysis is shown below:
Question 3
1 / -0

Which among the following is a non-electrolyte?

A
PbBr₂

B
CuSO₄

C
H₃PO₄

D
CS₂

Solution

CS₂ is a non-electrolyte because it does not form ions in aqueous solution.
Question 4
1 / -0

Which of the following elements would get discharged more readily at the cathode during electrolysis?

A
Pb

B
Ca

C
Ni

D
Al

Solution

The cation of an element lower in the reactivity series (having a greater reduction potential) is discharged at the cathode in preference to cations above it (having a lower reduction potential) in the reactivity series. Lead (Pb) will get discharged in preference to Ca, Ni and Al.
Question 5
1 / -0

On what factors does the selective discharge of ions depend?
1. The relative positions of ions in the electrochemical series.
2. The relative concentration of ions.
3. The nature of electrodes.

A
Both (1) and (2)

B
Both (1) and (3)

C
Only (1)

D
All of the above

Solution

The selective discharge of ions depends on the relative positions of ions in the electrochemical series, the relative concentration of ions and the nature of electrodes.
Question 6
1 / -0

Which of the following is/are discharged at cathode when electricity is passed through dilute CuSO₄ solution?

A
Cu²⁺, H₃O⁺

B
Cu²⁺

C
SO, OH^–

D
OH^–

Solution

Cu²⁺ ions are discharged at cathode when electricity is passed through dilute CuSO₄ solution.
Question 7
1 / -0

Which of the following ions is migrated to anode when electricity is passed through dilute NaCl solution?

A
Na⁺, H₃O⁺

B
H₃O⁺

C
Cl^–, OH^–

D
OH^–

Solution

Chloride and hydroxyl ions are migrated to anode when electricity is passed through dilute NaCl solution.
Question 8
1 / -0

Which of the following is not an inert electrode?

A
Pt

B
Au

C
C

D
Al

Solution

Inert electrode is an electrode that serves only as a source or sink for electrons without playing a chemical role in the electrode reaction. Precious metals, mercury and carbon are typically used as inert electrodes. Thus, aluminium is not an inert electrode.
Question 9
1 / -0

Why is the electrolyte named aqueous copper (II) sulphate acidified with dil. H₂SO₄?

A
To enhance the conductivity of the electrolyte

B
To enhance the hydrolysis of the electrolyte

C
To prevent the colour change of the solution

D
To prevent the discharge of ions

Solution

The electrolyte named aqueous copper (II) sulphate is acidified with dil. H₂SO₄ to enhance its conductivity.
Question 10
1 / -0

Which of the following is observed during the electrolysis of molten lead bromide?

A
Reddish brown fumes of bromine at cathode and Greyish lead at anode.

B
Reddish brown fumes of bromine at anode and greyish lead at cathode.

C
Blue – black fumes of bromine at anode and black lead at cathode.

D
Dark-red precipitates at cathode and black red at anode.

Solution

During the electrolysis of molten lead bromide, fumes of bromine are formed at anode and those of lead are formed at cathode.
Question 11
1 / -0

Why is the electrolytic cell made of silica during the electrolysis of molten lead bromide?

A
Because it is non-reactive

B
Because it is a good conductor of electricity

C
Because it helps discharge the ions

D
Because it absorbs the fumes evolved during the process

Solution

The electrolytic cell is made of silica during the electrolysis of molten lead bromide because it is non-reactive. It can withstand high temperature and is almost a non conductor of electricity.
Question 12
1 / -0

Which of the following is preferred as anode to other inert electrodes?

A
Platinum

B
Iron

C
Graphite

D
Silica

Solution

Graphite is preferred as anode to other inert electrodes such as platinum since graphite is unaffected by reactive bromine vapours.
Question 13
1 / -0

Which of the following is called anode mud?

A
Insoluble impurities

B
Thin strips of pure metal

C
Electrode used in the process

D
Electrolyte used in the process

Solution

In electrolytic refining, anode is made from impure metal and cathode is made from pure metal. When electricity is passed, the pure metal present in the anode goes and sticks to the cathode, and the impurities left behind settle down the anode. This is called anode mud.
Question 14
1 / -0

Which metals are used as cathode and anode during electrolysis of sodium metal?

A
Iron as cathode and graphite rod as anode.

B
Sodium as anode and iron as cathode.

C
Graphite rod as cathode and impure sodium as anode.

D
Iron as cathode and lead as anode.

Solution

Iron metal is used as cathode and graphite rod is used as anode during electrolysis of sodium metal.
Question 15
1 / -0

Which of the following is called an electrolyte during electrolysis of fused lead bromide?

A
Silica

B
Molten lead bromide

C
Graphite

D
Iron

Solution

Molten lead bromide acts as the electrolyte during electrolysis of fused lead bromide.
Question 16
1 / -0

What is the amount of sodium produced by passage of 2 moles of electrons in the electrolysis of fused NaCl?

A
23 g

B
46 g

C
11.5 g

D
34.5 g

Solution

We get one mole of sodium for every mole of electrons. Thus, 46 g (2 moles) of sodium is produced when 2 moles of electrons is passed in the electrolysis of fused NaCl.
Question 17
1 / -0

Which of the following is not used in electroplating?

A
Gold

B
Silver

C
Mercury

D
Brass

Solution

Mercury is not used in electroplating as it exists in liquid state at room temperature.
From the given options, nickel is more reactive than hydrogen, as shown in the reactivity series:
Question 18
1 / -0

Which of the following statements about electroplating is incorrect?

A
The article to be electroplated is always placed at the anode.

B
A low current should be passed for a longer period of time.

C
Direct current should be used.

D
The metal to be electroplated has to be periodically replaced.

Solution

Option 1 is incorrect as the article to be electroplated is always placed at the cathode.
Question 19
1 / -0

Which of the following processes is used for purifying metals by electrolysis?

A
Electroplating

B
Electrorefining

C
Electrometallurgy

D
Electrodeposition

Solution

Electrorefining is used for purifying metals by electrolysis.
Question 20
1 / -0

Which of the following is more reactive than hydrogen?

A
Gold

B
Mercury

C
Copper

D
Lead

Solution

The reactivity series of metals:

Hence, according to reactivity series, lead is more reactive than hydrogen.

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Chemical Effects of Current Test - 5

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Chemical Effects of Current Test - 5

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Question 1

from a negative electrode to a positive electrode

in both the directions

from a positive electrode to a negative electrode

from a cathode to an anode

Solution

Question 2

SO4-2 < Cl– < I– < OH–

SO4-2 < Cl– < OH– < I–

Cl– < I– < SO4-2 < OH–

Cl– < I– < OH– < SO4-2

Solution

Question 3

PbBr2

CuSO4

H3PO4

CS2

Solution

Question 4

Pb

Ca

Ni

Al

Solution

Question 5

Both (1) and (2)

Both (1) and (3)

Only (1)

All of the above

Solution

Question 6

Cu2+, H3O+

Cu2+

SO, OH–

OH–

Solution

Question 7

Na+, H3O+

H3O+

Cl–, OH–

OH–

Solution

Question 8

Pt

Au

C

Al

Solution

Question 9

To enhance the conductivity of the electrolyte

To enhance the hydrolysis of the electrolyte

To prevent the colour change of the solution

To prevent the discharge of ions

Solution

Question 10

Reddish brown fumes of bromine at cathode and Greyish lead at anode.

Reddish brown fumes of bromine at anode and greyish lead at cathode.

Blue – black fumes of bromine at anode and black lead at cathode.

Dark-red precipitates at cathode and black red at anode.

Solution

Question 11

Because it is non-reactive

Because it is a good conductor of electricity

Because it helps discharge the ions

Because it absorbs the fumes evolved during the process

Solution

Question 12

Platinum

Iron

Graphite

Silica

Solution

SO₄^-2< Cl^–< I^– < OH^–

SO₄^-2< Cl^– < OH^– < I^–

Cl^– < I^– < SO₄^-2 < OH^–

Cl^– < I^– < OH^– < SO₄^-2

PbBr₂

CuSO₄

H₃PO₄

CS₂

Cu²⁺, H₃O⁺

Cu²⁺

SO, OH^–

OH^–

Na⁺, H₃O⁺

H₃O⁺

Cl^–, OH^–

OH^–