\(Cu(s)|Cu^{+2}(10^{-3} \ M) \ || \ Ag^{+}(10^{-5} \ M)|Ag(s)\)
if \(E_{Cu^{+2}/Cu}^{o} \ = \ +0.34 \ V\), and \(E_{Ag^{+}/Ag}^{o} \ = \ +0.80 \ V\)
E_cell will be: 

1. 0.46 V
2. \(0.46-\frac{RT}{2F}ln10^{7}\)
3. \(0.46+\frac{RT}{2F}ln10^{7}\)
4. \(0.46-\frac{RT}{2F}ln10^{2}\)

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 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.

The correct statement among the following options is: 

The incorrect statement about the solution of electrolytes is:

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

Match Column-I (Types of cell) with Column-II (Characteristics shown by cells) and mark the appropriate option:

Codes:

Given below are two statements: 

In a typical fuel cell, the reactants (R) and products (P) are: 

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

(Given, equilibrium constant is 10⁶)