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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Given below are half-cell reactions:

\(\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}, \\ \mathrm{E}_{\mathrm{Mn}^{2+}}^{\circ} / \mathrm{MnO}_{4}^{-}=-1.510 \mathrm{~V} \\ \frac{1}{2} \mathrm{O}_{2}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{H}_{2} \mathrm{O}, \\ \mathrm{E}_{\mathrm{O}_{2} / \mathrm{H}_{2} \mathrm{O}}^{\circ}=+1.223 \mathrm{~V}\)

Will the permanganate ion, \(\mathrm{MnO}_{4}^{-}\) , liberate \(\mathrm{O}_{2}\) from water in the presence of an acid?

1. No, because \(\mathrm{E}_{\text {cell }}^{\circ}=-2.733 \mathrm{~V}\)
2. Yes, because \(\mathrm{E}_{\text {cell }}^{\circ}=+0.287 \mathrm{~V}\)
3. No, because \(\mathrm{E}_{\text {cell }}^{\circ}=-0.287 \mathrm{~V}\)
4. Yes, because \(\mathrm{E}_{\text {cell }}^{\circ}=+2.733 \mathrm{~V}\)
Subtopic:  Electrode & Electrode Potential |
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Find the emf of the cell in which the following reaction takes place at 298 K 
\(\begin{aligned} \mathrm{Ni}(\mathrm{s})+2 \mathrm{Ag}^{+}(0.001 \mathrm{M}) \rightarrow \mathrm{Ni}^{2+}(0.001 \mathrm{M})+2 \mathrm{Ag}(\mathrm{s}) \\ \small{\text { (Given that } \mathrm{E}_{\text {cell }}^{\circ}=10.5 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \text { at } \ 298 \mathrm{~K})} \end{aligned}\)
1. 1.05 V 
2. 1.0385 V 
3. 1.385 V 
4. 0.9615 V 

Subtopic:  Nernst Equation |
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