The number of Faradays (F) required to produce 20 g of calcium from molten CaCl₂ (Atomic mass of Ca=40 g mol^-1) is:

1. 2

2. 3

3. 4

4. 1

During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is

1. 55 minutes

2. 110 minutes

3. 220 minutes

4. 330 minutes

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

(Charge on electron = 1.60x 10^-19 C)

1.  $6\times {10}^{23}$

2.  $6\times {10}^{20}$

3.  $3.75\times {10}^{20}$

4.  $7.48\times {10}^{20}$

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 x 96500 C

3. 9650 C

4. 96.50 C

The weight of silver (at.wt. = 108) displaced by a quantity of electricity which displaces 5600 mL of O₂ at STP will be :

1. 5.4 g

2. 10.8 g

3. 54.0 g

4. 108.0 g

In producing chlorine by electrolysis, 100 kW power at 125 V is being consumed. How much chlorine per minute is liberated (ECE of chlorine is 0.367 X 10-6 kgC^-1)

1.$1.76\times {10}^{-3} kg$

2. $9.67\times {10}^{-3} kg$

3. $17.61\times {10}^{-3} kg$

4. $3.67\times {10}^{-3} kg$

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, what mass of aluminium is produced ?

(Assume 100 % current efficiency, atomic mass of Al = 27 g mol^-1)

1. 9.0 x 10³ g

2. 8.1 X 10⁴ g

3. 2.4 x 10⁵ g

4. 1.3 X 10⁴ g

A steady current of 1.5 A flows through a copper voltmeter for 10 min. If the electrochemical equivalent of copper is 30 × 10^-5 g C^-1, the mass of copper deposited on the electrode will be :

1. 0.40 g

2. 0.50 g

3. 0.67 g

4. 0.27 g