Electrochemistry MCQ | Questions – Paper 1

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Topic: Electrochemistry, Test No.: 01, Total MCQs: 15

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Question 1

Resistance of 0.2 M solution of an electrolyte is 50 W. The specific conductance of the solution is 1.3 S m–1. If resistance of the 0.4 M solution of the same electrolyte is 260 W, its molar conductivity is [AIEEE 2011]

A

62.5 S m2 mol–1

B

6250 S m2 mol–1

C

6.25 × 10–4 S m2 mol–1

D

625 × 10–4 S m2 mol–1

Question 2

E1, E2 and E3 are the emf values of the three galvanic cells respectively.

(a)

(b)

(c)

Which one of the following is true? [Karnataka CET 2010]

A

E2 > E3 > E1

B

E3 > E2 > E1

C

E1 > E2 > E3

D

E1 > E3 > E2

Question 3

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 [Karnataka CET 2010]

A

1025

B

1020

C

1015

D

1030

Question 4

9.65 C of electric current is passed through fused anhydrous magnesium chloride. The magnesium metal thus, obtained is completely converted into a Grignard reagent. The number of moles of the Grignard reagent obtained is ______. [Karnataka CET 2010]

A

5 ´ 10-4

B

1 ´ 10-4

C

5 ´ 10-5

D

1 ´ 10-5

Question 5

The potential of a hydrogen electrode at pH = 10 is [West Bengal JEE 2010]

A
0.59 V
B
0.00 V
C
–0.59 V
D
–0.059 V
Question 6

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to [CBSE AIPMT 2010]

A
increase in both i.e. number of ions and ionic mobility of ions.
B
increase in number of ions
C
increase in ionic mobility of ions
D
100% ionization of electrolyte at normal dilution
Question 7

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) [CBSE AIPMT 2010]

A
–44.5 kJ
B
–98.0 kJ
C
–89.0 kJ
D
–89.0 J
Question 8

The Gibbs energy for the decomposition of Al2O3 at 500°C is as follows:

Al2O3 ®  Al + O2, ΔrG = +966 kJ mol-1

The potential difference needed for electrolytic reduction of Al2O3 at 500°C is at least: [AIEEE 2010]

A
2.5 V
B
5.0 V
C
4.5 V
D
3.0 V
Question 9

Which of the following electrolytic solutions has the least specific conductance? [Karnataka CET 2008]

A
0.02 N
B
0.2 N
C
2 N
D
0.002 N
Question 10

The equivalent conductances of two strong electrolytes at infinite dilution in H2O (where ions move freely through a solution) at 25°C are given below:

= 91.0 S cm2 / equiv

= 426.2 S cm2 / equiv

What additional information/quantity one needs to calculate L° of an aqueous solution of acetic acid? [AIEEE 2007]

A

L° of NaCl

B

L° of CH3 COOK

C

The limiting equivalent conductance of H+

D

L° of chloroacetic acid (ClCH2COOH)

Question 11

The molar conductivities at infinite dilution in water at 25°C are 91.0 and 426.2 S cm2/mol respectively. To calculate , the additional value required is [AIEEE 2006]

A

B

C

D

Question 12

Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1 M is 100 Ω. The conductivity of this solution is 1.29 S m–1. Resistance of the same cell when filled with 0.2 M of the same solution is 520 Ω. The molar conductivity of 0.02 M solution of the electrolyte will be [AIEEE 2006]

A

124 × 10–4 S m2 mol–1

B

1240 × 10–4 S m2 mol–1

C

1.24 × 10–4 S m2 mol–1

D

12.4 × 10–4 S m2 mol–1

Question 13

The highest electrical conductivity of the following aqueous solutions is of [AIEEE 2005]

A
0.1 M acetic acid
B
0.1 M chloroacetic acid
C
0.1 M fluoroacetic acid
D
0.1 M difluoroacetic acid
Question 14

Saturated solution of KNO3 is used to make 'salt bridge' because [IIT JEE 2001]

A

velocity of K+ is greater than that of NO3-

B

velocity of NO3- is greater than that of K+

C

velocity of both K+ and NO3- are nearly the same

D

KNO3 is highly soluble in water

Question 15

For the electrochemical cell:

M | M+ ||X- | X, E° [M+ | M] = 0.44 V and

E° [X | X-] = 0.33 V.

From the data one can deduce that [IIT JEE 2000]

A

M + X ® M+ + X- is the spontaneous reaction

B

M+ + X- ® M + X is the spontaneous reaction

C

Ecell = 0.77 V

D

Ecell = -0.77 V

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