The molar conductivity of a 0.5 mol/dm³ solution of AgNO₃ with electrolytic conductivity of 5.76 × 10^–3 S cm^–1 at 298 K is:
1. 11.5 S cm²/mol
2. 21.5 S cm²/mol
3. 31.5 S cm²/mol
4. 41.5 S cm²/mol

The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is:

(Charge on electron = 1.60 × 10^–19 C)

1.  $6\times {10}^{23}$

2.  $6\times {10}^{20}$

3.  $3.75\times {10}^{20}$

4.  $7.48\times {10}^{20}$

The pressure of H₂ required to make the potential of H₂ - electrode zero in pure water at 298 K is:

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

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)