Electrochemistry MCQ | Questions – Paper 2


Topic: Electrochemistry, Test No.: 02, Total MCQs: 15

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Question 1

Li occupies higher position in the electrochemical series of metals as compared to Cu since [West Bengal CET 2012]

A

the standard reduction potential of Li+/Li is lower than that of Cu2+/Cu

B

the standard reduction potential of Cu2+/Cu is lower than that of Li+/Li

C

the standard oxidation potential of Li/Li+ is lower than that of Cu/Cu2+

D

Li is smaller in size as compared to Cu

Question 2

The standard reduction potential Eo for half reactions are

Zn = Zn2+ + Ze            Eo = +0.76 V

Fe = Fe2+ + Ze            Eo = + 0.41 V

The EMF of the cell reaction Fe2+ + Zn = Zn2+ + Fe is [West Bengal JEE 2011]

A
– 0.35 V
B
+ 0.35
C
+ 1.17 V
D
– 1.17 V
Question 3

Consider the following cell reaction:

2Fe(s) + O2(g) + 4H+(aq) ® 2Fe2+(aq) + 2H2O(l); E° = 1.67 V

At [Fe2+] = 10–3 M, P(O2) = 0.1 atm and pH = 3, the cell potential at 25°C is [IIT JEE 2011]

A
1.47 V
B
1.77 V
C
1.87 V
D
1.57 V
Question 4

The reduction potential of hydrogen half-cell will be negative if: [AIEEE 2011]

A

p(H2) = 2 atm and [H+] = 2.0 M

B

p(H2) = 1 atm and [H+] = 2.0 M

C

p(H2) = 1 atm and [H+] = 1.0 M

D

p(H2) = 2 atm and [H+] = 1.0 M

Question 5

Given . The value of standard electrode potential for the change, + e- ® Fe2+ will be [AIEEE 2009]

A
–0.072 V
B
0.385 V
C
0.770 V
D
–0.270 V
Question 6

Hydrogen gas is not liberated when the following metal is added to dil. HCl. [Karnataka CET 2008]

A
Mg
B
Sn
C
Ag
D
Zn
Question 7

Electrolysis of dilute aqueous NaCl solution was carried out by passing 10 milliampere current. The time required to liberate 0.01 mol of H2 gas at the cathode is (1 Faraday = 96500 C mol-1) [IIT JEE 2008]

A

9.65 ´ 104 s

B

19.3 ´ 104 s

C

28.95 ´ 104 s

D

38.6 ´ 104 s

Question 8

Given = -0.42 V

The potential for the cell

Cr / Cr3+ (0.1 M) || Fe2+ (0.01 M) | Fe is [AIEEE 2008]

A
–0.26 V
B
0.26 V
C
0.339 V
D
–0.339 V
Question 9

Given the data at 25°C,

Ag + I AgI + e ; Eo = 0.152 V

Ag Ag+ + e; Eo = −0.800 V

What is the value of log Ksp for AgI?

 [AIEEE 2006]

A
–8.12
B
+8.612
C
–37.83
D
–16.13
Question 10

The hydrogen electrode is dipped in a solution of pH 3 at 25°C. The potential would be (the value of 2.303 RT/F is 0.059 V) [Karnataka CET 2005]

A
0.177 V
B
0.087 V
C
0.059 V
D
–0.177 V
Question 11

The rusting of iron takes place as follows

2H+ + 2e- + O2 ® H2O(l); E° = +1.23 V

Fe2+ + 2e- ® Fe(s); E° = -0.44 V

Calculate ΔG° for the net process [IIT JEE 2005]

A

-322 kJ mol-1

B

-161 kJ mol-1

C

-152 kJ mol-1

D

-76 kJ mol-1

Question 12

Electrolyte

KCl

KNO3

 HCl

NaOAc

NaCl

L¥(S cm2mol-1)

149.9

145

426.2

91

126.5

Calculate using appropriate molar conductances of the electrolytes listed above at infinite dilution in H2O at 25°C [AIEEE 2005]

A
517.2
B
552.7
C
390.7
D
217.5
Question 13

Zn | Zn2+ (a = 0.1M) || Fe2+ (a = 0.01M)|Fe. The emf of the above cell is 0.2905 V. Equilibrium constant for the cell reaction is [IIT JEE 2004]

A
100.32/0.0591
B
100.32/0.0295
C
100.26/0.0295
D
e0.32/0.295
Question 14

In a cell that utilizes the reaction

Zn(s) + 2H+ (aq) ® Zn2+ (aq) + H2(g) addition of H2SO4 to cathode compartment, will: [AIEEE 2004]

A
lower the E and shift equilibrium to the left
B
lower the E and shift the equilibrium to the right
C
increase the E and shift the equilibrium to the right
D
increase the E and shift the equilibrium to the left
Question 15

The values of Cr, Mn, Fe and Co are -0.41, + 1.57, +0.77 and +1.97 V respectively.

For which one of these metals the change in oxidation state from +2 to +3 is easiest? [AIEEE 2004]

A
Cr
B
Mn
C
Fe
D
Co
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