In the electrochemical cell: 
$\mathrm{Z n   \left|\right. Z n S O_{4}   \left(\right. 0 . 01   M \left.\right)   \left|\right. \left|\right.   C u S O_{4} \left(\right. 1 . 0   M \left.\right)   \left|\right.   C u},$
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. $\mathrm{E_{1} < E_{2}}$

2. $\mathrm{E_{1} > E_{2}}$

3. $\mathrm{E_{2} = 0 \neq E_{1}}$

4. $\mathrm{E_{1} = E_{2}}$

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

The electrode potential for Mg electrode varies according to the equation

$E_{Mg^{2+}/Mg}\ = \ E_{Mg^{2+}/Mg}^{o} \ - \ \frac{0.059}{2}log\frac{1}{[Mg^{2+}]}$ 

The graph of E_{Mg²⁺ / Mg} vs log [Mg²⁺] among the following is:

1.		2.
3.		4.

Consider the following cell reaction 

2Fe(s) + ${\mathrm{O}}_2$(g) + 4${\mathrm{H}}^{+}$(aq) $\to$ 2${\mathrm{Fe}}^{2+}$(aq) + 2${\mathrm{H}}_2\mathrm{O}$(l)

E° = 1.67 V, At [${\mathrm{Fe}}^{2+}$] = 10${}^{-3}$ M, ${\mathrm{P}}_{{\mathrm{O}}_2}$ = 0.1 atm and pH = 3, the cell potential at 25 °C is : 

1. 1.27 V

2. 1.77 V

3. 1.87 V

4. 1.57 V

The value of E⁰ cell for the following reaction is:
$Cu^{2+}+ Sn^{2+}\to Cu +Sn^{4+ }$

(Given, equilibrium constant is 10⁶)

Consider the following  reaction:

$\frac{4}{3} \mathrm{Al}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \frac{2}{3} \mathrm{Al}_2 \mathrm{O}_3(\mathrm{~s})$, $∆\mathrm{G}=-827$ $\mathrm{KJ}$ ${\mathrm{mol}}^{-1}$.
The minimum e.m.f. required to carry out the electrolysis of Al₂O₃ is:
(F = 96500 C mol^–1)

1. 2.14 V

2. 4.28 V

3. 6.42 V

4. 8.56 V

The potential of hydrogen electrode in contact with a solution with pH =10, is:

The most stable oxidized species among the following is: 
$E_{{\mathrm{Cr}_2 \mathrm{O}_7^2}/ \mathrm{Cr}^{3+}}^{o} =1.33 \mathrm{~V} ; E_{\mathrm{Cl}_2 / \mathrm{Cl}^{-}}^{o}=1.36 \mathrm{~V}$
$E_{\mathrm{MnO_{4}}^{-} / \mathrm{Mn}^{2+}}^{o}=1.51 \mathrm{~V} ; E_{\mathrm{Cr}^{3+} / \mathrm{Cr}}^{o}=-0.74 \mathrm{~V}$