The  number of electrons involved in the deposition of 63.5 g of Cu from a solution of CuSO4 is:

6.022 × 1023 

3.011 × 1023 

12.044 × 1023 

 6.022 × 1022

Subtopic:  Faraday’s Law of Electrolysis |
 68%
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Value of m0 for  SrCl2 (strong electrolyte) in water at 25 °C from the data below is:

Conc. (mol/litre)  0.25 1
Ω-cmmol-1 260 250

1. 270 Ω-1 cm2 mol-1                                                     

2. 260 Ω-1 cm2 mol-1 

3. 250 Ω-1 cm2 mol-1                                                    

4. 255 Ω-1 cm2 mol-1 

Subtopic:   Kohlrausch Law & Cell Constant |
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Calculate the energy obtainable from a lead storage battery in which 0.1 mol lead is consumed. Assume a constant concentration of 10.0 M H2 SO4 

(1) 42.8 kJ                                         

(2) 12.8 kJ

(3) 32.3 kJ                                         

(4) 20.2 kJ

Subtopic:  Faraday’s Law of Electrolysis |
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Adiponitrile is manufactured electrolytically from acrylonitrile CH2= CHCN  CN  (CH2 )4  CH

How many kg of adiponitrile (molecular mass = 108) is produced in 9.65 hr using a current of 3750 A with 80% efficiency?

(1) 30 kg                                               

(2) 58 kg

(3) 60 kg                                               

(4) 80 kg

Subtopic:  Faraday’s Law of Electrolysis |
 66%
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A certain metal salt solutions is electrolysed in series with a silver coulometer. The weights of silver and the metal deposited are 0.5094 g and 0.2653 g. Calculate the valency of the metal if its atomic weight is nearly that of silver. 

(1) 1                                                 

(2) 2

(3) 3                                                 

(4) 4

Subtopic:  Faraday’s Law of Electrolysis |
 79%
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The temperature coefficient, of the emf is dεdT= – 0.00065 volt. deg-1 for the cell Cd|CdCl21m| AgClsAg at 25°C. Calculate the entropy change S298K,  for the cell reaction,Cd + 2AgCl Cd++ + 2Cl+ 2Ag

(1)  105.5 JK-1   

(2)  150.2 JK-1

(3)  75.5 JK-1

 (4)  125.5 JK-1

Subtopic:  Electrode & Electrode Potential |
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The reduction potential of a half-cell consisting of a Pt electrode immersed in 1.5 M Fe2+and 0.015 M Fe3+ solution at 25°C is EFe+3, Fe+2°=+0.770 v.

(1) 0.652 V                                                   

(2) 0.88 V

(3) 0.710 V                                                   

(4) 0.850 V

Subtopic:  Nernst Equation |
 59%
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In a concentration cell, Zn/Zn2+ (1.0 M) || Zn2+ (0.15 M)/Zn as the cell discharges,

(1) reaction proceeds to the right

(2) the two solutions approach each other in concentration

(3) no reaction takes place

(4) water gets decomposed

Subtopic:  Electrode & Electrode Potential |
 57%
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In a half-cell containing [Tl3+] = 0.1 M and [Tl+ ] = 0.01 M, the cell potential is – 1.2496 V for the reaction Tl+ Tl3+ + 2e-  The standard reduction potential of the Tl+ /Tl3+ couple at 25°C is

(1) 1.44 V                                          

(2) 0.61 V

(3) 2.44 V                                          

(4) 1.22 V

Subtopic:  Nernst Equation |
 73%
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Given cell: 

Pt(s)|H2(g)(P = 1 atm)| CH3COOH(0.1 M), HCl(0.1 M) || KCl(aq)|Hg2Cl2(s)|Hg

EMF of the cell is found to be 0.045 V at 298 K and the temperature coefficient is 3.4×10-4 V K-1. The cell entropy change of the following cell is : 

[Given Ka CH3COOH = 10-5  M]

1. 70.8 J K−1 mol−1                      

2. 65.2 J K−1 mol−1

3. 79.2 J K−1 mol−1                  

4. 83.5 J K−1 mol−1

Subtopic:  Relation between Emf, G, Kc & pH |
 62%
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