Mg(s) + 2Ag⁺(0.0001M) → Mg²⁺(0.130M) + 2Ag(s)

If  E^Ɵ(cell) for the above mentioned cell is 3.17 V, then E(cell) value will be-

(log 13=1.1)

1. 2.87 V
2. 3.08 V
3. 2.96 V
4. 2.68 V

Resistance of a conductivity cell filled with 0.1 mol L^–1 KCl solution is 100 Ω. If the resistance of the same cell when filled with 0.02 mol L^–1 KCl solution is 520 Ω. The conductivity of 0.1 mol L^–1 KCl solution is 1.29 S/m. The molar conductivity of 0.02 mol L^–1 KCl solution is-

1. 134 S cm² mol^–1
2. 124 S cm² mol^–1
3. 144 S cm² mol^–1
4. 154 S cm² mol^–1

Aluminium oxide may be electrolysed at 1000 °C to furnish aluminium metal.
The cathode reaction is  Al³⁺ + 3e^- → Al.
To prepare 5.12 kg of aluminium metal by this method would require:
(Atomic mass = 27 amu; 1 faraday=96,500 Coulombs)

1. 5.49×10¹ C of electricity
2. 5.49×10⁴ C of electricity
3. 1.83×10⁷ C of electricity
4. 5.49×10⁷ C of electricity

Consider the following  reaction:

$\frac{\mathrm{}}{}$\(\frac{4}{3} \mathrm{Al}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g}) \rightarrow \frac{2}{3} \mathrm{Al}_2 \mathrm{O}_3(\mathrm{~s})\), $∆\mathrm{G}=-827$ $\mathrm{KJ}$ ${\mathrm{mol}}^{-1}$.
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 value of E⁰ cell for the following reaction is:
\(Cu^{2+}+ Sn^{2+}\to Cu +Sn^{4+ } \)

(Given, equilibrium constant is 10⁶)

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

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