A device that converts the energy of combustion of fuels, like hydrogen and methane, directly into electrical energy is known as: 

1.	Fuel cell.	2.	Electrolytic cell.
3.	Dynamo.	4.	Ni-Cd cell.

When 0.1 mol MnO₄^2– is oxidized, the quantity of electricity required to completely oxidise MnO₄^2– to MnO₄^– is:

1. 96500 C

2. 2 × 96500 C

3. 9650 C

4. 96.50 C

A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of pH = 10 and by passing hydrogen gas around the platinum wire at one atm pressure. The oxidation potential of the electrode would be: 

The cell potential will be:

For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25 °C. The value of standard Gibbs energy, ΔG^o will be: 

(F = 96500 C mol^-1)

1. -89.0 kJ

2. -89.0 J

3. -44.5 kJ

4. -98.0 kJ

Al₂O₃ is reduced by electrolysis at low potentials and high currents. If 4.0 x 10⁴ A of current is passed through molten Al₂O₃ for 6 hours, the mass of aluminum produced is: (Assume 100 % current efficiency, the atomic mass of Al = 27 g mol^-1)

The molar conductance of $\frac{\mathrm{M}}{32}$ solution of a weak monobasic acid is 8.0 ohm^-1 cm² and at infinite dilution is 400 ohm^-1 cm². The dissociation constant of this acid is: 

Given:
(i) ${\mathrm{Cu}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Cu}$    E^o = 0.337 V 
(ii) ${\mathrm{Cu}}^{2+}+{\mathrm{e}}^{-}\to {\mathrm{Cu}}^{+}$  E^o = 0.153 V 
Electrode potential, E^o for the reaction, 
${\mathrm{Cu}}^{+}+{\mathrm{e}}^{-}\to \mathrm{Cu}$, will be: 

1. 0.52 V

2. 0.90 V

3. 0.30 V

4. 0.38 V

Kohlrausch's law states that at: