Nernst Equation (Electrochemistry) MCQs for CSIR NET GATE - ChemContent

Vijay Ishwar
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Chapter: Electrochemistry
Topic: Nernst Equation
Content: MCQ Questions & Solutions
Source: CSIR NET, GATE etc. Exams

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Quiz                        PDF

Q1. Given:

A. Fe(OH)2(s) + 2e- Fe(s) + 2OH-(aq); Eº = -0.877 V
B. Al3+(aq) + 3e-
Al(s); Eº = -1.66
C. AgBr(aq) + e- Ag(s) + Br-(aq); Eº = 0.071 V

The overall reaction for the cells in the direction of spontaneous change would be

[NET June 2014]

(a)  Cell with A and B : Fe Reduced
 Cell with A and C : Fe Reduced

(b)  Cell with A and B : Fe Reduced
 Cell with A and C : Fe Oxidized

(c)  Cell with A and B : Fe Oxidized
 Cell with A and C : Fe Oxidized

(d)  Cell with A and B : Fe Oxidized
 Cell with A and C : Fe Reduced

Q2. For the cell reaction, Sn(s) + Sn4+(aq) 2Sn2+(aq), separate electrode reactions would be written with the respective standard electrode potential data at 25ºC as

Sn4+(aq) + 2e- Sn2+(aq); Eº = +0.15 V

Sn2+(aq) + 2e- Sn(s); Eº = -0.14 V

When RT/F is given as 25.7 mV, logarithm of the equilibrium constant (ln K) is

[NET Dec 2014]

    (a)  22.6
(b)  226
(c)  2.26
(d)  2.26 x 10-1

Q3. Fuel cells provide clean electrical energy to a variety of applications including automobiles and stationary power sources. Normally hydrogen combines with oxygen to give electrical energy and water. If we use butane instead of hydrogen at 1.0 bar and 298 K, the following reaction occurs:

C4H10(g) + 13/2 O2(g) 4 CO2(g) + 5 H2O(l)

If the change in Gibbs free energy of this reaction is 2746.06 KJmol-1, involving 26 electrons, its open circuit voltage is

[NET Dec 2014]

    (a) 1.55 V
(b)  1.09 V
(c)  3.15 V
(d)  2.06 V

Q4. Dominant contribution to the escaping tendency of a charged particle with uniform concentration in a phase, depends on

[NET June 2015]

    (a)  chemical potential of that phase
(b)  electric potential of that phase
(c)  thermal energy of that phase
(d)  gravitational potential of that phase

Q5. The correct ΔG for the cell reaction involving steps

Zn(s) Zn2+(aq) + 2e-

Cu2+(aq) + 2e- Cu(s) is

[NET June 2015]

Q6. The temperature dependence of an electrochemical cell potential is

[NET June 2015]

    (a)  ΔG/nFT
(b)  ΔH/nF
(c)  ΔS/nF
(d)  ΔS/nFT

Q7. Conductometric titration of a strong acid with a strong alkali (MOH) shows linear fall of conductance up to neutralization point because of

[NET June 2015]

    (a)  formation of water
(b)  Increase in alkali concentration
(c)  faster moving H+ being replaced by slower moving M+
(d)  neutralization of acid

Q8. Given that E°(Cl2|Cl-) = 1.35 V and Ksp (AgCl) = 10-10 at 25°C, E° corresponding to the electrode reaction

1/2 Cl2(g) + Ag+(solution) + e- AgCl(s)

is [2.303RT/F = 0.06 V]

[NET Dec 2015]

    (a)  0.75 V
(b)  1.05 V
(c)  1.65 V
(d)  1.95 V

Q9. The standard EMF of the cell

Pt, H2(g) | HCl(solution) || AgCl(s), Ag(s)

[NET Dec 2015]

    (a)  increase with T
(b)  decrease with T
(c)  remains unchanged with T
(d)  decreases with HCl

Q10. The standard electrode potential E° at a fixed temperature and in a given medium is dependent on

[NET Dec 2016]

    (a)  only on electrode composition
(b)  the electrode composition and the extent of the reaction
(c)  the extent of the electrode reaction only
(d)  the electrode reaction and the electrode composition

Q11. On titrating conductometrically a NaOH solution with a mixture of HCl and CH3COOH solutions, plot the volume of mixed acid added (b) in y-axis against the conductance (a) in x-axis is expected to look like

[NET June 2016]

Q12. The ionic mobilities of NH4+ and HCO3- are 6 x 10-4 V-1s-1 and 5 x 10-4 V-1s-1 respectively. The transport numbers of NH4+ and HCO3- are, respectively

[NET Dec 2016]

    (a)  0.545 and 0.455
(b)  0.455 and 0.545
(c)  0.090 and 0.910
(d)  0.910 and 0.090

Q13. Given, 

    (i) Zn + 4 NH3 Zn(NH3)42+ + 2e-; Eº = 1.03 V
    (ii) Zn Zn2+ + 2e-; Eº = 0.763 V

The formation constant of the complex [Zn(NH3)42+] is approximately
(2.303 RT/F = 0.0591)

[NET Dec 2016]

    (a)  1 x 105
(b)  1 x 107
(c)  1 x 109
(d)  1 x 1012

Answer Key

Q1.b Q2.a Q3.b Q4.b Q5.d Q6.c Q7.c Q8.d Q9.b Q10.d Q11.c Q12.a Q13.c

Detailed Solutions [Click Here]

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