Electrochemistry Test

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Electrochemistry Test - 25

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following is true for electrolytic refining?

A
Pure metal is used at anode and impure metal at cathode

B
Pure metal is used at cathode and impure metal at anode

C
Both can be possible A and B

D
None of these

Solution

Impure metal will release electron hence form anode electrode and pure metal will absorb electron hence it will be posses as cathode electrode.

Pure metal is used as the cathode and impure metal as anode.
Question 2
1 / -0

The electric current in a chemical cell is due to movement of :

A
positive hole charges

B
positive ions only

C
negative ions only

D
positive and negative ions

Solution

An electrolyte solution is formed by mixing an electrolyte in a solvent. The electrolyte on dissolution furnishes ions. The preferred movement of ions under the influence of the electric field is responsible for electric current. Hence, the electric current in a chemical cell is due to the movement of positive and negative ions.

Therefore option D is correct.
Question 3
1 / -0

The internal resistance of a dry cell is of the order of:

A
0.2 to 0.4 Ohm.

B
1 to 1.4 Ohm.

C
2 to 5 Ohm.

D
1 to 15 Ohm.

Solution

In dry-cell battery, the electrolyte is in the form of a paste. And there is no presence of nickel and iron material. Due to that, the internal resistance of the dry is very less. The value is approximately in between 0.2 to 0.4 $$\Omega.$$
Question 4
1 / -0

An example of secondary battery cell is:

A
Edison Alkaline cell.

B
Daniel cell.

C
Lachanche cell.

D
Bunsen cell.

Solution

Voltiac cell, daniel cell, Lachanche cell, Bunsen cell, fuel are some well known example of primary battery cells. Whereas, lead acid cell and edison alkaline cell are two well known example of secondary cells.
Question 5
1 / -0

Molten $$AlCl_3$$ is electrolysed with the current of $$0.5 $$ empere to produced 27 g $$Al$$. Number of Farady used are :

A
$$3$$

B
$$5$$

C
$$6$$

D
None of these

Solution

$$Al^{3+} + 3e^- \rightarrow Al $$
From Faraday's laws of electrolysis, we know that
$$W= \frac{EQ}{96500} $$.
$$ \frac{Q}{96500} =\dfrac {W}{E}$$.
$$E = 27/3 = 9 $$.
$$\frac {Q}{96500} = 27/9 = 3F $$.
Hence option A is the right answer.
Question 6
1 / -0

In electrolysis experiment, after some times, the battery connection is reversed. Then

A
The electrolysis will stop

B
the rate of liberation of material at electrodes will increase

C
the rate of liberation will decrease

D
rate of liberation will remain unchanged

E
more heat will be produced at the electrodes

Solution

Due to the reverse connection of the battery, only the polarities of the electrode change but the electrolysis process continues to take place and the rate of liberation of materials at the electrode will not change.
Question 7
1 / -0

Internal resistance of a battery cell increases with :

A
increase in concentration of electrolyte

B
increase in distance between two electrodes

C
increase in area of the plates inside the electrolyte

D
increase in size of the electrodes

Solution

Internal resistance of a battery cell:
1) increases with increase in distance between two electrodes.
2) decreases with increase in concentration of electrolyte.
3) decreases with increase in area of the plate inside the electrolyte.
4) decreases with increase in size of the electrodes.
Question 8
1 / -0

The electric charge for electrode deposition of 1 g equivalent of a substance is:

A
1 ampere per second.

B
96,500 coulomb per second.

C
1 ampere for 1 hour.

D
charge on 1 mole of electrons.

Solution

Charge on one mole of electrons is equal to one Faraday, so one gram equivalent of a substance will be deposited by one mole of electrons.

1 g equivalent of a substance means one equivalent of substance which have total charge of one mole of electron.
Question 9
1 / -0

The half cell involving the reaction $$Cr_2O_7^{2-} (aq) + 14 H^+ (aq) + 6e \rightarrow 2Cr^{3+} (aq) + 7H_2O$$ can be represented as :

A
$$Pt, H^+ (aq), Cr_2O_7^{2-} (aq)$$

B
$$Pt, H^+ ,Cr^{3+} (aq)$$

C
$$Pt, H_2, Cr_2O_7^{2-} (aq), Cr^{3+} (aq)$$

D
$$Pt, H^+, Cr_2O_7^{2-} (aq), Cr^{3+} (aq)$$

Solution

It is reduction half cell of $$Cr_2O_7^{-2}$$ and is represented as:
$$(Pt), H^+, Cr_2O_7^{2-} (aq), Cr^{3+} (aq)$$
Question 10
1 / -0

In the atmosphere of industrial smog, copper corrodes to form:

A
basic copper carbonate and sulphate

B
copper oxide

C
copper sulphide

D
copper nitrate

Solution

Architectural structures built with copper corrode to give green verdigris (copper carbonate). It can be a mixture of carbonate and sulfate compounds in various amounts, depending upon environmental conditions such as sulfur-containing acid rain.

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Electrochemistry Test - 25

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Electrochemistry Test - 25

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Question 1

Pure metal is used at anode and impure metal at cathode

Pure metal is used at cathode and impure metal at anode

Both can be possible A and B

None of these

Solution

Question 2

positive hole charges

positive ions only

negative ions only

positive and negative ions

Solution

Question 3

0.2 to 0.4 Ohm.

1 to 1.4 Ohm.

2 to 5 Ohm.

1 to 15 Ohm.

Solution

Question 4

Edison Alkaline cell.

Daniel cell.

Lachanche cell.

Bunsen cell.

Solution

Question 5

$$3$$

$$5$$

$$6$$

None of these

Solution

Question 6

The electrolysis will stop

the rate of liberation of material at electrodes will increase

the rate of liberation will decrease

rate of liberation will remain unchanged

more heat will be produced at the electrodes

Solution

Question 7

increase in concentration of electrolyte

increase in distance between two electrodes

increase in area of the plates inside the electrolyte

increase in size of the electrodes

Solution

Question 8

1 ampere per second.

96,500 coulomb per second.

1 ampere for 1 hour.

charge on 1 mole of electrons.

Solution

Question 9

$$Pt, H^+ (aq), Cr_2O_7^{2-} (aq)$$

$$Pt, H^+ ,Cr^{3+} (aq)$$

$$Pt, H_2, Cr_2O_7^{2-} (aq), Cr^{3+} (aq)$$

$$Pt, H^+, Cr_2O_7^{2-} (aq), Cr^{3+} (aq)$$

Solution

Question 10

basic copper carbonate and sulphate

copper oxide

copper sulphide

copper nitrate

Solution

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