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) , C l2(g) ;   P = HClO4(aq)
4.	R = H2(g) , N2(g) ;  P = NH3(aq)

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

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. $1.75\times {10}^{-5}$ mol L^-1 

2. $2.50\times {10}^{-5}$ mol L^-1 

3. $1.75\times {10}^{-4}$ mol L^-1 

4. $2.50\times {10}^{-4}$ mol L^-1 

On electrolysis of dilute sulphuric acid using Platinum (Pt) electrode, the product obtained at the anode will be:

1. Oxygen gas

2. ${\mathrm{H}}_2\mathrm{S}$ gas

3. ${\mathrm{SO}}_2$ gas

4. Hydrogen gas 

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

Find the emf of the cell in which the following reaction takes place at 298 K:
\(\mathrm{Ni}(\mathrm{s})+2 \mathrm{Ag}^{+}(0.001 \mathrm{M}) \rightarrow \mathrm{Ni}^{2+}(0.001 \mathrm{M})+2 \mathrm{Ag}(\mathrm{s}) \)
\( \small{\text { (Given that } \mathrm{E}_{\text {cell }}^{\circ}=10.5 \mathrm{~V}, \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \text { at } \ 298 \mathrm{~K})} \)
1. 1.05 V
2. 1.0385 V 
3. 1.385 V
4. 0.9615 V 

The three cells with their \(E^\circ_{\text{(cell)}}\) values are given below:

\(\land^o_m\) for NaCl, HCl and \(CH_3COONa \) are 126.4, 425.9, and 91.05 S cm² mol^-1 respectively. If the conductivity of 0.001028 mol L^-1 acetic acid solution is \(4.95 \times 10^{-5} S ~cm^{-1} \), the degree of dissociation of the acetic acid solution is-

Two half cell reactions are given below:
\(\begin{aligned} &\mathrm{Co}^{3+}+e^{-} \rightarrow \mathrm{Co}^{2+}, \mathrm{E}_{\mathrm{Co}^{2+} / \mathrm{Co}^{3+}}^{\circ}=-1.81 \mathrm{~V} \\ &2 \mathrm{Al}^{3+}+6 e^{-} \rightarrow 2 \mathrm{Al}(\mathrm{s}), \mathrm{E}_{\mathrm{Al} / \mathrm{Al}^{3+}}^{\circ}=+1.66 \mathrm{~V} \end{aligned} \)
The standard EMF of a cell with feasible redox reaction will be: