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 

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-
1. 0.01233
2. 1.00 
3. 0.1233 
4. 1.233

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:
1. +7.09 V
2. +0.15 V
3. +3.47 V
4. –3.47 V