The molar conductance of NaCl, HCI, and CH3COONa at infinite dilution are 126.45, 426.16, and 91.0 S cm mol-1 respectively. The molar conductance of CH3COOH at infinite dilution will be:

1. 698.28 S cm2 mol-1

2. 540.48 S cm2 mol-1

3. 201.28 S cm2 mol-1

4. 390.71 S cm2 mol-1

  

Subtopic:   Kohlrausch Law & Cell Constant |
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The molar conductivity of 0.007 M acetic acid is 20 S cm2 mol-1. The dissociation constant of acetic acid is -

(\(\mathrm{\Lambda_{H^{+}}^{o} \ = \ 350 \ S \ cm^{2} \ mol^{-1} }\))
(\(\mathrm{\mathrm{\Lambda_{CH_{3}COO^{-}}^{o} \ = \ 50 \ S \ cm^{2} \ mol^{-1} }}\))

1. 1.75×10-5 mol L-1 

2. 2.50×10-5 mol L-1 

3. 1.75×10-4 mol L-1 

4. 2.50×10-4 mol L-1 

Subtopic:   Kohlrausch Law & Cell Constant |
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The number of Faradays (F) required to produce 20 g of calcium from molten CaCl2 (Atomic mass of Ca=40 g mol-1) is:

1. 2

2. 3

3. 4

4. 1

Subtopic:  Faraday’s Law of Electrolysis |
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On electrolysis of dilute sulphuric acid using Platinum (Pt) electrode, the product obtained at the anode will be:

1. Oxygen gas

2. H2S gas

3. SO2 gas

4. Hydrogen gas 

Subtopic:  Electrolytic & Electrochemical Cell |
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In a typical fuel cell, the reactants (R) and products (P) are :-

1. R=H2(g), O2(g); P=H2O2(l)

2. R=H2(g), O2(g); P=H2O(l)

3. R=H2(g), O2(g), Cl2(g); P=HClO4(aq)

4. R=H2(g), N2(g); P=NH3(aq)

Subtopic:  Batteries & Salt Bridge |
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For the cell reaction \(2Fe^{3+}(aq) \ + \ 2I^{-}(aq)\rightarrow 2Fe^{2+}(aq) \ + \ I_{2}(aq)\)

\(E_{cell}^{o} \ = \ 0.24 \ V\) at 298 K. The standard Gibbs energy ∆rG of the cell reaction is:

[Given: 96500 C mol-1]

1.  23.16 kJ mol-1

2.  -46.32 kJ mol-1

3.  -23.16 kJ mol-1

4.  46.32 kJ mol-1

Subtopic:  Relation between Emf, G, Kc & pH |
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For a cell involving one electron Ecell=0.59 V at 298 K. The equilibrium constant for the cell reaction is: Given that 2.303 RTF=0.059 V at T=298 K

1.  1.0×1030

2.  1.0×102

3.  1.0×105

4.  1.0×1010

Subtopic:  Relation between Emf, G, Kc & pH |
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Limiting molar conductivities, for the given solutions, are :

λm0(H2SO4)x cm2 mol-1

λm0(K2SO4)y cm2 mol-1

λm0(CH3COOK)z cm2 mol-1

From the data given above, it can be concluded that \(\lambda_m^0 \) in (\(S\ cm^2\ mol^{-1}\)) for CH3COOH will be :

1. 2z

2. 

3. x - y + z

4. (x-y)z

Subtopic:  Conductance & Conductivity |
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Consider the change in oxidation state of Bromine corresponding to different emf values as shown in the diagram below: 
 
Then the species undergoing disproportionation is:-

1. 

2. 

3. 

4. HBrO

Subtopic:  Electrode & Electrode Potential |
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In the electrochemical cell: 
  Zn | ZnSO4 (0.01 M) || CuSO4(1.0 M) | Cu, the emf of this Daniel cell is E1. When the concentration of ZnSO4 is changed to 1.0 M and that of CuSO4 is changed to 0.01 M, the emf changes to E2. From the following, which one is the relationship between E1 and E2
(Given, \(\frac{RT}{F}\) = 0.059)

1. E1<E2

2. E1>E2

3. E2=0E1

4. E1=E2

Subtopic:  Electrode & Electrode Potential | Nernst Equation |
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