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  number of electrons involved in the deposition of 63.5 g of Cu from a solution of $CuS{O}_4$ is:

1 $6.022$ $\times$ ${10}^{23}$ $$

2 $3.011$ $\times$ ${10}^{23}$ $$

3 $12.044$ $\times$ ${10}^{23}$ $$

4 $$ $6.022$ $\times$ ${10}^{22}$

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

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

For the cell, Ti/Ti⁺(0.001M)||Cu²⁺(0.1M)|Cu, ${\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}$ $$at

25 $°$C is 0.83 V. E_cell can be increased :

1. By increasing [Cu²⁺]

2. By increasing [Ti⁺]

3. By decreasing [Cu²⁺]

4. None of the above.

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 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

The same amount of electricity was passed through two cells containing molten Al₂O₃ and molten NaCl. If 1.8 g of Al were liberated in one cell, the amount of Na liberated in the other cell is:

1. 4.6 g

2. 2.3 g

3. 6.4 g

4. 3.2 g