Electrochemistry Test

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Electrochemistry Test - 4

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Weekly Quiz Competition

Question 1
1 / -0.25

Emf of the cell

Mg (s) | Mg²⁺ (0.001M) || Cu²⁺ (0.0001M) | Cu(s) at 298 K is

A
2.68 V

B
2.50 V

C
2.60 V

D
2.38 V

Solution
Question 2
1 / -0.25

Emf of the cell

Fe (s) | Fe²⁺ (0.001 M)|| H⁺ (1M)|H₂ (g) (1 bar) |Pt(s) at 298 K is

(Given: E^o_cell = +0.44 V)

A
0.53 V

B
0.55 V

C
0.50 V

D
0.48 V

Solution

⇒E_cell = 0.44 + 0.089V

⇒Ecell = 0.53V
Question 3
1 / -0.25

The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm^-1 . Calculate its molar conductivity.

A
120 S cm² mol^{-1 ×}

B
124 S cm² mol^-1

C
129 S cm² mol^-1

D
122 S cm² mol^-1

Solution

k (Conductivity) =0.0248 Scm⁻¹ , C (molarity) = 0.20 M, T (temperature) = 298 K
Λm = ? (molar conductivity)

Λm = (1000 ×k ) / C = (1000 ×0.0248) / 0.20 = 124 S cm² mol⁻¹

The molar conductivity is 124 S cm² mol⁻¹
Question 4
1 / -0.25

The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 Ω. What is the cell constant if conductivity of 0.001M KCl solution at 298 K is 0.146 ×10^-3 S cm^-1 .

A
0.219 cm^-1

B
0.239 cm^-1

C
0.229 cm^-1

D
0.209 cm^-1

Solution

Κ= G x cell constant and G = 1/R.
Question 5
1 / -0.25

How much charge is required for the reduction of 1 mol of Al³⁺ to Al?

A
3F

B
4F

C
5F

D
6F

Solution

For reduction of 1 mol of Al³⁺ to Al, 3 mol of electrons are required so total charge will be 3F.
Question 6
1 / -0.25

How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten Al _2^O₃ ?

A
4.84F

B
4.44F

C
4.54F

D
4.64F

Solution
Question 7
1 / -0.25

Three electrolytic cells A, B, C containing solutions of ZnSO₄ , AgNO₃ and CuSO₄ , respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell. How long did the current flow? What mass of copper and zinc were deposited?

A
16.20 min, Copper 0.487g, Zinc 0.437 g

B
15.10 min, Copper 0.452g, Zinc 0.437 g

C
14.40 min, Copper 0.427g, Zinc 0.437 g

D
13.10 min, Copper 0.403g, Zinc 0.437 g

Solution

And mass of Zn and Cu deposited will be in ratio of their equivalent mass.
Question 8
1 / -0.25

The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

A
10¹⁵

B
10 ³⁰

C
10²⁵

D
10²⁰

Solution
Question 9
1 / -0.25

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

A
increase in number of ions

B
increase in both i.e. number of ions and ionic mobility of ions

C
100% ionization of electrolyte at normal dilution

D
increase in ionic mobility of ions

Solution

Equivalent conductance increases on dilution for a strong electrolyte because of increase in mobility of ions.
Question 10
1 / -0.25

For the reduction of silver ions with copper metal the standard cell potential was found to be +0.46V at 25 °C. The value of standard Gibbs energy, ΔG °wll be (F = 96500 C mol^-1 )

A
-89.0 kJ

B
-44.5 kJ

C
-98.0 kJ

D
-89.0 J

Solution
Question 11
1 / -0.25

Which of the following electrolytic solutions has the least specific conductance?

A
0.002 N

B
2 N

C
0.02 N

D
0.2 N

Solution

Specific conductance decreases with dilution because of decrease in the number of ions per unit volume.
Question 12
1 / -0.25

The highest electrical conductivity of the following aqueous solutions is of

A
0.1 M fluoroacetic acid

B
0.1 M acetic acid

C
0.1 M difluoroacetic acid

D
0.1 M chloroacetic acid

Solution

Acidity increases on attaching electron withdrawing group because of stability of conjugate base.
Question 13
1 / -0.25

The standard electrode potential is measured by

A
Galvanometer

B
Voltmeter

C
Electrometer

D
Pyrometer

Solution

Voltmeter measures the potential.
Question 14
1 / -0.25

When KMnO4 acts as an oxidizing agent and ultimately forms MnO₄^2- , MnO₂ , Mn₂ O₃ , and Mn²⁺ then the number of electrons transferred in each case

A
1, 3, 4, 5

B
4, 3, 1, 5

C
3, 5, 7, 1

D
1, 5, 3, 7

Solution

No. of electrons = change in oxidation number of active elemnt.
Question 15
1 / -0.25

On the basis of the following E °values, the strongest oxidizing agent is:

A
[Fe(CN)₆ ]^4-

B
Fe²⁺

C
Fe³⁺

D
[Fe(CN)₆ ]^3-
Solution
The strongest oxidizing agent is one having more positive or less negative reduction potential.

For the strongest oxidizing agent, the oxidizing potential should be the least.

Here, the oxidizing potential of Fe⁺² is less than that of [Fe(CN)₆ ]^{4 −} . Therefore, Fe⁺² is a stronger oxidizing agent than [Fe(CN)₆ ]^{4 −} .

Also, the stronger oxidizing agent should easily reduce itself.

Here, Fe⁺³ is easily reduced than Fe⁺² . Therefore, among all the four, Fe⁺³ is the stronger oxidizing agent.

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Electrochemistry Test - 4

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Electrochemistry Test - 4

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Question 1

2.68 V

2.50 V

2.60 V

2.38 V

Solution

Question 2

0.53 V

0.55 V

0.50 V

0.48 V

Solution

Question 3

120 S cm2 mol-1 ×

124 S cm2 mol-1

129 S cm2 mol-1

122 S cm2 mol-1

Solution

Question 4

0.219 cm-1

0.239 cm-1

0.229 cm-1

0.209 cm-1

Solution

Question 5

3F

4F

5F

6F

Solution

Question 6

4.84F

4.44F

4.54F

4.64F

Solution

Question 7

16.20 min, Copper 0.487g, Zinc 0.437 g

15.10 min, Copper 0.452g, Zinc 0.437 g

14.40 min, Copper 0.427g, Zinc 0.437 g

13.10 min, Copper 0.403g, Zinc 0.437 g

Solution

Question 8

1015

10 30

1025

1020

Solution

Question 9

increase in number of ions

increase in both i.e. number of ions and ionic mobility of ions

100% ionization of electrolyte at normal dilution

increase in ionic mobility of ions

Solution

Question 10

-89.0 kJ

-44.5 kJ

-98.0 kJ

-89.0 J

Solution

Question 11

0.002 N

2 N

0.02 N

0.2 N

Solution

Question 12

0.1 M fluoroacetic acid

0.1 M acetic acid

0.1 M difluoroacetic acid

0.1 M chloroacetic acid

Solution

120 S cm² mol^{-1 ×}

124 S cm² mol^-1

129 S cm² mol^-1

122 S cm² mol^-1

0.219 cm^-1

0.239 cm^-1

0.229 cm^-1

0.209 cm^-1

10¹⁵

10 ³⁰

10²⁵

10²⁰

[Fe(CN)₆ ]^4-

Fe²⁺

Fe³⁺

[Fe(CN)₆ ]^3-